Flame tests using cotton buds DSCN0349 Nigel Baldwin 2024-10-23 | Flame tests using cotton buds DSCN0349
Aspirin hydrolysis Nigel Baldwin 2023-06-26 | High School ChemistryA level Chemistry practical to produce an organic solid and purify it.One required practical on the A level Chemistry syllabus that is widely used is the production of aspirin by the reaction of 2-hydroxybenzoic acid with ethanoic anhydride.But, what to do if ethanoic anhydride is banned in your location?One possibility is to do a hydrolysis of aspirin, essentially the reverse of the above mentioned reaction.In this video clip 6 aspirin tablets and 100ml of sodium hydroxide, 0.4M are used. The reaction was stirred overnight at room temperature, around 26 C.The next day the reaction mixture was acidified using 25ml of hydrochloric acid, 2M. The product of the reaction precipitated out and was removed by filtration under reduced pressure.Next steps, not shown in the video clip, are to dry the filtered solid and then recrystallise from ethanol.In another experiment, the precipitated solid was allowed to dry over the weekend. It was then dissolved in the minimum volume of hot ethanol, filtered and allowed to crystallise. A sample from this procedure had a melting point within 1 C of commercial 2-hydroxybenzoic acid in the school chemical store.Recrystallised solid 149 CChemical store 2-hydroxybenzoic acid 150 CBoth of these values recorded by A level chemistry students in the school laboratory are below the accepted literature value.e.g. Melting point of 2-hydroxybenzoic acid 158.6 C Wikipediaen.wikipedia.org/wiki/Salicylic_acidUnfortunately, we were unable to carry out a thin layer chromatography experiment to investigate the purity of the hydrolysis product further.Thanks to Dr Gavan Cooke for operating the vacuum pump for reduced pressure filtration using a Buchner funnel seen at the end of the video clip.If we were to repeat the experiment we would acidify the hydrolysis mixture more gradually.KAKW4470
Iron oxide, aluminium and magnesium Nigel Baldwin 2023-06-24 | High School ChemistryWear safety spectacles and carry out behind safety screenBackground video clipA small scale reaction between iron oxide, aluminium powder and magnesium ribbon.See details in the video clip UWFI7062
Microscale Thermite reaction PXL 20230602 052126660 Nigel Baldwin 2023-06-04 | High School ChemistryMicroscale Thermite reactionWear safety spectacles and carry out in a fume cupboard or behind perspex safety screens as available.See 9.2(c) Microscale Thermite, page 33 of CLEAPSS Safer chemicals, safer reactions L195 April 2023For the Thermite mixture we used 0.75g of iron (III) oxide mixed with 0.25g aluminium powderWe found the aluminium powder needs to be just that, a fine powder, because the reaction simply did not work with a coarse grain aluminium powder.Also, we used 0.35g to 0.40g of barium nitrate igniter. This fell well below the maximum 0.45g mass of igniter mentioned by CLEAPSS. Since we did not have any magnesium powder we did not add any to the barium nitrate igniter.We didn't have any small filter papers and found paper towel used for drying hands would suffice. A small piece of paper towel was wrapped around the end of a finger, the end of the paper towel twisted off to form a sealed end and then pushed into some sand whilst still on the finger. Pull out your finger whilst easing off the paper and the paper thimble should remain in the sand.A 7 to 8cm length of magnesium ribbon was curled into a spiral, similar to how one might picture a coiled snake with raised head and placed in the paper thimble.The Thermite mixture was dropped on top of the coiled magnesium using a steel spatula. One can use the spatula to pat down the mixture a little if one wishes.The igniter was then dropped on top of the mixture around where the magnesium ribbon snake was raising its head.Finally, the magnesium was lit using a Bunsen burner flame and the result was quite pleasing.
A really nice BZ reaction 20230404 Nigel Baldwin 2023-05-07 | High School ChemistryYou never know what you are going to get with BZ reactions.This one was particularly nice. Unfortunately, I only captured 21 seconds of shaky handheld footage after a Year 9 Chemistry class.
Testing for an alkene IMG 2225 Nigel Baldwin 2023-05-07 | High School ChemistrySafety This experiment should be done in a fume cupboardThe bromine water test is on our IGCSE Chemistry specification as a required practical. And yet the procurement of bromine water can be problematic.A quick substitute for bromine water on a small scale can be improvised using household bleach, 2M hydrochloric acid and potassium bromide solution.Lot's of interesting chemistry to discuss and the bromine generated is decolourised by the addition of an alkene quite nicely.I am sure this has been done many times before.After a discussion with Dr Colin Dickinson
IGCSE Chemistry quiz - identify three gases Nigel Baldwin 2023-02-17 | High School ChemistryIGCSE ChemistryIdentify the three colourless gases in the video clip from their test resultsPlease note that I didn't get any of the chemicals on my hands whilst making the video clip.Thanks to Dr Gavan Cooke for filming this one
Alkali metals in water in 47s Nigel Baldwin 2023-02-16 | High School ChemistryQuick revision clip of the reactions of lithium, sodium and potassium metals in water
Crystals from IGCSE Chemistry class XWOS6653 Nigel Baldwin 2023-02-15 | High School ChemistryIGCSE ChemistryMaking crystalsThree samples of crystals made by IGCSE Chemistry students in lessonsQuestions - What reactants could you use to make these compounds in an IGCSE Chemistry practical class?1 sodium ethanoate2 sodium chloride3 ammonium sulfateIn each case the salts were made in an acid + alkali reaction carried out in a 100ml beaker.Small volumes of the alkali were added to a approximately 20ml of dilute acid using a plastic dropping pipette. The pH change was monitored after each addition of alkali by sampling with a glass stirring rod and spotting onto Universal Indicator paper.Answers1 sodium hydroxide and ethanoic acid2 sodium hydroxide and hydrochloric acid3 dilute aqueous ammonia and sulphuric acid
Magnesium plus sulphuric acid NPGF8193 Nigel Baldwin 2023-02-14 | High School ChemistryIGCSE ChemistryMaking a saltMethod 1 acid + metal = salt + hydrogenAn excess of magnesium metal is added to a small volume of sulfuric acid in a beaker.Magnesium reacts with sulfuric acidQ1 What gas is produced?Q2 What salt is produced?The reaction can be monitored by observing the bubbles of colourless gas produced. However, magnesium also reacts slowly with water producing bubbles of the same colourless gas, so it is just as well to monitor the pH using Universal Indicator paper.The reaction can be stopped by filtering off the excess magnesium metal when the pH reaches 6.Answers to the questions above1 Hydrogen gas2 Magnesium sulphateThe salt produced is usually obtained in it's hydrated form, i.e. it contains water of crsytallisation.Q3 What is the formula of the most commonly encountered hydrated form of magnesium sulfate?AnswerMagnesium heptahydrate MgSO4·7H2O
Limewater and carbon dioxide tests on two scales IMG 1978 Nigel Baldwin 2023-02-13 | High School ChemistryIGCSE ChemistryTesting for carbon dioxide gas using limewaterTraditional apparatus using a delivery tube and smaller scale apparatus using a cut off bulb from a plastic dropping pipetteThe cut off plastic dropping pipette bulbs are easy to wash out and re-use.
Iron III thiocyanate art DGHG7361 Nigel Baldwin 2022-05-25 | High School ChemistrySafety Wear safety spectacles, lab coat and glovesFun with iron III thiocyanatethe dark red one that is sometimes called fake bloodAfter chatzida 8 minutes of joy with Chemistry experimentsexperiment number 3 The Bleeding Heartyoutu.be/NOiHE_9a2McThank you Professor Chatzidakisrequirements3% hydrogen peroxide, 250ml in a beakerapprox. 1.5g potassium thiocyanatea length of steel wire, a rusty nail may doa few drops of 6M hydrochloric acidinstructionsplace the hydrogen peroxide in a small beakeradd the potassium thiocyanate and stir until dissolvedbend the steel wire into a desired shape and dangle in the beakercarefully run drops of 6M HCl down the wireenjoy the showcommentsone may be able to use a smaller mass of thiocyanateammonium thiocyanate was used instead of potassium thiocyanate in the video clip linked in the description above to chatzida
Factors affecting the rate of a chemical reaction WNOD4382 Nigel Baldwin 2022-05-24 | High School ChemistrySafety DO NOT USE 50% hydrogen peroxide, it decomposes very violently and exothermically when mixed with manganese dioxide. 50% hydrogen peroxide should be diluted at least 10X to 5% or less for use in experiments.Wear safety spectacles, gloves and a lab coatFactors affecting the rate of a chemical reactionTopic primer or revision videoWhat are the four factors that lead to an increased rate of reaction in IGCSE Chemistry courses?Four reactions in test-tubes1 Surface area of solid reactantslimestone chips versus powdered calcium carbonatecalcium carbonate and hydrochloric acid2 Effect of a catalysttwo black powders and hydrogen peroxidecopper II oxide and manganese dioxide3 ConcentrationMagnesium and hydrochloric acidDilute acid about 0.1M and concentrated acid 2M4 TemperatureHot and coldSodium thiosulfate, 0.5ml 0.1M and hydrochloric acid 2ml 2M
Heating iodine Nigel Baldwin 2022-05-06 | High School ChemistryHeating iodineSafetyHeating iodine should always be carried out in a fume cupboard.It turns into purple iodine gas very easily and this should not be breathed in.The violet vapour is harmful. It attacks the eyes, skin and lungs.Iodine is also very toxic to aquatic life.ExperimentWhat happens when you heat solid iodine in an evaporating basin using a Bunsen burner?Does it melt?Is there any evidence in the video of it turning directly from a solid to a gas? Does it sublime?Does it have a low melting point or a high melting point?Research a value for the melting point of iodineWhat does the behaviour of iodine on heating tell us about its structure? Is it formed from a giant structure or a small molecule structure?Key Stage 3 Chemistry resourceFor homework or those studying at home
Heating sulphur Nigel Baldwin 2022-05-06 | High School ChemistryHeating sulfuror sulphurSafetyHeating sulfur should always be carried out in a fume cupboard.It burns very easily with a pale blue flame producing toxic sulfur dioxide.Sulfur dioxide is a toxic gas which should not be breathed in.ExperimentWhat happens when you heat solid sulfur in a crucible using a Bunsen burner?Does it melt?Does it have a low melting point or a high melting point?Research a value for the melting point of sulfurWhat does the melting point of sulfur tell us about its structure? Is it formed from a giant structure or a small molecule structure?Key Stage 3 Chemistry resourceFor homework or those studying at home
Separating salt and sand Nigel Baldwin 2022-05-05 | High School ChemistryHow would you separate a mixture of salt and sand?What techniques would you use? Key Stage 3 resource video For homework or those studying at home
Titration of HCl against NaOH using methyl orange indicator MYFI9765 Nigel Baldwin 2022-04-20 | High School ChemistryTitrationA titration of 25ml of sodium hydroxide of unknown concentration against 1M hydrochloric acid using methyl orange indicatorSafetySafety spectacles must be worn when carrying out the titration0.4M sodium hydroxide is labelled irritant1M hydrochloric acid is labelled irritantAny spillages should be washed off with copious amounts of water immediatelyMethyl orange indicator coloursred in acidyellow in alkaliorange at the endpointI describe the colour as peach in the video clip, but you should use the word orange in GCSE chemistry examinationsThe video clip is a little jumpy due to my editingHere's a revision calculation for GCSE Chemistry students Using the following data obtained from the video clip, calculate the concentration of the sodium hydroxide solution Table of resultsStarting volume 2.4mlEnd volume 12.4 mlTitration volume 10.0mlThe end volume was possibly 12.45 or 12.5 ml but this was not as clear as it should have been on the video clip. This illustrates the need to carry out repeat titrations until two concordant results are obtained.Two concordant results in this titration experiment would have been two titration volumes with the same value or within 0.1ml of each other.Titration calculationThe titration equation isNaOH + HCl = NaCl + H2OThus 1 mol NaOH = 1 mol HClStep 1 What were the number of moles of HCl used in the titrationNumber of moles of HCl = concentration x volume in dm310 ml HCl = 0.01dm3 HClNumber of moles of HCl = 1 x 0.01 = 0.01 molStep 2 From the titration equation0.01 mol HCl = 0.01 mol NaOHStep 3 What is the concentration of the NaOHConcentration = number of moles NaOH / volume NaOH25ml NaOH = 0.025dm3Concentration = 0.01 / 0.025= 0.4 M0.4M = 0.4 mol / dm3You Tube text descriptions do not allow brackets etcThe experiment was filmed using a smartphone in portrait orientation to facilitate revision on a smartphone
Testing three blue solutions and other unknowns NTRG2511 Nigel Baldwin 2022-04-11 | High School ChemistryIGCSE ChemistryTesting anions and cations in solutionTest-tube reactions1 Three blue solutions labelled 1, 2 and 3chloride and sulfate tests are carried outIdentify which is the sulfate, which is the chloride and which is the nitrateWhich metal cation produces blue solutions on the IGCSE Chemistry specification2 Green and orange solutions labelled 4 and 5addition of sodium hydroxideandchloride and sulfate tests are carried outFrom the result of the addition of sodium hydroxide you should be able to confirm the identity of the metal cations as listed on the IGCSE Chemistry specificationThen you can identify which is the sulfate and which is the chloride from the results of the further tests3 Two colourless solutions labelled 6 and 7addition of a few drops of dilute sodium hydroxidefollowed by excess of dilute sodium hydroxideFrom the results of the addition of sodium hydroxide you can tell which of the two solutions contains aluminium ions.The other colourless solution is known to contain either calcium or magnesium ions. Which further test could you carry out to tell which of these two metal ions is in fact presentThe IGCSE Chemistry specification mentioned above is the Oxford AQA International GCSE Chemistry specification 9202See section 3.4.3 Identification of ionsResults1, 2 and 3 are all pale blue solutions and hence are all copper II salts given the limitations of our specification.These solutions are also known to be either a nitrate, a chloride or a sulfateSolution 1white ppt with acidified barium chloride, therefore this must be a SulfateSolution 1 is copper II sulfateSolution 2No ppt with either acidified silver nitrate or acidified barium chlorideTherefore, this must be the Nitrate Solution 2 is copper II nitrateSolution 3white ppt with acidified silver nitrate, therefore this must be a ChlorideSolution 3 is copper II chlorideSolution 4Green solutiongreen ppt with dilute sodium hydroxideIron IIwhite ppt with acidified barium chloridesulfateSolution 4 is iron II sulfateSolution 5Orange solutionorange ppt with dilute sodium hydroxideIron IIIwhite ppt with acidified silver nitratechlorideSolution 5 is iron III chlorideSolutions 6 and 7 were known to contain either magnesium, calcium or aluminium ionsSolution 6 white ppt with dilute sodium hydroxideppt did not dissolve in excess sodium hydroxidetherefore this solution contains either magnesium or calcium ionsA flame test should be carried out to differentiate the two possibilitiescalcium gives a red orange coloured flamemagnesium does not produce a colour in a blue Bunsen burner flameSolution 7white ppt with dilute sodium hydroxideppt dissolved in excess dilute sodium hydroxidetherefore this solution contained aluminium ions
Magnesium and iron sulfate solution IMG 0760 Nigel Baldwin 2022-04-03 | High School ChemistryA fun little experiment in which a small piece of magnesium ribbon was placed in iron sulfate solutionA displacement reaction occurredThe magnesium soon became attracted to a magnet. Can you explain why?Write a word equation for the reactionWrite a symbol equation for the reaction based on iron II sulfateNoteIron ammonium sulfate was actually usedYouTube does not permit the use of brackets in text
GCSE Chemistry Testing three unknown substances DXDE9049 Nigel Baldwin 2022-04-03 | High School ChemistryGCSE ChemistryTesting three unknown white crystalline solids.The solids were labelled X, Y and ZIf the solids were known to be citric acid, sodium hydrogencarbonate and potassium chloride, which one was which?Testing for Solubility in waterpH using Universal Indicator paperFlame testsHalide ion test using acidified silver nitrateCarbonate testResultsX dissolved in water quicklypH 6 a flame test that included lilac, but admittedly there were orange-red colours visible tooa white precipitate with acidified silver nitrateYdissolved in water quicklypH 2 or 3no flame colourno precipitate with acidified silver nitratereacted with calcium carbonate to produce bubbles of colourless gas which were presumed to be carbon dioxideZ dissolved in water but not as quickly as the otherspH 8yellow flame colourorange-red colour was visible on the outside of the flame tooinitially produced bubbles of colourless gas and a white precipitate in a first silver nitrate test acidified with 0.1M nitric acidwhen acidified with 1M nitric acid in a second silver nitrate test no white precipitate was observedbubbles of colourless gas were produced on addition of 1M HCl to a solution of Z and when the gas was passed through limewater a white precipitate was produced. Carbon dioxide. Z was a carbonate.IdentificationsX potassium chlorideY citric acidZ sodium hydrogencarbonate aka sodium bicarbonateIt would have been nice to have a clearer flame test with XI did not have any blue glass with which to view the flame colour produced by X although lilac colour was clearly visible
Testing for oxygen with a glowing splint Slow Motion clip IMG 0509 Nigel Baldwin 2022-02-13 | High School ChemistryHydrogen peroxide and dried yeast were used to generate oxygen gas. However, the rate of production of gas was too slow, so a little potassium iodide was added to the mixture and oxygen gas was produced far quicker.The beaker got very hot and big bubbles of gas were produced.A glowing splint was introduced into the beaker near the bursting bubbles at the bottom.The clip was shot at 240fps and should be in Slow motionThe movie clip was shot in portrait mode for viewing on a smartphone. I hope that You Tube doesn't autocorrect the orientation.
Testing for oxygen with a glowing splint IMG 0508 Nigel Baldwin 2022-02-13 | High School ChemistryHydrogen peroxide and dried yeast were used to generate oxygen gas. However, the rate of production of gas was too slow, so a little potassium iodide was added to the mixture and oxygen gas was produced far quicker.The beaker got very hot and big bubbles of gas were produced.A glowing splint was introduced near the top of the beaker near the bursting bubbles.The movie clip was shot in portrait mode for viewing on a smartphone. I hope that You Tube doesn't autocorrect the orientation.
Testing for oxygen with a glowing splint IMG 0505 Nigel Baldwin 2022-02-13 | High School ChemistryHydrogen peroxide and dried yeast were used to generate oxygen gas. However, the rate of production of gas was too slow, so a little potassium iodide was added to the mixture and oxygen gas was produced far quicker.The beaker got very hot and big bubbles of gas were produced.A glowing splint was introduced near the top of the beaker near the bursting bubbles.The movie clip was shot in portrait mode for viewing on a smartphone. I hope that You Tube doesn't autocorrect the orientation.
Oxygen gas test with a glowing splint WZNEE5015 Nigel Baldwin 2022-02-13 | High School ChemistryHydrogen peroxide and dried yeast were used to generate oxygen gas. However, the rate of production of gas was too slow, so a little potassium iodide was added to the mixture and oxygen gas was produced far quicker.The beaker got very hot and big bubbles of gas were produced.A glowing splint was introduced near the top of the beaker near the bursting bubbles.This is an edited version of the original clip using iMovieThe movie clip was shot in portrait mode for viewing on a smartphone. I hope that You Tube doesn't autocorrect the orientation.
Chlorine gas and potassium bromide solution IMG 0498 Nigel Baldwin 2022-02-13 | High School ChemistryDisplacement reactionBubbling chlorine gas into potassium bromide solutionIt was filmed in portrait orientation for viewing on a smartphone, I hope YouTube doesn't autocorrect to landscape view
Chlorine gas and potassium iodide solution IMG 0495 Nigel Baldwin 2022-02-13 | High School ChemistryDisplacement reactionBubbling chlorine gas into potassium iodide solutionIt was filmed in portrait orientation for viewing on a smartphone, I hope YouTube doesn't autocorrect to landscape view
Testing for hydrogen 2 IMG 0442 Nigel Baldwin 2022-01-30 | High School ChemistryTesting for hydrogen gas with a burning wooden splint.Commonly referred to as the pop test.The hydrogen gas burns with a small explosion, often producing a squeaky pop sound during the process.Note that the bung was only placed very loosely on the mouth of the tube and did not make an airtight seal, but did trap enough gas for testing successfully.Portrait orientation for viewing on a smartphone.The video clip was shot at 240fps, but I don't know if it will play back in slow motion on You Tube.At 240 fps one can stop frame and see the gas burning with a flame that extends down into the tube.
Testing for hydrogen 1 IMG 0441 Nigel Baldwin 2022-01-30 | High School ChemistryTesting for hydrogen gas with a burning wooden splint.Commonly referred to as the pop test.The hydrogen gas burns with a small explosion, often producing a squeaky pop sound during the process.Portrait orientation for viewing on a smartphone.
Testing for oxygen with a glowing splint 2 IMG 0436 Nigel Baldwin 2022-01-30 | High School ChemistryTesting for oxygen with a glowing splint Hydrogen peroxide and a small amount of manganese dioxide were used to generate the oxygen in a conical flaskPortrait orientation for viewing on a smartphone
Testing for oxygen with a glowing splint 1 IMG 0432 Nigel Baldwin 2022-01-30 | High School ChemistryTesting for oxygen with a glowing splint Hydrogen peroxide and a small amount of manganese dioxide were used to generate the oxygen in a conical flaskPortrait orientation for viewing on a smartphone
Limewater test for carbon dioxide No sound IMG 0423 Nigel Baldwin 2022-01-26 | High School ChemistryLimewater test for carbon dioxidePortrait orientation for viewing on a smartphone
Testing carbon dioxide with limewater IMG 0422 Nigel Baldwin 2022-01-26 | High School ChemistryVideo clip with sound, portrait orientationUsing limewater to test for carbon dioxideCarbon dioxide is produced by reacting calcium carbonate with dilute hydrochloric acid in a test-tube.The gas is sampled using a plastic dropping pipette and bubbled through limewater.Limewater is a solution of calcium hydroxide, which is sparingly soluble in water.The limewater produces a white precipitate of calcium carbonate on reacting with carbon dioxide gas.
Reactions of acids and using Universal Indicator at school PXL 20220121 Nigel Baldwin 2022-01-23 | High School ChemistryUsing Universal Indicator paper to measure the pH of four solutions and two reactions with dilute hydrochloric acid.QuestionsCan you identify the four solutions whose labels have fallen off in the video?Can you identify the names of the gases produced during the two reactions shown for dilute hydrochloric acid?What are the tests for hydrogen gas and carbon dioxide gas on the GCSE Chemistry specification?Further questionsWhat would you expect to see when dilute hydrochloric acid is added to dilute sodium hydroxide solution? How could you show that a reaction occurs? Is there a heat change associated with this type of reaction? What is it?Answers at the end of the description.Universal Indicator paper was used to measure the pH of four colourless solutions. These were known to be either hydrochloric acid, sodium hydroxide, ethanoic acid or ammonia solution. All of the solutions were approximately 0.1M concentration.Dilute hydrochloric acid was reacted with a small piece of magnesium ribbon in a test-tube. The gas produced was tested by trapping it in the test-tube and then introducing it to an ethanol spirit burner flame. The gas should be tested with a burning wooden splint. Dilute hydrochloric acid was reacted with a few small marble chips and bubbles of colourless gas were produced.I was unable to bubble the gas through limewater which is the diagnostic test at GCSE level Chemistry. However, the gas did extinguish a burning splint very rapidly.These reactions are typical of those carried out at Key Stage 3 and Key Stage 4 in Chemistry at school and are presented here in portrait orientation for viewing on a smartphone.Answers to the questions posed aboveUniversal IndicatorSolution A = dark red, pH 1, hydrochloric acid Solution B = orange, pH 4, ethanoic acidSolution C = green, pH 8, ammonia solutionSolution D = blue-purple, pH 12 - 13, sodium hydroxide solutionHydrochloric acid + magnesium metal produced hydrogen gas.Bubbles of colourless gas were observed. Remember, you cannot claim to see hydrogen gas when writing answers to examination questions.Hydrogen gas burns with a pop when tested with a lit splint or burning wooden splint. Hydrochloric acid + calcium carbonate produced carbon dioxide gas.Bubbles of colourless gas were observed.Carbon dioxide gas produces a white precipitate when bubbled through limewater. We often say that limewater turns milky when carbon dioxide is bubbled through it.Carbon dioxide will extinguish a burning wooden splint, but so will other gases on the GCSE Chemistry specification such as nitrogen gas and chlorine gas, so this is not a diagnostic test.Answers to further questionsHydrochloric acid reacts with sodium hydroxide to produce sodium chloride and water. The sodium chloride product is soluble in water and no visible change is observed with our eyes during the reaction. However, the reaction can be monitored using Universal Indicator.In the above example scenario when hydrochloric acid is added to sodium hydroxide the colours observed would change from purple-blue to blue, then green, then yellow, then orange, then finally red when the acid would be in excess.The neutralisation reaction could also be monitored by taking temperature readings since heat is given out during the reaction. This is due to the formation of water molecules. The neutralisation reaction is exothermic. However, this is very difficult to show in a video clip using dilute 0.1M solutions of hydrochloric acid and sodium hydroxide and an alcohol thermometer.
The reactions of lithium, sodium and potassium with water PXL 20220119 Nigel Baldwin 2022-01-20 | High School ChemistryThe reactions of alkali metals with waterSmall pieces of lithium, sodium and potassium are added to water in large beakers. The water had Universal Indicator added to it prior adding the metals. ObservationsCompare the similarities and differences in the reactions of the three group 1 metals with water.A short video clip in portrait orientation which may be better for viewing on a smartphone.The lilac colour to the flame produced by potassium was very subdued in this experiment.
Bicarbonate rockets in slow motion 2 C0133 Nigel Baldwin 2021-08-29 | Lockdown chemistryFun chemistry experiments you might choose to do at home.Safety firstDo not stand over, put your face close to or point a bicarbonate rocket at anyone during launch. Stand well back and enjoy.DO NOT USE GLASS BOTTLESRequirementsA small plastic bottleA bung (cut from a rubber pencil eraser to fit the mouth of the plastic bottle)10ml vinegar, approx.0.5g of sodium hydrogen carbonate, approx.Half a square of soft toilet tissueProcedurePour the vinegar into the bottle to a depth of 0.5 to 1 cmSpread the sodium hydrogen carbonate onto the tissue paper and fold the edges of the paper forming a cylinder with the sodium hydrogen carbonate insideFold the tissue paper into a U shape and twist the two ends light together Holding the bottle almost horizontal, insert the tissue paper until the end just protrudes from the mouth of the bottleDON'T LET THE PAPER COME IN CONTACT WITH THE VINEGAR AT THIS STAGEInsert the rubber bung, trapping the end of the paperPlace the bottle vertically on a flat surface, standing on the bung and stand back for lift-offEnjoy and repeat as necessaryThe chemistry of the chemical reaction between ethanoic acid and sodium hydrogen carbonate can be exploredacid + carbonate = salt + carbon dioxide + waterHave fun with small scale chemistry and microscale chemistryInspired and encouraged by Bob Worley, Jonathan Barton and Abdul Khan
Bicarbonate rockets in slow motion Nigel Baldwin 2021-08-29 | Lockdown chemistryFun chemistry experiments you might choose to do at home.Safety firstDo not stand over, put your face close to or point a bicarbonate rocket at anyone during launch. Stand well back and enjoy.DO NOT USE GLASS BOTTLESRequirementsA small plastic bottleA bung (cut from a rubber pencil eraser to fit the mouth of the plastic bottle)10ml vinegar, approx.0.5g of sodium hydrogen carbonate, approx.Half a square of soft toilet tissueProcedurePour the vinegar into the bottle to a depth of 0.5 to 1 cmSpread the sodium hydrogen carbonate onto the tissue paper and fold the edges of the paper forming a cylinder with the sodium hydrogen carbonate insideFold the tissue paper into a U shape and twist the two ends light together Holding the bottle almost horizontal, insert the tissue paper until the end just protrudes from the mouth of the bottleDON'T LET THE PAPER COME IN CONTACT WITH THE VINEGAR AT THIS STAGEInsert the rubber bung, trapping the end of the paperPlace the bottle vertically on a flat surface, standing on the bung and stand back for lift-offEnjoy and repeat as necessaryThe chemistry of the chemical reaction between ethanoic acid and sodium hydrogen carbonate can be exploredacid + carbonate = salt + carbon dioxide + waterHave fun with small scale chemistry and microscale chemistryThe clip was originally filmed on an iPhone at 120fpsInspired and encouraged by Bob Worley, Jonathan Barton and Abdul Khan
Biarb rocket PXL 20210815 Nigel Baldwin 2021-08-15 | Lockdown Chemistry School ExperimentsChemistry experiments you might be able to do at home under lockdown.SAFETY FIRST - DO NOT STAND OVER OR TOO NEAR TO THE BICARBONATE ROCKET AS IT IS ABOUT TO LAUNCH.WEAR SAFETY SPECTACLESPart 3 Launching the rocketThis movie clip shows how to add the sodium bicarbonate to the vinegar and perform a successful launch.Reduce the amount of bicarbonate and increase the amount of tissue paper to slow down the reaction.Have fun with chemistry experiments at home when you can, even under lockdown.Thanks to Jonathan Barton, Bob Worley and Abdul Khan for inspiration and encouragement.
Bicarb rocket - Testing the bung is water tight PXL 20210815 Nigel Baldwin 2021-08-15 | Lockdown Chemistry School ExperimentsChemistry experiments you might be able to do at home under lockdown.This short movie clip shows an example of testing the bung in the top of the plastic bottle to make sure it is water tight and hopefully airtight under pressure.This is the critical part of the rocket to ensure a successful take-off. If the bung leaks all you will get is a launchpad failure.Have fun with chemistry experiments at home when you can, even under lockdown.Thanks to Jonathan Barton, Bob Worley and Abdul Khan for inspiration and encouragement.
Preparing a bicarb rocket at home PXL 20210815 Nigel Baldwin 2021-08-15 | Lockdown Chemistry School ExperimentsChemistry experiments you might be able to do at home under lockdown.SAFETY FIRST - GET AN ADULT TO CUT THE RUBBER BUNG OUT OF A SOFT PENCIL ERASER USING A SHARP KNIFE. Part 1 Making the rocketIn this movie clip you can see an example of materials you might be able to obtain from the supermarket in order to make a small bicarbonate rocket.The small plastic bottle used was approximately 20 - 30ml capacity and was an inexpensive candy container.The remaining equipment is probably familiar and should be low cost.Materials listSmall plastic bottleSoft rubber pencil eraserWhite vinegar -although any vinegar found in the kitchen should workBicarbonate of soda - sodium hydrogen carbonateA sheet of tissue paperSharp knife to cut out the rubber bung - make sure an adult does thisWhen the rubber bung is cut out from the eraser its best to cut out a cone shape to ensure an airtight fit in the bottle when the bung is inserted. See next movie clip.Have fun with chemistry experiments at home when you can, even under lockdown.Thanks to Jonathan Barton, Bob Worley and Abdul Khan for inspiration and encouragement.
Heating a mixture of copper (II) oxide and carbon C0118 Nigel Baldwin 2021-08-09 | High School ChemistryA brief movie clip showing a mixture of copper (II) oxide and carbon being heated in a test-tube.A thermal reduction reaction is seen to occur.
Snow statues close-up DSCN1174 Nigel Baldwin 2021-05-18 | Greenhouse chemistryA close-up recap of the snow statues experiments in the previous two movie clips.
Snow statues 2 Nigel Baldwin 2021-05-18 | Green house chemistrySafety adviceDo not ingest any of the chemicals, particularly the potassium hexacyanoferrate II and potassium hexacyanoferrate III if these are used.Wash off any spillages in contact with skin immediately and wear safety spectacles.This movie clip follows on from the previous one showing the results of the snow statue experiments after 24 hours.There is a brief discussion at the end of the clip of some of the factors involved in producing a good cardboard snow statue.In order to carry out this experiment at home you need access to a tiny amount of potassium ferrocyanide, aka potassium hexacyanoferrate II.You may be able to buy this online. I was able to buy 50g for 6 UK pounds.You may be able to take a saturated solution of sodium chloride to the chemistry department of your school if you attend one and ask them to add 2 drops of a 0.1M solution of potassium hexacyanoferrate II to it.Potassium hexacyanoferrate II is one of the chemicals used in commercial cooking salt or household table salt and thus there is very low risk involved once the tiny amount has been added to the saturated sodium chloride solution.Lot's of interesting snow statues and snow scene experiments can be safely carried out once you have acquired your stock solution. Just remember to use pure salt, such as sea salt with no additives added when making up your saturated solution of sodium chloride.Have fun with chemistryAn explanation of the formation of the snow crystals is given heremelscience.com/GB-en/chemistry/experiments/xmas-treeor heremelscience.com/GB-en/chemistry/experiments/xmas-v2_xmas-treeand a nice time lapse of the procedure heremelscience.com/SA-en/articles/homemade-christmas-tree
Snow statues Nigel Baldwin 2021-05-18 | Greenhouse chemistrySnow statues Making snow statues or snow scenes using a saturated solution of sodium chlorideThere are edited jumps in the movies clip0 to 2m 14s Setting up the experiments2m 15s to 2m 35s After approximately 2 hours2m 36s to 3m 2s After approximately 4 hours3m 3s to finish After approximately 7 and a half hoursFive solutions were usedTwo solutions at the front or in the foregroundLeft = saturated sodium chloride solution + potassium ferrocyanideRight = saturated sodium chloride solution + potassium ferricyanideThree solutions at the back or in the rear of the shot as followsLeft = saturated solution of Low salt, a mixture potassium chloride 51%, sodium chloride 48% and anti-caking agents 1%. The anti-caking agents are listed as magnesium carbonate, potassium hexacyanoferrate II and sodium hexacyanoferrate II.Middle or centre = saturated solution of sodium chloride made from sea salt, large crystals of sodium chloride with no additives explicitly stated on the bottleRight = saturated solution of cooking salt with ingredients listed as salt and an anti-caking agent sodium ferrocyanideA note on some chemical namesSalt = sodium chlorideSodium ferrocyanide = sodium hexacyanoferrate IIPotassium ferrocyanide = potassium hexacyanoferrate IIPotassium ferricyanide = potassium hexacyanoferrate IIIPlease note YouTube does not allow the use of brackets in these descriptions. When writing names of chemicals in chemistry brackets should be placed around the Roman numerals in the above chemical names.Questions1 What is the chemical name and formula of common salt?2 What is the chemical name and formula of the compound added to common salt in Low salt?3 What is the health benefit of using Low salt instead of common salt, sodium chloride4 What chemical is added to a saturated solution of sodium chloride to produce profuse white crystals that look like snow on a cardboard cutout shape?5 What is the colour are the snow-like crystals formed if potassium hexacyanoferrate III is added a saturated solution of sodium chloride when carrying out these experiments?6 What colour is hydrated iron III oxide and what name is used to refer to it in common English language?7 Why are large crystals of sea salt of far greater purity than cooking salt or table salt used at home?8 Why are chemicals such as magnesium carbonate and sodium ferrocyanide added to cooking salt or table salt? 9 What is another chemical name for potassium ferrocyanide and in what oxidation state is the iron in it?10 What is another chemical name for potassium ferricyanide and in what oxidation state is the iron in it?11 Find out the chemical formulae for the followinga sodium ferrocyanideb potassium ferrocyanidec potassium ferricyanideAnswers1 sodium chloride NaCl2 potassium chloride KCl3 It is used to help reduce blood pressure4 potassium ferrocyanide or potassium hexacyanoferrate II5 yellow6 orange, rust7 Because chemicals often referred to as anti-caking agents are added to the sodium chloride, salt8 To make the salt flow easily out of the container, even when moderate amounts of water are absorbed by the salt in humid atmospheres. Anti-caking agents stop the salt forming into lumps.9 potassium hexacyanoferrate II and Fe2+10 potassium hexacyanoferrate III and Fe3+11 a to c It is not possible to write down the letters and symbols correctly in this description due to YouTube limitations, however they will be shown in a subsequent movie clip
Recrystallisation of copper sulfate C0068 Nigel Baldwin 2021-05-02 | Greenhouse chemistryRecrystallisation of copper sulfateErrors and safety adviceWear safety spectacles and wash off any material that comes in contact with skin immediately2mins 50sec Do not use boiling water as this is too risky and unnecessary7mins 50sec Error. Water evaporates, not the copper sulfate crystalsThe ExperimentI wanted to see if I could carry out a recrystallisation of an ionic solid in the greenhouse using only materials commonly found at home.250g of copper sulfate was obtained online for a couple of poundsThe copper sulfate from the online supplier was a greenish solid in colour, rather than the expected bright blue crystals.A sample of the greenish solid was dissolved in hot water and filtered to remove any insoluble impurities.The filtrate was placed in a bowl and left to stand overnight. Water evaporated and crystals of copper sulfate formed.The crystals were removed from the solution by filtration and washed with de-ionised water.Blue copper sulfate crystals were obtained.
Sodium chloride crystals from cooking salt and sea salt DSCN1087 Nigel Baldwin 2021-04-29 | Greenhouse chemistryClose-up movie clip of the crystals obtained from saturated solutions prepared from cooking salt and sea salt.Questions1 Give the chemical name of the compound commonly referred to as salt2 Name the two types of salt used in these experiments3 What shape are the crystals obtained from sea salt?4 What is the anti-caking agent added to cooking salt?5 Does the anti-caking agent appear to affect the shape crystals produced from cooking salt? Explain your answer. 6 Name two factors that affect how quickly solutions evaporate.7 How could you alter the experimental conditions to produce larger crystals of sodium chloride from a saturated solution of sea salt8 A common chemical reaction carried out at school is the neutralisation of an acid with a base. A base that is soluble in water is called an alkali.The general equation is acid + base = salt + waterName the acid and the alkali frequently used at school to produce sodium chloride in this way.9 In everyday language when we use the word salt, we are usually referring to sodium chloride, as in this movie clip.However, in chemistry the term salt has a much broader meaning, it is used as a general term for ionic compounds.a Name another sodium saltb Name another chloride saltc Name a salt that is neither a sodium salt, nor a chloride saltAnswers1 Sodium chloride2 Cooking salt and sea salt3 Cubic, cubes, cuboid, square shaped4 Sodium ferrocyanide5 Yes, the anti-caking agent does appear to affect the shape of the crystals produced. A mixture of irregularly shaped crystals appear to form, although there are some cubic crystals in the mixture. In general the solid particles are too small to discern a single, regular shape6 Temperature, surface area of the solution and the humidity and movement of the surrounding air are four factors that affect the rate of evaporation. There are others.7 Let the solution evaporate slowly at a cool temperature, in a narrow vessel with reduced surface area in still, not too dry surrounding air.8 hydrochloric acid + sodium hydroxide = sodium chloride + water9 Many answers are possible here, e.g.a sodium iodideb potassium chloridec copper sulfateNote YouTube does not allow angled brackets in text descriptions
Recrystallisation of sodium chloride at home C0061 Nigel Baldwin 2021-04-29 | Greenhouse chemistryRecrystallisation of sodium chloride from the kitchen.Saturated solutions were made by adding an excess of solid salt to a small volume of hot tap water from a kettle.Two saturated salt solutions were made, one using cooking salt and another using sea salt.With cooking salt approximately 200g of salt were added to about 250ml water.For sea salt approximately 100g of salt was added to about 120ml waterThe salt solutions were made up in 1 litre milk cartons that had been thoroughly washed with water before use. Milk cartons were used because they allowed the salt solutions to be shaken quite easily. The salt solutions were left to stand overnight before pouring into the bowls as shown in the movie clip.After pouring the solutions were left to evaporate for a few days. The rate of evaporation depends on the temperature and humidity which were quite variable in the greenhouse. Nevertheless, crystals were formed overnight and grew larger over the next few days.Cooking salt contained sodium chloride and a small amount of sodium ferrocyanide as an anti-caking agent.Sea salt contained solid sea salt, sodium chloride with no additives.The crystals obtained by allowing saturated solutions of the two salts to evaporate looked quite different.A close-up view of the results from the two experiments can be seen in another movie clip.
Electrolysis of yellow tulip extract DSCN0956 Nigel Baldwin 2021-04-17 | Greenhouse chemistryElectrolysis of a water ethanol extract from a yellow tulip flower.6v battery, carbon fibre electrodes.See the previous post on 15th April 2021 for details and research links.Yellow tulip flower extractColourless in acid, as develops around the anode during electrolysis.Deep yellow in alkali, around the cathode.Can you explain the difference in colours observed?Fun with small scale and microscale chemistry.
Electrolysis of tulip flower extract DSCN0933 Nigel Baldwin 2021-04-16 | Greenhouse ChemistryIt's the time of year when tulips are in the garden which gives an opportunity to try out the electrolysis of a tulip flower extract as shown by Bob Worley in 2020In the experiment shown here a few dark red tulip flower petals were cut up into small pieces and left to stand in an ethanol water mixture before filtering. The extract so obtained was elctrolysed using a 6v battery and carbon fibre electrodes in the greenhouse.Bobs original video clip can been seen here Fruit skin and fruit dyes as indicators, Apr 24, 2020youtu.be/WX2dSdvVPe0At the end of this video clip Bob details the anthocyanins responsible for the colours observed and the same electrolysis of a tulip flower extract shown here.Also see pH Profiling of Plant Extracts, Jul 31, 2020youtu.be/tbR5dHcWWdsMany examples of the colours observed for various flower extracts in acid and alkaline conditions can be seen here in a Tweet from the Crocodile Chemist, Mar 2nd 2020 Garden Indicators projecttwitter.com/CrocodileChemi1/status/1366724709975552002?s=20and the linked Google sheet heredocs.google.com/spreadsheets/d/1JqyWXZcYqyitfHPyyqVwHu7AVvV6Malo-T66uwDn9Ko/htmlview#It's worth noting that the colours observed for the tulip flower extract in acid and alkali at the end of the video clip agree with those reported on the Garden Indicators project spreadsheetTulip flower extract in water ethanolcolour in acid redcolour in alkali greenMany thanks to UncleBob@UncleBo80053383 and CrocodileChemist@CrocodileChemi1for inspiration and ideasHave fun with microscale chemistry!
What time is it? Nigel Baldwin 2021-04-06 | Greenhouse chemistryWhat time is it?A failed iodine clockFun with vitamin C, iodine and hydrogen peroxide in the greenhouse.Small droplets of a mixture containing vitamin C, starch solution and Povidone iodine were placed on a sheet of plastic.Small droplets of hydrogen peroxide solution were placed next to them.Pairs of droplets were mixed using a cocktail stick.A clock face was fashioned by the reacting droplets.What time is it showing at the end of the video?Fun with micro-scale chemistry. ROTATE 1617715994966
Testing for oxygen gas C0055 Nigel Baldwin 2021-03-27 | Greenhouse chemistryTesting for oxygen gas with a glowing splint.IGCSE ChemistryThe splint re-lights or catches fire in oxygen.SafetyUse extreme caution when opening an alkaline battery or cell. Wear gloves and safety spectacles. Do not let the black powder inside the cell come into contact with your skin. It is alkaline and corrosive.The black powder contains manganese dioxide which acts as a catalyst for the breakdown of hydrogen peroxide, releasing oxygen gas.
Testing for hydrogen gas C0053 Nigel Baldwin 2021-03-27 | Greenhouse chemistryTesting for hydrogen gas with a burning splint.IGCSE ChemistryIf the gas burns with a pop, it's hydrogen, which is why many refer to this as the pop test.
