Lab Manual For Zumdahl/zumdahl's Chemistry, 9th
Lab Manual For Zumdahl/zumdahl's Chemistry, 9th
9th Edition
ISBN: 9781285692357
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 4, Problem 93AE

Using the general solubility rules given in Table 6-1. name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions.

a. chloride ion

b. calcium ion

c. iron(III) ion

d. sulfate ion

e. mercury(I) ion, Hg22+

f. silver ion

a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Chloride: AgNO3,Pb(NO3)2andHg2(NO3)2 forms precipitate with Cl- . The net ionic equations are

Ag+(aq)+Cl-(aq)AgCl(s)Pb2+(aq)+2Cl-(aq)PbCl2(s)Hg22+(aq)+2Cl-(aq)Hg2Cl2(s)

Explanation of Solution

To name three reagents that precipitates with Cl- ion.

The three reagents that precipitates chlorine ion are AgNO3,Pb(NO3)2andHg2(NO3)2 .

AgNO3 on reaction with salt of Chloride gives a precipitate of Silver chloride, that’s insoluble salt by rule 3. The net ionic equation can be given as,

Ag+(aq)+Cl-(aq)AgCl(s)

Pb(NO3)2 on reaction with salt of Chloride gives a precipitate of Lead chloride, that’s insoluble salt by rule 3. The net ionic equation can be given as,

Pb2+(aq)+2Cl-(aq)PbCl2(s)

Hg2(NO3)2 on reaction with salt of Chloride gives a precipitate of Mercuric chloride, that’s insoluble salt by rule 3. The net ionic equation can be given as,

Hg22+(aq)+2Cl-(aq)Hg2Cl2(s)

b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Calcium: Na2SO4,Na2CO3andNa3PO4 forms precipitate with Ca2+ . The net ionic equations are

Ca2+(aq)+SO42-(aq)CaSO4(s)Ca2+(aq)+CO32-(aq)CaCO3(s)3Ca2+(aq)+2PO43-(aq)Ca3(PO4)2(s)

Explanation of Solution

To name three reagents that precipitates with Ca2+

The three reagents that precipitate with Ca2+ are Na2SO4,Na2CO3andNa3PO4

Na2SO4 on reaction with salt of Calcium gives Calcium sulphate that is insoluble according to rule 4. The net ionic equation can be given as,

Ca2+(aq)+SO42-(aq)CaSO4(s)

Na2CO3 on reaction with salt of Calcium gives Calcium carbonate that is insoluble according to rule 6. The net ionic equation can be given as,

Ca2+(aq)+CO32-(aq)CaCO3(s)

Na3PO4 on reaction with salt of Calcium gives Calcium phosphate that is insoluble according to rule 6. The net ionic equation can be given as,

3Ca2+(aq)+2PO43-(aq)Ca3(PO4)2(s)

c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Iron (III): NaOH,Na2SandNa2CO3 forms precipitate with Fe3+ . The net ionic equations are

Fe3+(aq)+3OH-(aq)Fe(OH)3(s)2Fe3+(aq)+3S2-(aq)Fe2S3(s)2Fe3+(aq)+3CO32-(aq)Fe2(CO3)3(s)

Explanation of Solution

To name three reagents that precipitates with Iron (III)

The three reagents that precipitate with Iron (III) are NaOH,Na2SandNa2CO3 .

NaOH on reaction with salt of Iron (III) gives Iron (III) hydroxide that is insoluble according to rule 5. The net ionic equation is

Fe3+(aq)+3OH-(aq)Fe(OH)3(s)

Na2S on reaction with salt of Iron (III) gives Iron (III) sulphide that is insoluble according to rule 6. The net ionic equation is

2Fe3+(aq)+3S2-(aq)Fe2S3(s)

Na2CO3 on reaction with salt of Iron (III) gives Iron (III) carbonate that is insoluble according to rule 6. The net ionic equation is

2Fe3+(aq)+3CO32-(aq)Fe2(CO3)3(s)

d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Sulphate: BaCl2,Pb(NO3)2,Ca(NO3)2 forms precipitate with SO42- . The net ionic equations are

Ba2+(aq)+SO42-(aq)BaSO4(s)Pb2+(aq)+SO42-(aq)PbSO4(s)Ca2+(aq)+SO42-(aq)CaSO4(s)

Explanation of Solution

To name three reagents that precipitates with Sulphate

The three reagents that precipitate with Sulphate are BaCl2,Pb(NO3)2,Ca(NO3)2

BaCl2 when treated with a salt of Sulphate gives a precipitate of Barium sulphate that is insoluble according to rule 4. The net ionic equation is

Ba2+(aq)+SO42-(aq)BaSO4(s)

Pb(NO3)2 when treated with a salt of Sulphate gives a precipitate of Lead sulphate that is insoluble according to rule 4. The net ionic equation is

Pb2+(aq)+SO42-(aq)PbSO4(s)

Ca(NO3)2 on reaction with salt of Sulphate gives Calcium sulphate that is insoluble according to rule 4. The net ionic equation can be given as,

Ca2+(aq)+SO42-(aq)CaSO4(s)

e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Mercury (I): Na2SO4,NaClandNaI forms precipitate with Hg22+ . The net ionic equations are

           Hg22+(aq)+SO42-(aq)Hg2SO4(s)Hg22+(aq)+2Cl-(aq)Hg2Cl2(s)Hg22+(aq)+2I-(aq)Hg2I2(s)

Explanation of Solution

To name three reagents that precipitates with Mercury (I) ion

The three reagents that precipitate with Mercury (I) ion are Na2SO4,NaClandNaI

Na2SO4 on treatment with salt of Mercury (I) ion gives Mercury sulphate that is insoluble according to rule 4. The net ionic equation is,

Hg22+(aq)+SO42-(aq)Hg2SO4(s)

NaCl on treatment with salt of Mercury (I) ion gives Mercury chloride that is insoluble according to rule 3. The net ionic equation is,

Hg22+(aq)+2Cl-(aq)Hg2Cl2(s)

NaI on treatment with salt of Mercury (I) ion gives Mercury iodide that is insoluble according to rule 3. The net ionic equation is,

Hg22+(aq)+2I-(aq)Hg2I2(s)

f)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The reagent that helps in the formation of precipitate with their net ionic equation has to be written.

Concept introduction: Salts are formed by the neutralization reaction of acid and base.

The rules for salts to be soluble in water are as follows

  1. 1. Most of the nitrate salts are soluble
  2. 2. Salts containing the cation as alkali metal such as Sodium, Magnesium, Rubidium etc and Ammonium are said to be water soluble.
  3. 3. Salts of Bromide, Chloride and iodide are said to be water soluble except in case of cations such as silver, lead and mercury.
  4. 4. Most of the Sulphate salts are soluble except Barium sulphate, Mercury sulphate, Lead sulphate and Calcium sulphate.
  5. 5. Most of the Hydroxides are sparingly soluble except Sodium hydroxide and Potassium hydroxide.
  6. 6. Most of the Sulphide, Carbonate, Chromates and Phosphates are less soluble except those include in the rule 2.

Answer to Problem 93AE

Silver: NaBr,Na2CrO4andNa3PO4 forms precipitate with Ag+ . The net ionic equations are

Ag+(aq)+Br-(aq)AgBr(s)2Ag+(aq)+CrO42-(aq)Ag2CrO4(s)3Ag+(aq)+PO43-Ag3PO4(s)

Explanation of Solution

To name three reagents that precipitates with Silver

The three reagents that precipitate with Silver are NaBr,Na2CrO4andNa3PO4

NaBr on treatment with salt of Silver gives Silver bromide that is insoluble according to rule 3. The net ionic equation is,

Ag+(aq)+Br-(aq)AgBr(s)

Na2CrO4 on treatment with salt of Silver gives Silver chromate that is insoluble according to rule 6. The net ionic equation is,

2Ag+(aq)+CrO42-(aq)Ag2CrO4(s)

Na3PO4 on treatment with salt of Silver gives Silver phosphate that is insoluble according to rule 6. The net ionic equation is,

3Ag+(aq)+PO43-Ag3PO4(s)

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Chapter 4 Solutions

Lab Manual For Zumdahl/zumdahl's Chemistry, 9th

Ch. 4 - Assume you have a highly magnified view of a...Ch. 4 - You have a solution of table salt in water. What...Ch. 4 - You have a sugar solution (solution A) with...Ch. 4 - You add an aqueous solution of lead nitrate to an...Ch. 4 - Order the following molecules from lowest to...Ch. 4 - Why is it that when something gains electrons, it...Ch. 4 - Consider separate aqueous solutions of HCl and...Ch. 4 - Prob. 8ALQCh. 4 - Prob. 9ALQCh. 4 - The exposed electrodes of a light bulb are placed...Ch. 4 - Differentiate between what happens when the...Ch. 4 - A typical solution used in general chemistry...Ch. 4 - Prob. 15QCh. 4 - A student wants to prepare 1.00 L of a 1.00-M...Ch. 4 - List the formulas of three soluble bromide salts...Ch. 4 - When 1.0 mole of solid lead nitrate is added to...Ch. 4 - What is an acid and what is a base? 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A...Ch. 4 - A mixture contains only NaCl and Fe(NO3)3. A...Ch. 4 - A student added 50.0 mL of an NaOH solution to...Ch. 4 - Some of the substances commonly used in stomach...Ch. 4 - Acetylsalicylic acid is the active ingredient in...Ch. 4 - When hydrochloric acid reacts with magnesium...Ch. 4 - A 2.20-g sample of an unknown acid (empirical...Ch. 4 - Carminic acid, a naturally occurring red pigment...Ch. 4 - Chlorisondamine chloride (C14H20Cl6N2) is a drug...Ch. 4 - Saccharin (C7H5NO3S) is sometimes dispensed in...Ch. 4 - Douglasite is a mineral with the formula 2KC1...Ch. 4 - Many oxidationreduction reactions can be balanced...Ch. 4 - The blood alcohol (C2H5OH) level can be determined...Ch. 4 - Calculate the concentration of all ions present...Ch. 4 - A solution is prepared by dissolving 0.6706 g...Ch. 4 - For the following chemical reactions, determine...Ch. 4 - What volume of 0.100 M NaOH is required to...Ch. 4 - Prob. 114CWPCh. 4 - A 450.0-mL sample of a 0.257-M solution of silver...Ch. 4 - The zinc in a 1.343-g sample of a foot powder was...Ch. 4 - A 50.00-mL sample of aqueous Ca(OH)2 requires...Ch. 4 - When organic compounds containing sulfur are...Ch. 4 - Assign the oxidation state for the element Listed...Ch. 4 - A 10.00-g sample consisting of a mixture of sodium...Ch. 4 - The units of parts per million (ppm) and parts per...Ch. 4 - In the spectroscopic analysis of many substances,...Ch. 4 - In most of its ionic compounds, cobalt is either...Ch. 4 - Polychlorinated biphenyls (PCBs) have been used...Ch. 4 - Consider the reaction of 19.0 g of zinc with...Ch. 4 - A mixture contains only sodium chloride and...Ch. 4 - Prob. 127CPCh. 4 - Zinc and magnesium metal each react with...Ch. 4 - You made 100.0 mL of a lead(II) nitrate solution...Ch. 4 - Consider reacting copper(II) sulfate with iron....Ch. 4 - Consider an experiment in which two burets, Y and...Ch. 4 - Complete and balance each acid-base reaction. a....Ch. 4 - What volume of 0.0521 M Ba(OH)2 is required to...Ch. 4 - A 10.00-mL sample of sulfuric acid from an...Ch. 4 - A 0.500-L sample of H2SO4 solution was analyzed by...Ch. 4 - A 6.50-g sample of a diprotic acid requires 137.5...Ch. 4 - Citric acid, which can be obtained from lemon...Ch. 4 - Prob. 138CPCh. 4 - It took 25.06 0.05 mL of a sodium hydroxide...Ch. 4 - Prob. 140IPCh. 4 - In a 1-L beaker, 203 mL of 0.307 M ammonium...Ch. 4 - Prob. 142IPCh. 4 - The unknown acid H2X can be neutralized completely...Ch. 4 - Three students were asked to find the identity of...Ch. 4 - You have two 500.0-mL aqueous solutions. 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