Asked by admin @ in Chemistry viewed by 291 People
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
Answered by admin @
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.
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