Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 15, Problem 32QAP

A solution is prepared by mixing 45.00 mL of 0.022 M AgNO3 with 13.00 mL of 0.0014 M Na2CO3. Assume that volumes are additive.

(a) Will precipitation occur?

(b) Calculate [Ag+], [CO32-], [Na+], and [NO3-] after equilibrium is established.

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

Whether the reaction undergoes precipitation or not needs to be determined.

Concept introduction:

For a reaction, if ionic ( Q) product of the compound is greater than solubility product of compound, then precipitation occurs.

Answer to Problem 32QAP

The reaction undergoes precipitation.

Explanation of Solution

It is given that volume of 0.022MAgNO3 is 45.00mL.

Volume of 0.0014MNa2CO3 is 13.00mL.

Reaction of AgNO3 with Na2CO3 is as follows:

AgNO3+Na2CO3Ag2CO3+NaNO3

Totalvolumeofsolution=13mL+45 mL=58mL

Molar concentration of [Ag+] and [CO32] in 58mL solution are as follows:

[Ag+]=0.022M×45mL58mL=1.7×102M

So, [Ag+] ion concentration is 1.7×102M.

[CO32]=0.0014M×13mL58mL=3.13×104M

So, [CO32] ion concentration is 3.13×104M.

Calculate ionic product (Q) for Ag2CO3

Q=[Ag+]2[CO32]=(1.7×102)2×3.13×104=9.05×108

So, ionic product ( Q)of silver carbonate (Ag2CO3) is 9.05×108.

Solubility of silver carbonate (Ag2CO3) is 8.1×1012

Q>Solubilityproduct

So, precipitation of silver carbonate (Ag2CO3) occurs.

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

The equilibrium concentration of [Ag+],[CO32],[Na+],[NO3] needs to be determined.

Concept introduction:

The equilibrium reaction after mixing solution of AgNO3 and Na2CO3 is,

AgNO3(aq)+Na2CO3(aq)Ag2CO3(s)+2NaNO3(aq)

The molarity of solution is calculated as follows:

M=nV

Here, n is number of moles of solute and V is volume of solution in L.

Answer to Problem 32QAP

[Ag+]=0.0164M[CO32]=3.125×108M[Na+]=6.22×104M[NO3]=1.72×102M

Explanation of Solution

The equilibrium reaction after mixing solution of AgNO3 and Na2CO3 is,

AgNO3(aq)+Na2CO3(aq)Ag2CO3(s)+2NaNO3(aq)   ....... (1)

MolesofAgNO3=0.022M×45ml=0.99mol

MolesofNa2CO3=0.0014M×13ml=0.0182mol

As 0.0182 mol of Na2CO3 is completely utilized to react with 0.99 mol of AgNO3. Na2CO3 is the limiting reagent.

ICE table for equation (1) is,

2AgNO3(aq)+Na2CO3(aq)2NaNO3(aq)Initial0.990.01820Change0.03640.01820.0182Equilibrium0.95400.0182

Totalvolumeofsolution=13mL+45mL=58 mL

Equilibrium concentration of Ag ion is,

[Ag+]=0.954mol58mL=0.0164

Equilibrium concentration of NO3 ion is,

[NO3]=0.022M×45 mL58mL=1.72×102M

Equilibrium concentration of NO3 ion is,

[Na+]=0.0182mol×258mL=6.22×104M

Equilibrium concentration of CO3 ion is,

Ksp(Ag2CO3)=8×1012Ksp(Ag2CO3)=[Ag+]2[CO32]

[CO32]=Ksp(Ag2CO3)[Ag+]2=8×1012(1.6×102)2=3.125×108M

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Chapter 15 Solutions

Chemistry: Principles and Reactions

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