In the qualitative cation analysis for 1.00 mL of the saturated PbCl 2 ( a q ) at 25 ∘ C , the presence of sufficient Pb 2+ to produce a precipitate of PbCrO 4 (s) needs to be shown. Concept introduction: When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb 2+ , Hg 2 2+ , Ag + . To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing. PbCl 2 is more soluble than other two precipitates; Hg 2 Cl 2 and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl 2 precipitate dissolves in hot water and only Hg 2 Cl 2 and AgCl remains as precipitates. Presence of Pb 2+ can be identified by adding a CrO 4 2- solution. When Pb 2+ reacts with CrO 4 2- , it forms a yellow color precipitate PbCrO 4 .

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Question

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

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Answer 2

Question

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

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Answer 3

Question

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

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Answer 4

Question

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

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Answer 5

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

Answer 6

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

Answer 7

Chapter 18, Problem 64E

Interpretation Introduction

Interpretation:

In the qualitative cation analysis for 1.00 mL of the saturated PbCl2(aq) at 25 ∘C, the presence of sufficient Pb²⁺to produce a precipitate of PbCrO₄(s) needs to be shown.

Concept introduction:

When a solution is treated with HCl and a precipitate is formed, one or more of these cations may be present in the solution; Pb²⁺, Hg₂²⁺, Ag⁺. To identify these individual cations, the precipitate is filtered and the dried precipitate is further subjected to testing.

PbCl₂ is more soluble than other two precipitates; Hg₂Cl₂ and AgCl. When the temperature increases, solubility of a solid increases. So, when the precipitate obtained from group 1 analysis is washed with hot water, PbCl₂ precipitate dissolves in hot water and only Hg₂Cl₂ and AgCl remains as precipitates. Presence of Pb²⁺ can be identified by adding a CrO₄^2- solution. When Pb²⁺ reacts with CrO₄^2-, it forms a yellow color precipitate PbCrO₄.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 18 - Write K10 expressions for the following...Ch. 18 - Write solubility equilibrium equations that are...Ch. 18 - The following K10 values ate found in a handbook....Ch. 18 - Calculate the aqueous solubility, in moles per...Ch. 18 - Prob. 5E Ch. 18 - Which of the following saturated aqueous solutions...Ch. 18 - Fluoridated drinking water contains about 1 part...Ch. 18 - In the qualitative cation analysis procedure, Bi2+...Ch. 18 - Prob. 9E Ch. 18 - A 725mL sample of a saturated solution of calcium...

Solution Summary: The author analyzes the presence of Pb 2+ in a saturated solution of HCl, and explains how it is more soluble than other two precipitates.

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Chapter 18 Solutions