Q1:
Lie big Condenser
To condense the vapor
Different Boiling points
Heat the alkane mixture, the alkane with the lowest boiling point will vaporize and distill over in the conical flask while the remaining two alkanes will remain in the round bottom flask because of fractionating column, Then change the conical flask and heat again, the alkane with second lowest boiling point will distill over leaving only one alkane. Once again change flask and heat again until the last alkane distills over.
Q2:
When effervescence/bubble formation/ fizzing stops
Graph was like inversely proportional curve (kinda like y=1/x)
Time I got from my graph was 215s
Errors:
i) I wrote that use burette instead of measuring cylinder
ii) Reaction time error when starting and stopping the stopwatch so repeat each experiment at least 3 times and take average time
conc=1.4mol/dm^3 (do 35/50 * 2)
Universal indicator, compare the color with pH color chart
Red color solution
Directly proportional relationship between rate of reaction and concentration:
less concentration takes higher time and high concentration takes lower time so greater the concentration greater the rate of reaction.
Q3:
Hazard: the boiling tube will be too hot to touch after heating (liquid will flow out also correct ig)
Precaution: use of pair of tongs and gloves to handle the tube
Substance is Hydrated
Substance contains Sulfur (idk if this point correct though)/ iron (II) to iron (III) oxidation
Damp Red litmus: damp red litmus paper turns blue
Damp Blue litmus: No change
C contains ammonium ion\
Heat solid using Bunsen burner
Iron red-brown precipitate when dropwise, and precipitate remains insoluble in excess
the iron formed an aqueous solution which is yellow in color which initially interferes with the ppt color
Sulfate (SO4-2) ion
Q4:
Apparatus: Burette, conical flask, white tile, methyl orange indicator, retort stand, volumetric pipette
Titrate each aqueuous ammonia sample against a fixed volume of dilute HCl, take 25 cm^3 of dil HCl in the conical flask using piptte and fill up the burette with sample of aq NH3, and add indicator to the HCl. Then add small volumes of aq NH3 dropwise from the beaker until endpoint is reached and HCL is neutralized, that is when indicator colour change from red to orange. Note the volume of aq NH3 for the sample used. Repeat this procedure for the remaining two samples of aq NH3. The sample of which the least volume is used to neutralize is the sample with the highest concentration and hence the best cleaner.
NOTE: THESE ARE JUST MY ANSWERS, IT IS NOT NECESSARY THAT ALL OF THEM ARE CORRECT