[merkl]

You can work out how many moles of CO₂ gas are given off, and compare it to the equation.

[jadekathryn]

Hi, I've got my method for the titration- I'm titrating sulphuric acid and then comparing that to monobasic HCl but i'm stuck on how to show that it is actually dibasic. IS it that you need twice as much HCl in volume or the moles? I was going to work out  the molar masses of each acid used and then see if sulphuric was double hydrochloric using
Molar Mass of acid=    concentration x volume / 1000

but i don't know if this is right??? x         
                                 
 

[chocoholic4lyf]

titrate sulphuric acid with NaOH and compare this with HCl. you should see that you need twice as much NaOH to neutralise the H2SO4 then the HCl

[spy derman]

has anyone finished their plan?

[Mr. Brightside]

I haven't even started it mate 

Neither have a couple of my friends though. I think we're all doing it tomorrow, & then refining it on monday morning before the exam.

Cutting it close, i know, but we love to live on the edge & all that 

& am I the only one who has never done gas collection before? Not really any idea of how to do a method for it....

[merkl]

I've finished and handed it in. My school wanted them in crazy early.

[unileverbrand]

What apparatus do you use for the gas collection? And does anyone else have to write about making their own sodium hydroxide?

[jadekathryn]

I was talking to my teacher and apparently it is best not u compare with HCl as this doesnt give you an oppurtunity to get marks for mole calculations and that i should just use stoichiometry from "assumed results" of the titration.. so i thought as it is a 2:1 reaction i should assume the volume of acid needed to be half the volume of the NaOH (i am using 25ml) so 12.5 but then what calculations should i do? any help would be realllly appreciated im so stuck! thanks x

[chocoholic4lyf]

i hope everyone finished their planning and did good in their practical!!!