Question

2. Which compound has the highest molar solubility in neutral aqueous solution? (A) ZnS. Ksp-3x10-23 (B) Agl, Ksp 8.52x10-17 (C) BaCO, Ksp 2.58x10 ) Fe(OH)3, Ksp-2.79x10-39 (E) Pblz, Ksp 8.7x10 3. A solution contains 0.01 M Pb2+ and 0.01 M Agt What happens when Na SO(s) is added to bring SO1 to 0.01 M? (Kp(PbSO.)-1.6x10-8. Ksp(Ag SO4) 4x10.) Neither PbSO4 nor Ag SO4 precipitate (B) Both PbSO4 and Ag SO4 precipitate (C) AgaSO4 selectively precipitates. (D) PbSO4 selectively precipitates. 4. Which will change the value of Ksp for AgCI? (A) Adding Ag into the solution (B) Adding water into the solution (C) Increasing the temperature of the solution )Removing Cl from the solution (E) Increasing the pressure.

Answer 1

Question-2:-

Your answer is B

Your answer is correct

Here we see the compound are notnot bro into same number of ions but we know that the solubility product value directly propositional to the solubility of ionic components

For a

30 x 10^-24 = x^2
molar solubility = 5.4 x 10^-12 M

For b
85.2 x 10^-18= x^2
molar solubility =9.x23 10^-9 M

For c

25.8 x 10^-10= x^2
molar solubility = 5.07x 10^-5M

For d
27.9× 10^-40 = (x)(3x)^3 = 27x^4
molar solubility =1.03 x 10^- 10M

For e

87.0× 10^-10 = x^2
molar solubility = 9.3 x 10^-5 M

Question no 2

Answer is C

By addition of Na2SO4 , Ag2SO4 will form by precipitation

Because it reaction quotient will be greater than Ksp

Question 3

Answer is C

Ksp remains constant doesnot change with addition of new ion concentration .

Ksp can be changed only with change in temperature.

Thank you

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