Question

A 1.0 M H2S solution has a pH = 3.75 at equilibrium. What is the value of Ka?

3.16 × 10−21

3.16 × 10−8

8.89 × 10−5

8.89 × 10−8

Answer 1

i know its not a or c

Answer 2

\(\sf \huge K_A=\dfrac{[H_3O^+][HS^-]}{[H_2S]}\)

the pH gives you \([H_3O^+]\) which is equal to \([HS^-]\)

Answer 3

btw, you might wanna make an ICE table for this

Answer 4

so i would set it up like this?