Question

When equal volumes of the following solutions are mixed, precipitation of AgCl ($K_{sp}$ = 1.8×10⁻¹⁰) will occur only with(a) 10⁻⁴ M (Ag⁺) and 10⁻⁴ M (Cl⁻)(b) 10⁻⁵ M (Ag⁺) and 10⁻⁵ M (Cl⁻)(c) 10⁻⁶ M (Ag⁺) and 10⁻⁶ M (Cl⁻)(d) 10⁻¹⁰ M (Ag⁺) and 10⁻¹⁰ M (Cl⁻)

Answer 1

Answer:

a) 10⁻⁴ M (Ag⁺) and 10⁻⁴ M (Cl⁻) is the correct answer.

Explanation:

Given data:

When equal volumes of the some solutions are mixed, precipitation of AgCl will occur

K{sp} = 1.8×10⁻¹⁰

When two solutions are mixed having equal volumes, the concentrated will be reduced.

It will become half of the initial solution.

Also, AgCl will precipate only when

[Ag+][Cl-] > Ksp

Hence we will check all the options

a)

[Ag+]= 10^-4/2 M

[Cl-] = 10^-4/2 M

[Ag+][Cl-] = 10^-4/2 M*10^-4/2 M

= 10^-8/4

= 2.5*10^-9

Which is greater than Ksp

Thus (a) is the correct answer

Thus 10⁻⁴ M (Ag⁺) and 10⁻⁴ M (Cl⁻) is the correct answer.