Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 6, Problem 95AE

a)

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.

a)

Expert Solution
Check Mark

Answer to Problem 95AE

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)

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.

b)

Expert Solution
Check Mark

Answer to Problem 95AE

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)

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.

c)

Expert Solution
Check Mark

Answer to Problem 95AE

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)

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.

d)

Expert Solution
Check Mark

Answer to Problem 95AE

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)

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.

e)

Expert Solution
Check Mark

Answer to Problem 95AE

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)

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.

f)

Expert Solution
Check Mark

Answer to Problem 95AE

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 6 Solutions

Chemistry: An Atoms First Approach

Ch. 6 - Prob. 2ALQCh. 6 - You have a sugar solution (solution A) with...Ch. 6 - Prob. 4ALQCh. 6 - Prob. 5ALQCh. 6 - Prob. 6ALQCh. 6 - Consider separate aqueous solutions of HCl and...Ch. 6 - Prob. 8ALQCh. 6 - Prob. 9ALQCh. 6 - The exposed electrodes of a light bulb are placed...Ch. 6 - Differentiate between what happens when the...Ch. 6 - Consider the following electrostatic potential...Ch. 6 - Prob. 15QCh. 6 - A typical solution used in general chemistry...Ch. 6 - Prob. 17QCh. 6 - A student wants to prepare 1.00 L of a 1.00-M...Ch. 6 - List the formulas of three soluble bromide salts...Ch. 6 - When 1.0 mole of solid lead nitrate is added to...Ch. 6 - What is an acid and what is a base? An acid-base...Ch. 6 - A student had 1.00 L of a 1.00-M acid solution....Ch. 6 - Prob. 23QCh. 6 - Prob. 24QCh. 6 - Prob. 25ECh. 6 - Match each name below with the following...Ch. 6 - Prob. 27ECh. 6 - Commercial cold packs and hot packs are available...Ch. 6 - Calculate the molarity of each of these solutions....Ch. 6 - A solution of ethanol (C2H5OH) in water is...Ch. 6 - Calculate the concentration of all ions present in...Ch. 6 - Prob. 32ECh. 6 - Prob. 33ECh. 6 - Prob. 34ECh. 6 - Prob. 35ECh. 6 - Prob. 36ECh. 6 - Prob. 37ECh. 6 - Prob. 38ECh. 6 - A solution is prepared by dissolving 10.8 g...Ch. 6 - A solution was prepared by mixing 50.00 mL of...Ch. 6 - Calculate the sodium ion concentration when 70.0...Ch. 6 - Suppose 50.0 mL of 0.250 M CoCl2 solution is added...Ch. 6 - Prob. 43ECh. 6 - A stock solution containing Mn2+ ions was prepaned...Ch. 6 - On the basis of the general solubility rules given...Ch. 6 - On the basis of the general solubility rules given...Ch. 6 - When the following solutions are mixed together,...Ch. 6 - When the following solutions are mixed together,...Ch. 6 - For the reactions in Exercise 47, write the...Ch. 6 - For the reactions in Exercise 48, write the...Ch. 6 - Write the balanced formula and net ionic equation...Ch. 6 - Give an example how each of the following...Ch. 6 - Write net ionic equations for the reaction, if...Ch. 6 - Write net ionic equations for the reaction, if...Ch. 6 - Prob. 55ECh. 6 - Prob. 56ECh. 6 - What mass of Na2CrO4 is required to precipitate...Ch. 6 - What volume of 0.100 M Na3PO4 is required to...Ch. 6 - What mass of solid aluminum hydroxide can be...Ch. 6 - What mass of barium sulfate can be produced when...Ch. 6 - What mass of solid AgBr is produced when 100.0 mL...Ch. 6 - What mass of silver chloride can be prepared by...Ch. 6 - A 100.0-mL aliquot of 0.200 M aqueous potassium...Ch. 6 - A 1.42-g sample of a pure compound, with formula...Ch. 6 - You are given a 1.50-g mixture of sodium nitrate...Ch. 6 - Write the balanced formula, complete ionic, and...Ch. 6 - Write the balanced formula, complete ionic, and...Ch. 6 - Write the balanced formula equation for the...Ch. 6 - Prob. 70ECh. 6 - What volume of each of the following acids will...Ch. 6 - Prob. 72ECh. 6 - Hydrochloric acid (75.0 mL of 0.250 M) is added to...Ch. 6 - Prob. 74ECh. 6 - A 25.00-mL sample of hydrochloric acid solution...Ch. 6 - A 10.00-mL sample of vinegar, an aqueous solution...Ch. 6 - What volume of 0.0200 M calcium hydroxide is...Ch. 6 - A 30.0-mL sample of an unknown strong base is...Ch. 6 - A student titrates an unknown amount of potassium...Ch. 6 - The concentration of a certain sodium hydroxide...Ch. 6 - Assign oxidation states for all atoms in each of...Ch. 6 - Assign the oxidation state for nitrogen in each of...Ch. 6 - Prob. 84ECh. 6 - Specify which of the following are...Ch. 6 - Specify which of the following equations represent...Ch. 6 - Consider the reaction between sodium metal and...Ch. 6 - Consider the reaction between oxygen (O2) gas and...Ch. 6 - Balance each of the following oxidationreduction...Ch. 6 - Balance each of the following oxidationreduction...Ch. 6 - Prob. 91AECh. 6 - Prob. 92AECh. 6 - Prob. 93AECh. 6 - Prob. 94AECh. 6 - Prob. 95AECh. 6 - Consider a 1.50-g mixture of magnesium nitrate and...Ch. 6 - A 1.00-g sample of an alkaline earth metal...Ch. 6 - A mixture contains only NaCl and Al2(SO4)3. A...Ch. 6 - The thallium (present as Tl2SO4) in a 9.486-g...Ch. 6 - Prob. 100AECh. 6 - A student added 50.0 mL of an NaOH solution to...Ch. 6 - Prob. 102AECh. 6 - Acetylsalicylic acid is the active ingredient in...Ch. 6 - When hydrochloric acid reacts with magnesium...Ch. 6 - A 2.20-g sample of an unknown acid (empirical...Ch. 6 - Carminic acid, a naturally occurring red pigment...Ch. 6 - Chlorisondamine chloride (C14H20Cl6N2) is a drug...Ch. 6 - Prob. 108AECh. 6 - Prob. 109AECh. 6 - Many oxidationreduction reactions can be balanced...Ch. 6 - Prob. 111AECh. 6 - Calculate the concentration of all ions present...Ch. 6 - A solution is prepared by dissolving 0.6706 g...Ch. 6 - For the following chemical reactions, determine...Ch. 6 - What volume of 0.100 M NaOH is required to...Ch. 6 - Prob. 116CWPCh. 6 - A 450.0-mL sample of a 0.257-M solution of silver...Ch. 6 - The zinc in a 1.343-g sample of a foot powder was...Ch. 6 - Prob. 119CWPCh. 6 - When organic compounds containing sulfur are...Ch. 6 - Prob. 121CWPCh. 6 - Prob. 122CPCh. 6 - The units of parts per million (ppm) and parts per...Ch. 6 - Prob. 124CPCh. 6 - Prob. 125CPCh. 6 - Prob. 126CPCh. 6 - Consider the reaction of 19.0 g of zinc with...Ch. 6 - A mixture contains only sodium chloride and...Ch. 6 - Prob. 129CPCh. 6 - Prob. 130CPCh. 6 - Prob. 131CPCh. 6 - Consider reacting copper(II) sulfate with iron....Ch. 6 - Prob. 133CPCh. 6 - Prob. 134CPCh. 6 - What volume of 0.0521 M Ba(OH)2 is required to...Ch. 6 - A 10.00-mL sample of sulfuric acid from an...Ch. 6 - Prob. 137CPCh. 6 - A 6.50-g sample of a diprotic acid requires 137.5...Ch. 6 - Citric acid, which can be obtained from lemon...Ch. 6 - Prob. 140CPCh. 6 - Prob. 141CPCh. 6 - Tris(pentatluorophenyl)borane, commonly known by...Ch. 6 - In a 1-L beaker, 203 mL of 0.307 M ammonium...Ch. 6 - The vanadium in a sample of ore is converted to...Ch. 6 - The unknown acid H2X can be neutralized completely...Ch. 6 - Three students were asked to find the identity of...Ch. 6 - You have two 500.0-mL aqueous solutions. Solution...
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