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1a)ii)Hello! I have doubts in question 1 of this paper
http://studyguide.pk/Past Papers/CIE/International A And AS Level/9701 - Chemistry/9701_w04_qp_4.pdf
A) Why is the concentration of H2SO4 halved in q1 a (ii)??
Mark scheme: (pH = 0.70) ⇒ [H+
] = 10-0.7 = 0.20 (mol dm-3) [1]
∴ [H2
SO4] = (0.10 mol dm-3)
B) I dont understand how to solve q1 a (iii)
Mark scheme : (end point is at 34.0 cm3
(± 0.5 cm3),
so amount of H+ used = 0.2 x 25/1000 = 0.0050 mol ecf from (ii) [1]
moles of guanidine = moles of H+ = 0.0050 mol
[guanidine] = 0.005 x 1000/34.0 = 0.147 (mol dm-3) [1]
please if anybody could explain I would be very very thankful to you!!
pH = -log[H+]
0.7 = -log[H+]
-0.7 = log[H+]
10^-0.7 = [H+]
[H+] = 0.2 moldm^-3
Ratio of H2SO4 and H+ is 1 : 2
so 1 mol of H2SO4 ----> 2 mol of H+
so, how many moles of H2SO4 will be produce by 0.2 mol of H+ ? ---> crossmultiply and it will be 0.2/2 = 0.1 mol hence its halved.
iii) amount of H+ used = 0.2 * 25 * 10^-3 = 0.005 mol (When a 25.0 cm3 sample of dilute sulphuric acid was titrated against a solution of guanidine, the following titration curve was obtained.)
so now moles of B = moles of H+ used as ratio is 1 : 1 = 0.005 mol
So concentration of B = 0.005 / (34 * 10^-3) = 0.147 moldm^-3 (From graph u can read that end point is at 34cm^3)
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