Question

Chemistry:

How do we calculate the pH of 0.1M H2S solution? Given That;

Ka1 (H2S) = 1.0x 10-7

Ka2 (H2S)= 1.3 x 10-14

Answer 1

The pH of 0.1 M H2S solution is 4

Explanation:

• K2  is much smaller than K1
• It is supposed that Hydronium ions [H3O+] will be produced in first reaction of  dissociation.

H2S + H2O - - - - - -  -> H3O+ + HS−

So,  

K1 = [H3O+] [HS] / [H2S]

Then,

K1 = [H3O+]^2 / [H2S]

[H3O+] = (√K1.[H2S])

=(√1.0×10−7×0.1)

=1.0×10−4

Now, pH = −log [H3O+] = −log[1.0×10−4]

= 4

Hence the pH of 0.1 M H2S solution is 4.

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Answer 2

Explanation:

here u go

hope it helps

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