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Chemistry A-Level Techniques and Procedures - Statistics

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Hint Answer % Correct
2. pipette 25cm^3 alkaline solution into a ____ ____ conical flask
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1. ____ the balance zero
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6. record the start reading to the nearest ____ cm^3 0.05
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7. carry out the titration and record the end reading to the nearest ____ cm^3 0.05
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1. rinse and fill the burette with ____ acid
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ensure the oven's temperature is ____ the melting point of the salt below
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3. use a ____ to add the correct amount of acid to neutralise the alkali burette
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2. close the ____ ____ burette tap
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5. plot a ____ ____ of concentration against absorbance calibration curve
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4. use a ____ to hold your burette in place clamp
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therefore, we can use iodine-thiosulfate titration to find the ____ of a solution of chlorate (I) concentration
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7. repeat until you have three ____ results within 0.10cm^3 of each other and use the mean concordant
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3. vertically attach a ____ so the water flows in at the bottom and out at the top condenser
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2. transfer 25cm^3 alkaline solution to a clean ____ ____ conical flask
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3. leave to ____ cool
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5. heat over a Bunsen burner to evaporate the water until ____ start to appear crystals
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1. rinse pipette with ____ ____ and then a small volume of the solution to be pipetted distilled water
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1. rinse burette with ____ ____ and then a small volume of the solution to be used distilled water
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6. filter the mixture and wash the residue with cold ____ ____ distilled water
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5. allow the plate to ____ dry
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3. cover with a watch glass to prevent ____ evaporation
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keep the cap on to reduce fuel loss by ____ evaporation
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3. pour the solution into the burette using a ____. fill to above the zero line funnel
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5. stir the mixture with a ____ ____ to ensure the solute has completely dissolved glass rod
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4. empty the solid into the ____ and accurately reweigh the empty weighing bottle glassware
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4. run the liquid from the pipette to the ____ glassware
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3. add 2-3 drops of ____ and swirl to mix indicator
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swirl after each drop until the colour of the ____ just changes indicator
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1. put the reactants in a ____ ____ flask pear-shaped/round-bottomed
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____ is colourless in acidic solutions and pink in basic ones phenolphthalein
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2. using a ____ ____ draw enough liquid into the pipette until it is exactly the right volume pipette filler
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5. match the calculated ____ values with those in a database Rf
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5. the first titration is the ____ titration to indicate roughly how much acid is required rough
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8. the oven's temperature should be below the melting point of the ____ salt
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3. accurately record the mass of the ____ plus the weighing bottle solid
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3. transfer the weighed ____ into the water solute
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2. suspend the plate in a baker containing the ____ solvent
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3. check the bulb of the electrode is completely immersed, then wait for the reading to ____ stabilise
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1. rinse a clean dry beaker with the ____ ____ then half-fill it stock solution
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5. ____ mass of empty weighing bottle from mass of solid + weighing bottle subtract
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4. run the acid, ____ the flask, until the solution just changes colour swirling
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2. use a thermometer to take the initial ____ temperature
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8. find the ____ by subtracting the initial reading from the final reading titre
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7. transfer the residue to a ____ ____ and heat in an oven to dry the solid watch glass
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2. place a ____ ____ on the balance weighing bottle
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1. calculate the mass of solute required and weigh out in a ____ ____ weighing bottle
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5. put the conical flask on a ____ ____ to make the end point easier to see white tile
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a pure substance melts within ____K of the true melting point 0.5
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8. add deionised water, swirling at intervals to mix the contents, until the level is within about ____ cm^3 of the mark on the flask's neck 1
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calibrate to pH ___ for alkaline solutions 10.00
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6. carry on heating until the temperature has risen by about ____ to ____ K 15 20/1520/fifteentwenty/fifteen twenty
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3. when the vapour temperature is about ____ degrees below the boiling point of the liquid, put the collecting beaker in place 2/two
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calibrate to pH ___ for acidic solutions 4.00
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4. collect the liquid until the temperature of the vapour rises ____ the boiling point of the liquid you are collecting above
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this allows for the greatest values of ____ absorbance
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4. measure the ____ of each of the standard solutions absorbance
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a measure of the closeness of agreement between an individual test result and the accepted reference value accuracy
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1. carry out an ____ ____ ____ to find how much acid solution is needed to neutralise 25cm^3 alkaline solution acid base titration
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5. open the tap and allow the solution to run into a beaker until there are no ____ ____ air bubbles
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1. pour some chlorate (I) solution into a clean, dry beaker and transfer a 25cm^3 ____ into a conical flask aliquot
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5. dry the crude product by adding ____ ____ ____ and swirling anhydrous sodium sulfate
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the ____ will need to be made of the impure metal anode
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2. add ____ ____ ____ (stop large bubbles forming suddenly and allow for a smooth boiling process) anti bumping granules
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1. put the mixture in a pear-shaped flask and add ____ ____ ____ anti bumping granules
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the contents of the flask will turn ____ ____ due to iodine being present blue-black
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you will know it's the right volume when the ____ __ __ ____ is level with the mark bottom of the meniscus
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9. use a dropping pipette to add deionised water so the ____ __ __ ____ is level with the mark on the neck of the flask at eye level bottom of the meniscus
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9. test any liquid product with ____ ____. it should remain orange/brown bromine water
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add a few drops of ____ ____ bromine water
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at this stage, the contents will be ____ due to iodine being produced brown
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2. dampen a piece of filter paper and place flat in the ____ ____ Buchner funnel
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to measure both acidic and alkaline solutions with a wide range of values, calibrate with acidic, alkaline and neutral ____ buffers
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2. transfer into a ____ ____ of pH 7.00 buffer solution
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you need to ___ the pH electrode for temperature because pH is dependent on temperature calibrate
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1. pour a known volume of water into a copper ____ and record its temperature calorimeter
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1. seal the end of a glass ____ ____ by heating it to melting in a Bunsen flame capillary tube
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2. strongly heat the ____ catalyst
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the ____ should be made of the pure metal cathode
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____ ions are strong enough oxidising agents to oxidise iodide ions to iodine chlorate
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5. rinse the crystals with ____ ____ cold solvent
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1. set up apparatus, place several test tubes of water in the ____ ____ collection trough
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similar to a ____ in that a light source is passed through a sample and absorbance or transmission is measured colorimeter
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for a coloured solution, it can be determined by ____ colorimetry
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7. the end point is where the solution is ____ colourless
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if an alkene is present, the bromine water will change from orange/brown to ____ colourless
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1. select the filter with the ____ colour to the test solution complementary
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the second stage is determining ____ of one of the ions in solution concentration
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2. determine ____ of one of the components in the equilibrium mixture concentration
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10. heat until the solid has dried to a ____ ____ constant mass
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8. leave to ____, then dismantle cool
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this ensures that when the hydrocarbon vapour passes over it, the temperature is high enough for any ____ reactions to take place cracking
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5. follow the procedure for ____ (given above) crystallisation
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3. zero the colorimeter using a ____ of pure solvent cuvette
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10. test the gas by shaking with bromine water. it should ____ decolorise
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2. filter and wash the precipitate several times with cold, ____ ____ deionised water
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2. pour 100cm^3 ____ ____ into a 250cm^3 beaker deionised water
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1. wash the electrode with ____ ____ deionised water
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2. the ____ ____ delivers gas to the burette delivery tube
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7. remove the ____ ____ from the collection trough before stopping heating to prevent suck back delivery tube
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9. at regular intervals, remove the watch glass and solid, cool in a ____ and weigh dessicator
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11. leave to cool in a ____ (these allow materials to cool in a dry atmosphere so prevent reabsorption of moisture) dessicator
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4. heat to constant mass and then leave to cool in a ____ dessicator
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when you use a ____ measuring device, you should record all the figures shown on the instrument digital
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4. if the crude product is alkaline and needs neutralising, add a ____ ____ until it's neutral dilute acid
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if so, do this by filling test tubes with water as these will ____ the water displace
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5. discard the first tube of gas because this will just be ____ air displaced
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6. the pure product can then be separated by ____ distillation
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4. surround with a ____ ____ to help reduce energy losses draught excluder
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6. titrate again. run the acid solution to 1cm^3 below the rough titre then add acid ____ dropwise
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3. ____ the outside of the pipette dry
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3. transfer the precipitate to a clean watch glass and place in a ____ ____ drying oven
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6. dry the crystals in a ____ ____ drying oven
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for a metal ion/metal half cell, the ____ will be made from the solid metal electrode
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4. take the voltmeter reading to find ____ ____ (or standard ____ ____ in this case electrode potential
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1. pass an electric current through the ____ electrolyte
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9. weigh the burner again. you can use this to determine ____ ____ __ ____ enthalpy change of combustion
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6. calculate the maximum temperature reached and use this to determine ____ ____ __ ____ enthalpy change of neutralisation
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1. allow a mixture to reach ____ equilibrium
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the difference between an individual measurement and the true value or accepted reference value of the quantity being measured error
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when using a non-digital device, you should record all the figures that are certain plus one that is ____ estimated
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4. transfer the neutralised solution to a clean ____ ____ evaporating basin
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1. in a beaker, warm ____ insoluble base in dilute acid excess
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2. add a known mass of solid reactant in ____ excess
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6. compare the ____ value to the published value experimental
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7. ____ the spirit burner and replace the cap extinguish
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5. plot a graph of temperature against time and ____ to find the theoretical maximum temperature change extrapolate
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4. filter off excess solid base and transfer the ____ to a clean, dry evaporating basin filtrate
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3. support the calorimeter over a spirit burner containing the ____ to be tested fuel
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4. record changes in temperature every 30 seconds until there is no ____ ____ further change
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4. the ____ will enter the burette and you can take a reading gas
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6. continue heating until no more ____ is produced gas
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you may need to collect ____ products gaseous
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the system must be ____ ____ gas tight
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uncertainty is usually taken to be ____ a division on either side of the smallest scale on the scale you're using half
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1. construct the ____ ____ whose electrode potential is to be measured half cell
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5. vapours should reach no more than ____ up the column before condensing back into a liquid halfway
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4. heat with a ____ ____ so the reaction mixture boils gently heating mantle
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8. keep stirring the water. make a note of the ____ temperature reached highest
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3. connect the two electrodes to a ____ ____ ____ high resistance voltmeter
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3. heat the ____ gently, collecting any gases that pass into the collection tubes hydrocarbon
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for a basic solution, concentration can be determined using acid-base titration with the ____ ions hydroxide
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1. mix the organic product with another ____ liquid such as water immiscible
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the wider the melting range, the more ____ the substance impure
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5. touch the tip of the pipette to the ____ of the glassware inside
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3. filter to remove any ____ ____ and retain the filtrate insoluble impurities
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1. use a measuring cylinder to add a known volume of a known concentration of acid to an ____ ____ insulated vessel
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1. add a known volume of a known concentration of reactant solution to an ____ ____ insulated vessel
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10. insert a stopper in the flask and ____ it several times to ensure thorough mixing invert
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1. use an ____ ____ to collect the gas over water inverted burette
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2. add excess iodide ions, using a measuring cylinder to transfer e.g. 15cm^3 of 0.5 mol dm^3 potassium ____ to the conical flask iodide
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____ is used to detect colourless organic compounds iodine
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the electrolyte must contain ____ of that metal ions
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3. use this to work out the other concentrations and calculate ____ using the equation Kc
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4. top the vessel with a ____ with a hole in and place the thermometer through the hole in the ____ lid
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3. top the vessel with a ____ with a hole in lid
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you can repeat this for multiple ____ in a mixture if necessary liquids/substances
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percentage uncertainty = uncertainty x number of measurements x 100 divided by ____ ____ measured quantity
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3. use a ____ ____ to add a known volume of a known concentration of alkali and stir to mix measuring cylinder/volumetric pipette
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5. note the temperature at which the solid starts and finishes melting - the difference is the ____ ____ melting range
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ensure the ____ reads 7.00 and adjust to that value if necessary meter
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2. dissolve the mixture in the ____ quantity of hot solvent minimum
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in that case, the solution will contain a ____ of the two ions mixture
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if the reading is ____ switch the connections on the voltmeter negative
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2. warm until the solution is ____, adding more solid base if needed neutral
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____ is used to detect compounds with free amino groups such as proteins, amino acids, and amines ninhydrin
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2. tap the ____ end of the tube into a solid so a small amount goes into the tube open/unsealed
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6. carry out titrations. near the end point, the contents of the flask will be a ____ ____ colour pale straw
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if the reaction involves two ions of the same element in different oxidation states, the electron should be ____ platinum
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ensure the reading on the voltmeter is ____ positive
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this ensures that the half-cell connected to the ____ ____ of the voltmeter is the positive electrode positive terminal
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1. add in equal volumes of the desired salt solutions in a beaker to form a ____ of the insoluble salt precipitate
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the closeness of agreement between independent measurements made under the same conditions precision
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just one is sufficient because the concentration of one ion is ____ to the other proportional
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if electrolysis to be carried out to ____ a metal: purify
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1. spot the test mixture and ____ ____ on a pencil baseline 1cm from the base of the TLC plate reference samples
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the opposite of uncertainty (if uncertainty is great, the measurement is unreliable) reliability
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4. filter and discard the ____ residue
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4. ____ the weighing bottle to calculate actual mass in the beaker reweigh
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3. leave the mixture to cool to ____ ____ room temperature
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first, prepare a ____ ____ in deionised water saturated salt
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3. tap the tube so the solid falls to the bottom of the ____ end sealed
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2. allow the layers to separate and dispose of the aqueous layer using a ____ ____ separating funnel
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1. warm deionised water in a small conical flask and add the salt, ____ frequntly shaking
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1. connect a conical flask to a vacuum pump via the ____ ____ side arm
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3. if acid impurities are present, add ____ ____ ____ solution and shake well to remove them sodium hydrogen carbonate
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4. fill burette with a standard solution of 0.1mol dm^3 ____ ____ sodium thiosulfate
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2. keep adding ____ until no more dissolves solute
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4. remove the plate when the solvent is near the top and mark the ____ ____ with a pencil solvent front
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2. weigh a ____ ____ spirit burner
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in all cases, ensure ____ ____ standard conditions
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2. connect the half-cell to a ____ ____ ____ ____ standard hydrogen half cell
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2. make up a range of ____ ____ of the test solution, both above and below the concentration of the unknown solution standard solutions
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at this point, add a few drops of ____ solution starch
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4. fix the tube in melting point apparatus and gently heat the surrounding liquid, ____ to ensure even heating stirring
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5. disconnect the flask from the vacuum pump before turning the pump off to prevent ____ ____ suck back
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4. change and cork any full tubes to prevent ____ ____ and continue to heat suck back
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3. add excess hydrogen ions by adding 20cm^3 of 1 mol dm^3 ____ ____ sulfuric acid
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5. record changes in ____ every 30 seconds until there is no further change temperature
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Ksp is ____ dependent, so take the ____ of the solutions you're working with temperature
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1. select a solvent in which the desired substance is very soluble at high ____ and insoluble at low ____ temperatures
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3. make up to the mark with the usual procedure. you will have diluted your solution by a factor of ____ here ten
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6. locate spots. you may need to add a stain or view under ____ ____ ultraviolet light
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the TLC plate fluoresces under ____ ____. compounds with aromatic rings or conjugated structures appear as dark spots ultraviolet light
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an estimate attached to a measurement which characterises the range of values within which the true value is asserted to lie uncertainty
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6. measure the absorbance of the ____ sample and use the calibration curve to determine its concentration unknown
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4. this creates a partial ____ so the filtrate is quickly pulled through vacuum
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for this step, use a ____ ____ to retain heat vacuum filtration
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4. leave the filtrate to cool until crystals form and collect the crystals by ____ ____ vacuum filtration
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3. switch the ____ ____ on then pour in the mixture to be filtered vacuum pump
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2. the thermometer should read the temperature of the ____ vapour
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a visible spectrophotomer can give data for absorption or transmission for any given value of the ____ ____ visible spectrum
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6. transfer the solution to a clean 250cm^3 ____ ____ volumetric flask
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2. use a pipette filler to pipette 25cm^3 of the stock solution into a 250cm^3 ____ ____ volumetric flask
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7. rinse the beaker and stirring rod with deionised water, ensuring all ____ go into the flask washings
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3. the burette is inverted in a ____ ____ and itself filled with water initially water trough
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in the case of a colorimeter, the coloured light used as a source can only be selected from a specific number of different ____ wavelengths
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5. remove the cap of the spirit burner and light the ____ wick
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