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Chapter 16: Problem 4

Write the equilibrium equations on which the following \(K_{s p}\) expressions are based. (a) \(\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{CO}_{3}{ }^{2-}\right]\) (b) \(\left[\mathrm{Co}^{3+}\right]\left[\mathrm{OH}^{-}\right]^{3}\) (c) \(\left[\mathrm{Ag}^{+}\right]^{2}\left[\mathrm{~S}^{2-}\right]\) (d) \(\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{Cl}^{-}\right]^{2}\)

Short Answer

Expert verified
Question: Write the equilibrium equations for the following solubility product constant expressions: a) Ksp = [Ca²⁺][CO₃²⁻] b) Ksp = [Co³⁺][OH⁻]³ c) Ksp = [Ag⁺]²[S²⁻] d) Ksp = [Pb²⁺][Cl⁻]² Answer: a) CaCO₃ ⇌ Ca²⁺ + CO₃²⁻ b) Co(OH)₃ ⇌ Co³⁺ + 3OH⁻ c) Ag₂S ⇌ 2Ag⁺ + S²⁻ d) PbCl₂ ⇌ Pb²⁺ + 2Cl⁻

Step by step solution

01

(a) Identify the chemical species

We have two chemical species here: \(\mathrm{Ca^{2+}}\) and \(\mathrm{CO_3^{2-}}\). These ions are formed through the dissociation of calcium carbonate (CaCO3).
02

(a) Write the dissociation reaction

The dissociation reaction of calcium carbonate (CaCO3) is given by: \(\mathrm{CaCO_3} \leftrightarrows \mathrm{Ca^{2+}} + \mathrm{CO}_{3}^{2-}\)
03

(a) Write the equilibrium equation

The equilibrium equation for this reaction is: Ksp = \(\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{CO}_{3}{ }^{2-}\right]\)
04

(b) Identify the chemical species

We have two chemical species here: \(\mathrm{Co^{3+}}\) and \(\mathrm{OH^-}\). These ions are formed through the dissociation of cobalt(III) hydroxide (Co(OH)3).
05

(b) Write the dissociation reaction

The dissociation reaction of cobalt(III) hydroxide (Co(OH)3) is given by: \(\mathrm{Co(OH)}_3 \leftrightarrows \mathrm{Co^{3+}} + 3\mathrm{OH^-}\)
06

(b) Write the equilibrium equation

The equilibrium equation for this reaction is: Ksp = \(\left[\mathrm{Co}^{3+}\right]\left[\mathrm{OH}^{-}\right]^{3}\)
07

(c) Identify the chemical species

We have two chemical species here: \(\mathrm{Ag^+}\) and \(\mathrm{S^{2-}}\). These ions are formed through the dissociation of silver(I) sulfide (Ag2S).
08

(c) Write the dissociation reaction

The dissociation reaction of silver(I) sulfide (Ag2S) is given by: \(\mathrm{Ag}_2\mathrm{S} \leftrightarrows 2\mathrm{Ag^+} + \mathrm{S}^{2-}\)
09

(c) Write the equilibrium equation

The equilibrium equation for this reaction is: Ksp = \(\left[\mathrm{Ag}^{+}\right]^{2}\left[\mathrm{~S}^{2-}\right]\)
10

(d) Identify the chemical species

We have two chemical species here: \(\mathrm{Pb^{2+}}\) and \(\mathrm{Cl^-}\). These ions are formed through the dissociation of lead(II) chloride (PbCl2).
11

(d) Write the dissociation reaction

The dissociation reaction of lead(II) chloride (PbCl2) is given by: \(\mathrm{PbCl}_2 \leftrightarrows \mathrm{Pb^{2+}} + 2\mathrm{Cl^-}\)
12

(d) Write the equilibrium equation

The equilibrium equation for this reaction is: Ksp = \(\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{Cl}^{-}\right]^{2}\)

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Most popular questions from this chapter

Solid lead nitrate is added to a solution that is \(0.020 \mathrm{M}\) in \(\mathrm{OH}^{-}\) and \(\mathrm{SO}_{4}^{2-}\). Addition of the lead nitrate does not change the volume of the solution. (a) Which compound, \(\mathrm{PbSO}_{4}\) or \(\mathrm{Pb}(\mathrm{OH})_{2}\left(K_{s p}=2.8 \times 10^{-16}\right)\), will precipitate first? (b) What is the \(\mathrm{pH}\) of the solution when \(\mathrm{PbSO}_{4}\) first starts to precipitate?

Water from a well is found to contain \(3.0 \mathrm{mg}\) of calcium ion per liter. If \(0.50 \mathrm{mg}\) of sodium sulfate is added to one liter of the well water without changing its volume, will a precipitate form? What should \(\left[\mathrm{SO}_{4}{ }^{2-}\right]\) be to just start precipitation?

Consider the insoluble salts \(\mathrm{JQ} \mathrm{K}_{2} \mathrm{R}, \mathrm{L}_{2} \mathrm{~S}_{3}, \mathrm{MT}_{2}\), and \(\mathrm{NU}_{3}\). They are formed from the metal ions \(\mathrm{J}^{+}, \mathrm{K}^{+}, \mathrm{L}^{3+}, \mathrm{M}^{2+}\), and \(\mathrm{N}^{3+}\) and the nonmetal ions \(\mathrm{Q}^{-}, \mathrm{R}^{2-}, \mathrm{S}^{2-}, \mathrm{T}^{-}\), and \(\mathrm{U}^{-}\). All the salts have the same \(K_{\text {sp }}, 1 \times 10^{-10}\), at \(25^{\circ} \mathrm{C}\). (a) Which salt has the highest molar solubility? (b) Does the salt with the highest molar solubility have the highest solubility in g salt/100 g water? (c) Can the solubility of each salt in \(\mathrm{g} / 100 \mathrm{~g}\) water be determined from the information given? If yes, calculate the solubility of each salt in \(\mathrm{g} / 100 \mathrm{~g}\) water. If no, why not?

Write a net ionic equation for the reaction with ammonia by which (a) silver chloride dissolves. (b) aluminum ion forms a precipitate. (c) copper(II) forms a complex ion.

Calculate the solubility (in grams per liter) of magnesium hydroxide in the following. (a) pure water (b) \(0.041 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) (c) \(0.0050 \mathrm{MgCl}_{2}\)
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