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i was able to understand it but i wasnt able to solve it (the third part) ~sorry; was not much help~its q. 3d
Can you also solve that question of pka of on2006 when you knew the year
(i) they asked us the pH, for that we will dissociate the acid and form an equation
CH3CH2COOH -----------> CH3CH2COO- + H+
we use this equation in in the formula Ka=[CH3CH2COO-]x[H+]/[CH3CH2COOH]
we have the conc. for [CH3CH2COOH] = 0.5 and Ka = 1.34 x 10^-5
since we have only one H+ and one rest of the molecule CH3CH2COO-, we can assume that they will have equal concentrations! so we will take them as "x"
equating everything:
1.34 x 10^-5 = [x][x]/[0.5]
1.34 x 10^-5 x [0.5] = [x]^2
take square root on both sides and you will get
[x] = 2.6 x 10^-3
now use this conc. in the equation pH= -log[H+]
you will get 2.6 pH
(ii) our equation will be:
NaOH + CH3CH2COOH ---------> [CH3CH2COO-Na+] + H2O
1 : 1 ----------> 1 : 1
0.03 : 0.05 ----------> 0.03 : -
~this part is not asked, it's related to the next part~
(iii) they first found out the no. of moles of the acid, by using it's concentration and volume, we got, 0.5 x 0.1 = 0.05 mol
according to our equation the mole ratio between them is of [1:1] and they already gave us the moles of NaOH as 0.03 mol
0.05 was the no. of moles present in our solution and the no. that reacted with the NaOH was 0.03 (since our acid:base was 1:1) so we subtract them, 0.05-0.03 = 0.02 mol
0.02 mol is the amount of acid left and the 0.03 mol is used up to make sodium propanoate
in this question the concept of excess moles is applied!! the acid has to be in excess or it will all be used up and neutralized, base on the other hand will be all used up will be 100% converted to salt, sodium prppanoate, thus our no. of moles for NaOH = no. of moles of sodium proponoate
thus our sodium proponate is 0.03 mol ~do you get it or is it starting to get confusing?~
(iv) in this part we use two equations, pKa = -logKa -----> eq.1 and the equation for the pH of buffer
pH = pKa + log([salt]/[acid])------> eq.2.................||in case of a base buffer the equation changes pH = (Kw - pKb) + log([base]/[salt]), ours is an acid buffer so we dont need this one right now||
use the eq.1 to find pKa = -log[ 1.34 x 10^-5] = 4.87,
equate it in eq.2
pH = 4.87 + log([0.03]/[0.02]) = 5.046
that will be all
as for that previous qustion i solved it just recently so i'll try to look for it again and tell you when i find the ans! inshallah!