Question

The solubility of a salt of weak acid (ab) at ph 3 is y×10–3 mol l−1. The value of y is ____. (given that the value of solubility product of ab (ksp) = 2×10–10 and the value of ionization constant of hb (ka) = 1×10–8 ) askiitians

Answer 1

Hey Dear,

● Answer -

y = 4.47

◆ Explanation -

# Given -

Ka = 1×10^8

Ksp = 2×10^-10

pH = 3

# Solution -

Hydrogen ion conc of compound is calculated by -

pH = -log[H+]

3 = -log[H+]

[H+] = 10^-3

Solubility of given salt is calculated by -

s = √[Ksp([H+]/Ka+1)]

s = √[2×10^-10(10^-3/10^8+1)]

s = 4.47×10^-3 /mol

Therefore, value of y iz 4.47.

Hope this helped you.