General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 17, Problem 17.50QP

(a)

Interpretation Introduction

Interpretation:

From the given data, the molar solubility of PbBr2 dissolved in various solutions have to be calculated.

Concept introduction:

  • Molar solubility is defined as amount of solute that can be dissolved in one litre of solution before it attains saturation.
  • Solubility of a compound is expressed as concentration of its ions in saturated solution.
  • The solubility product constant (Ksp) is defined as the equilibrium between compound and its ions in an aqueous solution.
  • Solubility product is the multiplication of concentration of dissolved ion,  raised to the power of coefficients.
  • Ionic compound A3B Ksp= [A]3[B].
  • When the concentration of one of the ions of a chemical solution got higher, it reacts with counter charged ions and precipitated out as salt till the ion product equals solubility product is called common ion effect.

To calculate: The molar solubility of PbBr2 in pure water.

(a)

Expert Solution
Check Mark

Answer to Problem 17.50QP

The molar solubility of PbBr2 in pure water is 1.3×10-2M

Explanation of Solution

Given,

The KspofPbBr2is8.9×10-6

Strength of KBris0.20M

Strength of Pb(NO3)2is0.20M

  PbBr2(s)  Pb2+(aq) + 2Br-(aq)Initial concentration (M):                   0          0 Change in concentration (M):  s                +s             +2sEquilibrium concentration(M):           s+2ssismolarsolubilityKsp = [Pb2+][Br-]28.9×10-6(s)(2s)2 8.9×10-6=4s3 s=molar solubility = 0.013 Mor1.3×10-2M

The molar solubility can be calculated using solubility product constant.  From the concentrations of lead and bromine ions obtained in equilibrium table and substituting in solubility product expression, the molar solubility is determined.

(b)

Interpretation Introduction

Interpretation:

From the given data, the molar solubility of PbBr2 dissolved in various solutions have to be calculated.

Concept introduction:

  • Molar solubility is defined as amount of solute that can be dissolved in one litre of solution before it attains saturation.
  • Solubility of a compound is expressed as concentration of its ions in saturated solution.
  • The solubility product constant (Ksp) is defined as the equilibrium between compound and its ions in an aqueous solution.
  • Solubility product is the multiplication of concentration of dissolved ion,  raised to the power of coefficients.
  • Ionic compound A3B Ksp= [A]3[B].
  • When the concentration of one of the ions of a chemical solution got higher, it reacts with counter charged ions and precipitated out as salt till the ion product equals solubility product is called common ion effect.

To calculate: The molar solubility of PbBr2 in 0.20 M KBr.

(b)

Expert Solution
Check Mark

Answer to Problem 17.50QP

The molar solubility of PbBr2 in 0.20 M KBr is 2.2×10-4M

Explanation of Solution

  PbBr2(s)  Pb2+(aq) 2Br-(aq)Initial concentration (M):                   0          0 Change in concentration (M):  s              +s                +2sEquilibrium concentration(M):           s0.20+2ssismolarsolubilityKsp = [Pb2+][Br-]28.9×10-6(s)(0.20+2s)2 8.9×10-6=(s)(0.20)2s=molar solubility=2.2×10-4M

The molar solubility can be calculated using solubility product constant.  The molar solubility of PbBr2 in 0.20 M KBr is less than in pure water because of common ion (bromide ions)

(c)

Interpretation Introduction

Interpretation:

From the given data, the molar solubility of PbBr2 dissolved in various solutions have to be calculated.

Concept introduction:

  • Molar solubility is defined as amount of solute that can be dissolved in one litre of solution before it attains saturation.
  • Solubility of a compound is expressed as concentration of its ions in saturated solution.
  • The solubility product constant (Ksp) is defined as the equilibrium between compound and its ions in an aqueous solution.
  • Solubility product is the multiplication of concentration of dissolved ion,  raised to the power of coefficients.
  • Ionic compound A3B Ksp= [A]3[B].
  • When the concentration of one of the ions of a chemical solution got higher, it reacts with counter charged ions and precipitated out as salt till the ion product equals solubility product is called common ion effect.

The molar solubility of PbBr2 in 0.20 M Pb(NO3)2.

(c)

Expert Solution
Check Mark

Answer to Problem 17.50QP

The molar solubility of PbBr2 in 0.20 M Pb(NO3)2 is 3.3×10-3M

Explanation of Solution

  PbBr2(s)  Pb2+(aq) + 2Br-(aq)Initial concentration (M):0.20            0           Change in concentration (M):  -s                +s                +2sEquilibrium concentration(M):           0.20+2s+2ssismolarsolubilityKsp = [Pb2+][Br-]28.9×10-6(s)(0.20+2s)2 8.9×10-6=(0.20)(2s)2s=molar solubility=3.3×10-3M

The molar solubility can be calculated using solubility product constant.  The molar solubility of PbBr2 in 0.20 M Pb(NO3)2 is less than in pure water because of common ion (lead ions)

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Chapter 17 Solutions

General Chemistry

Ch. 17.5 - Prob. 2PECh. 17.5 - Prob. 3PECh. 17.6 - Prob. 1PECh. 17.6 - Prob. 1RCCh. 17.7 - Prob. 1PECh. 17.7 - Prob. 1RCCh. 17 - Prob. 17.1QPCh. 17 - Prob. 17.2QPCh. 17 - Prob. 17.3QPCh. 17 - 17.4 The pKbs for the bases X−, Y−, and Z− are...Ch. 17 - 17.5 Specify which of these systems can be...Ch. 17 - 17.6 Specify which of these systems can be...Ch. 17 - 17.7 The pH of a bicarbonate–carbonic acid buffer...Ch. 17 - Prob. 17.8QPCh. 17 - 17.9 Calculate the pH of the buffer system 0.15 M...Ch. 17 - 17.10 What is the pH of the buffer 0.10 M...Ch. 17 - 17.11 The pH of a sodium acetate–acetic acid...Ch. 17 - 17.12 The pH of blood plasma is 7.40. Assuming the...Ch. 17 - Prob. 17.13QPCh. 17 - Prob. 17.14QPCh. 17 - 17.16 A student wishes to prepare a buffer...Ch. 17 - Prob. 17.17QPCh. 17 - Prob. 17.18QPCh. 17 - Prob. 17.19QPCh. 17 - 17.20 A 5.00-g quantity of a diprotic acid is...Ch. 17 - Prob. 17.21QPCh. 17 - Prob. 17.22QPCh. 17 - 17.23 The diagrams shown here represent solutions...Ch. 17 - 16.38 The diagrams shown here represent solutions...Ch. 17 - 17.25 Explain how an acid-base indicator works in...Ch. 17 - 17.26 What are the criteria for choosing an...Ch. 17 - 17.27 The amount of indicator used in an acid-base...Ch. 17 - 17.28 A student carried out an acid-base titration...Ch. 17 - 17.29 Referring to Table 17.1, specify which...Ch. 17 - 17.30 The ionization constant Ka of an indicator...Ch. 17 - 17.31 Define solubility, molar solubility, and...Ch. 17 - 17.32 Why do we usually not quote the Ksp values...Ch. 17 - 17.33 Write balanced equations and solubility...Ch. 17 - Prob. 17.34QPCh. 17 - Prob. 17.35QPCh. 17 - 17.36 Silver chloride has a larger Ksp than silver...Ch. 17 - Prob. 17.38QPCh. 17 - 17.39 The molar solubility of MnCO3 is 4.2 × 10−6...Ch. 17 - Prob. 17.40QPCh. 17 - Prob. 17.41QPCh. 17 - 17.42 Using data from Table 17.2, calculate the...Ch. 17 - 17.43 What is the pH of a saturated zinc hydroxide...Ch. 17 - 17.44 The pH of a saturated solution of a metal...Ch. 17 - Prob. 17.45QPCh. 17 - 17.46 A volume of 75 mL of 0.060 M NaF is mixed...Ch. 17 - 17.47 How does a common ion affect solubility? Use...Ch. 17 - Prob. 17.48QPCh. 17 - Prob. 17.49QPCh. 17 - Prob. 17.50QPCh. 17 - Prob. 17.51QPCh. 17 - 17.52 Calculate the molar solubility of BaSO4 (a)...Ch. 17 - Prob. 17.55QPCh. 17 - Prob. 17.56QPCh. 17 - 17.57 If 2.50 g of CuSO4 are dissolved in 9.0 ×...Ch. 17 - 17.58 Calculate the concentrations of Cd2+, , and...Ch. 17 - Prob. 17.59QPCh. 17 - Prob. 17.60QPCh. 17 - Prob. 17.61QPCh. 17 - Prob. 17.62QPCh. 17 - Prob. 17.63QPCh. 17 - 16.88 In a group 1 analysis, a student adds HCl...Ch. 17 - 17.65 Both KCl and NH4Cl are white solids. Suggest...Ch. 17 - 17.66 Describe a simple test that would enable you...Ch. 17 - Prob. 17.67QPCh. 17 - Prob. 17.68QPCh. 17 - Prob. 17.69QPCh. 17 - 17.70 The pKa of the indicator methyl orange is...Ch. 17 - Prob. 17.71QPCh. 17 - Prob. 17.72QPCh. 17 - 17.73 The two curves shown here represent the...Ch. 17 - 17.74 The two curves shown here represent the...Ch. 17 - Prob. 17.75QPCh. 17 - 17.76 A solution is made by mixing exactly 500 mL...Ch. 17 - Prob. 17.77QPCh. 17 - Prob. 17.78QPCh. 17 - 17.79 For which of these reactions is the...Ch. 17 - Prob. 17.80QPCh. 17 - Prob. 17.81QPCh. 17 - Prob. 17.82QPCh. 17 - Prob. 17.83QPCh. 17 - 17.84 Find the approximate pH range suitable for...Ch. 17 - Prob. 17.85QPCh. 17 - 17.86 Which of these substances will be more...Ch. 17 - Prob. 17.87QPCh. 17 - Prob. 17.88QPCh. 17 - Prob. 17.89QPCh. 17 - Prob. 17.90QPCh. 17 - Prob. 17.91QPCh. 17 - 17.92 When a KI solution was added to a solution...Ch. 17 - Prob. 17.93QPCh. 17 - Prob. 17.94QPCh. 17 - Prob. 17.95QPCh. 17 - 17.96 Solid NaI is slowly added to a solution that...Ch. 17 - Prob. 17.97QPCh. 17 - 17.98 (a) Assuming complete dissociation and no...Ch. 17 - 17.99 Acid-base reactions usually go to...Ch. 17 - 17.100 Calculate x, the number of molecules of...Ch. 17 - Prob. 17.101QPCh. 17 - 17.102 What reagents would you employ to separate...Ch. 17 - 17.103 CaSO4 (Ksp = 2.4 × 10−5) has a larger Ksp...Ch. 17 - 17.104 How many milliliters of 1.0 M NaOH must be...Ch. 17 - Prob. 17.105QPCh. 17 - Prob. 17.106QPCh. 17 - Prob. 17.107QPCh. 17 - Prob. 17.108QPCh. 17 - Prob. 17.109QPCh. 17 - Prob. 17.111SPCh. 17 - Prob. 17.112SPCh. 17 - Prob. 17.113SPCh. 17 - Prob. 17.114SPCh. 17 - Prob. 17.115SPCh. 17 - Prob. 17.116SPCh. 17 - 17.117 The titration curve shown here represents...Ch. 17 - Prob. 17.118SP
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