The solubility product of Zn(OH)2 is 10^-14 at 25^∘ C. What would be the concentration Zn^+2 ion

Name: Problem 73, Chapter 7: Advanced Problems in Physical Chemistry for Competitive Examinations
Uploaded: 2021-11-13T11:21:35-08:00
Duration: 1 min 24 s
Channel: Manik Pulyani
Description: The solubility product of Zn(OH)2 is 10^-14 at 25^∘ C. What would be the concentration Zn^+2 ion in 0.1 M-NH4 OH solution which is 50 % ionized? (a) 2 ×10 (b) 4 ×10^-12 (c) 4 ×10^-8 (d) 2 ×10^-11

step 1 Okay, for this question we have balanced chemical equations as 2 positive quers plus twice of hy

Question

The solubility product of $\mathrm{Zn}(\mathrm{OH})_{2}$ is $10^{-14}$ at $25^{\circ} \mathrm{C}$. What would be the concentration $\mathrm{Zn}^{+2}$ ion in $0.1 \mathrm{M}-\mathrm{NH}_{4} \mathrm{OH}$ solution which is $50 \%$ ionized? (a) $2 \times 10$ (b) $4 \times 10^{-12}$ (c) $4 \times 10^{-8}$ (d) $2 \times 10^{-11}$

   The solubility product of $\mathrm{Zn}(\mathrm{OH})_{2}$ is $10^{-14}$ at $25^{\circ} \mathrm{C}$. What would be the concentration $\mathrm{Zn}^{+2}$ ion in $0.1 \mathrm{M}-\mathrm{NH}_{4} \mathrm{OH}$ solution
which is $50 \%$ ionized?
(a) $2 \times 10$
(b) $4 \times 10^{-12}$
(c) $4 \times 10^{-8}$
(d) $2 \times 10^{-11}$

Advanced Problems in Physical Chemistry for Competitive Examinations

Neeraj Kumar 2015 Edition

Chapter 7, Problem 73

Instant Answer

Solved by Expert Manik Pulyani

11/13/2021

Step 1

Since the NH4OH solution is 50% ionized, the concentration of OH- ions is 0.5 * 0.1 M = 0.05 M. Show more…

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The solubility product of $\mathrm{Zn}(\mathrm{OH})_{2}$ is $10^{-14}$ at $25^{\circ} \mathrm{C}$. What would be the concentration $\mathrm{Zn}^{+2}$ ion in $0.1 \mathrm{M}-\mathrm{NH}_{4} \mathrm{OH}$ solution which is $50 \%$ ionized? (a) $2 \times 10$ (b) $4 \times 10^{-12}$ (c) $4 \times 10^{-8}$ (d) $2 \times 10^{-11}$

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Key Concepts

Solubility Product (Ksp)

The solubility product is an equilibrium constant that applies to the dissolution process of sparingly soluble compounds. It quantifies the product of the ion concentrations each raised to the power of its stoichiometric coefficient at equilibrium. In precipitate formation, Ksp allows us to determine whether a solid will form by comparing the reaction quotient with the Ksp value.

Partial Ionization of Weak Bases

Weak bases, such as ammonium hydroxide, do not fully dissociate in aqueous solution; instead, they ionize partially. The degree of ionization, expressed as a percentage, determines the effective concentration of hydroxide ions available in solution. This effective concentration directly influences equilibrium processes like the precipitation reaction involving metal hydroxides when combined with the solubility product concept.

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