CHEMISTRY: THE MOLECULAR NATURE OF MATTE
CHEMISTRY: THE MOLECULAR NATURE OF MATTE
9th Edition
ISBN: 9781265974688
Author: SILBERBERG
Publisher: MCG
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Chapter 19, Problem 19.147P

(a)

Interpretation Introduction

Interpretation:

[Ag+] present in the solution is (1.8×1010)[Cl-] and [AgCl2] present in the solution is (3.2×105)×[Cl-] have to be shown.

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at 25oC. The concentration terms are raised to the coefficients of their respective ions. It is denoted by Ksp.

This value indicates the degree of dissociation of a compound in water. More the value of Ksp more is the solubility of the compound.

Considering an equilibrium of salt AxBy with its respective ions in solution and thus Ksp is calculated.

  AxByxAy++yBx-

  Ksp=[xAy+]x[yBx-]y

Formation constant:

A stability constant or formation constant is an equilibrium constant for the formation of a complex ion in the solution and it measures the strength of interaction between the reactants that forms the complex.

(b)

Interpretation Introduction

Interpretation:

Value of [Cl-] has to be found for the given [Ag+]=[AgCl2].

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at 25oC. The concentration terms are raised to the coefficients of their respective ions. It is denoted by Ksp.

This value indicates the degree of dissociation of a compound in water. More the value of Ksp more is the solubility of the compound.

Considering an equilibrium of salt AxBy with its respective ions in solution and thus Ksp is calculated.

  AxByxAy++yBx-

  Ksp=[xAy+]x[yBx-]y

Formation constant:

A stability constant or formation constant is an equilibrium constant for the formation of a complex ion in the solution and it measures the strength of interaction between the reactants that forms the complex.

(c)

Interpretation Introduction

Interpretation:

Plot of solubility of AgCl versus Cl- has to be explained.

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

 Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at 25oC. The concentration terms are raised to the coefficients of their respective ions. It is denoted by Ksp.

This value indicates the degree of dissociation of a compound in water. More the value of Ksp more is the solubility of the compound.

Considering an equilibrium of salt AxBy with its respective ions in solution and thus Ksp is calculated.

  AxByxAy++yBx-

  Ksp=[xAy+]x[yBx-]y

Le Chatelier’s principle:

When a system in equilibrium then is subjected to any external disturbance like change of pressure, volume, temperature etc… Then the system acts in a way to prevent that change. This is called Le-Chatelier’s principle.

(d)

Interpretation Introduction

Interpretation:

The solubility of AgCl has to be found at the [Cl-] calculated at part (b) which is the minimum solubility of AgCl at that [Cl-].

Concept introduction:

Solubility:

Solubility is defined as the maximum amount of the solute that can be dissolved in the solvent at equilibrium.

 Solubility product constant:

Solubility product constant is defined for equilibrium between solids and its respective ions in the solution. Generally, solubility product refers only to insoluble or slightly soluble ionic substances that make equilibrium in water.

It is defined as the product of concentration of ions of a sparingly soluble salt in its saturated solution at 25oC. The concentration terms are raised to the coefficients of their respective ions. It is denoted by Ksp.

This value indicates the degree of dissociation of a compound in water. More the value of Ksp more is the solubility of the compound.

Considering equilibrium of salt AxBy with its respective ions in solution and thus the Ksp is calculated.

  AxByxAy++yBx-

  Ksp=[xAy+]x[yBx-]y

Formation constant:

A stability constant or formation constant is an equilibrium constant for the formation of a complex ion in the solution and it measures the strength of interaction between the reactants that forms the complex.

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Chapter 19 Solutions

CHEMISTRY: THE MOLECULAR NATURE OF MATTE

Ch. 19.3 - Prob. 19.6AFPCh. 19.3 - Prob. 19.6BFPCh. 19.3 - Prob. 19.7AFPCh. 19.3 - Prob. 19.7BFPCh. 19.3 - Prob. 19.8AFPCh. 19.3 - Prob. 19.8BFPCh. 19.3 - Prob. 19.9AFPCh. 19.3 - Prob. 19.9BFPCh. 19.3 - Prob. 19.10AFPCh. 19.3 - Prob. 19.10BFPCh. 19.3 - Prob. 19.11AFPCh. 19.3 - Prob. 19.11BFPCh. 19.3 - Prob. 19.12AFPCh. 19.3 - Prob. 19.12BFPCh. 19.4 - Cyanide ion is toxic because it forms stable...Ch. 19.4 - Prob. 19.13BFPCh. 19.4 - Prob. 19.14AFPCh. 19.4 - Calculate the solubility of PbCl2 in 0.75 M NaOH....Ch. 19 - Prob. 19.1PCh. 19 - Prob. 19.2PCh. 19 - Prob. 19.3PCh. 19 - Prob. 19.4PCh. 19 - Prob. 19.5PCh. 19 - Prob. 19.6PCh. 19 - Prob. 19.7PCh. 19 - Prob. 19.8PCh. 19 - Does the pH increase or decrease with each of the...Ch. 19 - The scenes below depict solutions of the same...Ch. 19 - The scenes below show three samples of a buffer...Ch. 19 - What are the [H3O+] and the pH of a propanoic...Ch. 19 - What are the [H3O+] and the pH of a benzoic...Ch. 19 - Prob. 19.14PCh. 19 - Prob. 19.15PCh. 19 - Prob. 19.16PCh. 19 - Find the pH of a buffer that consists of 0.95 M...Ch. 19 - Prob. 19.18PCh. 19 - Prob. 19.19PCh. 19 - Prob. 19.20PCh. 19 - Find the pH of a buffer that consists of 0.50 M...Ch. 19 - A buffer consists of 0.22 M KHCO3 and 0.37 M...Ch. 19 - A buffer consists of 0.50 M NaH2PO4 and 0.40 M...Ch. 19 - What is the component concentration ratio,...Ch. 19 - Prob. 19.25PCh. 19 - Prob. 19.26PCh. 19 - Prob. 19.27PCh. 19 - Prob. 19.28PCh. 19 - A buffer that contains 0.40 M of a base, B, and...Ch. 19 - A buffer that contains 0.110 M HY and 0.220 M Y−...Ch. 19 - A buffer that contains 1.05 M B and 0.750 M BH+...Ch. 19 - A buffer is prepared by mixing 204 mL of 0.452 M...Ch. 19 - A buffer is prepared by mixing 50.0 mL of 0.050 M...Ch. 19 - Prob. 19.34PCh. 19 - Prob. 19.35PCh. 19 - Prob. 19.36PCh. 19 - Choose specific acid-base conjugate pairs to make...Ch. 19 - An industrial chemist studying bleaching and...Ch. 19 - Oxoanions of phosphorus are buffer components in...Ch. 19 - The scenes below depict the relative...Ch. 19 - Prob. 19.41PCh. 19 - What species are in the buffer region of a weak...Ch. 19 - Prob. 19.43PCh. 19 - Prob. 19.44PCh. 19 - Prob. 19.45PCh. 19 - Prob. 19.46PCh. 19 - Prob. 19.47PCh. 19 - Prob. 19.48PCh. 19 - Prob. 19.49PCh. 19 - Prob. 19.50PCh. 19 - Prob. 19.51PCh. 19 - Prob. 19.52PCh. 19 - Prob. 19.53PCh. 19 - Prob. 19.54PCh. 19 - Prob. 19.55PCh. 19 - Prob. 19.56PCh. 19 - Prob. 19.57PCh. 19 - Prob. 19.58PCh. 19 - Prob. 19.59PCh. 19 - Prob. 19.60PCh. 19 - Prob. 19.61PCh. 19 - Use figure 19.9 to find an indicator for these...Ch. 19 - Prob. 19.63PCh. 19 - Prob. 19.64PCh. 19 - Prob. 19.65PCh. 19 - Prob. 19.66PCh. 19 - Write the ion-product expressions for (a) silver...Ch. 19 - Write the ion-product expressions for (a)...Ch. 19 - Write the ion-product expressions for (a) calcium...Ch. 19 - Prob. 19.70PCh. 19 - The solubility of silver carbonate is 0.032 M at...Ch. 19 - Prob. 19.72PCh. 19 - Prob. 19.73PCh. 19 - The solubility of calcium sulfate at 30°C is 0.209...Ch. 19 - Prob. 19.75PCh. 19 - Prob. 19.76PCh. 19 - Prob. 19.77PCh. 19 - Calculate the molar solubility of Ag2SO4 in (a)...Ch. 19 - Prob. 19.79PCh. 19 - Prob. 19.80PCh. 19 - Prob. 19.81PCh. 19 - Prob. 19.82PCh. 19 - Prob. 19.83PCh. 19 - Write equations to show whether the solubility of...Ch. 19 - Prob. 19.85PCh. 19 - Prob. 19.86PCh. 19 - Prob. 19.87PCh. 19 - Does any solid PbCl2 form when 3.5 mg of NaCl is...Ch. 19 - Prob. 19.89PCh. 19 - Prob. 19.90PCh. 19 - Prob. 19.91PCh. 19 - A 50.0-mL volume of 0.50 M Fe(NO3)3 is mixed with...Ch. 19 - Prob. 19.93PCh. 19 - Prob. 19.94PCh. 19 - Write a balanced equation for the reaction of in...Ch. 19 - Prob. 19.96PCh. 19 - Prob. 19.97PCh. 19 - Prob. 19.98PCh. 19 - What is [Ag+] when 25.0 mL each of 0.044 M AgNO3...Ch. 19 - Prob. 19.100PCh. 19 - Prob. 19.101PCh. 19 - Prob. 19.102PCh. 19 - When 0.84 g of ZnCl2 is dissolved in 245 mL of...Ch. 19 - When 2.4 g of Co(NO3)2 is dissolved in 0.350 L of...Ch. 19 - Prob. 19.105PCh. 19 - A microbiologist is preparing a medium on which to...Ch. 19 - As an FDA physiologist, you need 0.700 L of formic...Ch. 19 - Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2],...Ch. 19 - Water flowing through pipes of carbon steel must...Ch. 19 - Gout is caused by an error in metabolism that...Ch. 19 - In the process of cave formation (Section 19.3),...Ch. 19 - Phosphate systems form essential buffers in...Ch. 19 - The solubility of KCl is 3.7 M at 20°C. Two...Ch. 19 - It is possible to detect NH3 gas over 10−2 M NH3....Ch. 19 - Manganese(II) sulfide is one of the compounds...Ch. 19 - The normal pH of blood is 7.40 ± 0.05 and is...Ch. 19 - A bioengineer preparing cells for cloning bathes a...Ch. 19 - Sketch a qualitative curve for the titration of...Ch. 19 - Prob. 19.119PCh. 19 - The scene at right depicts a saturated solution of...Ch. 19 - Prob. 19.121PCh. 19 - The acid-base indicator ethyl orange turns from...Ch. 19 - Prob. 19.123PCh. 19 - Prob. 19.124PCh. 19 - Prob. 19.125PCh. 19 - Prob. 19.126PCh. 19 - Prob. 19.127PCh. 19 - Prob. 19.128PCh. 19 - Calcium ion present in water supplies is easily...Ch. 19 - Calculate the molar solubility of Hg2C2O4 (Ksp =...Ch. 19 - Environmental engineers use alkalinity as a...Ch. 19 - Human blood contains one buffer system based on...Ch. 19 - Quantitative analysis of Cl− ion is often...Ch. 19 - An ecobotanist separates the components of a...Ch. 19 - Some kidney stones form by the precipitation of...Ch. 19 - Prob. 19.136PCh. 19 - Prob. 19.137PCh. 19 - Because of the toxicity of mercury compounds,...Ch. 19 - A 35.0-mL solution of 0.075 M CaCl2 is mixed with...Ch. 19 - Rainwater is slightly acidic due to dissolved CO2....Ch. 19 - Prob. 19.141PCh. 19 - Ethylenediaminetetraacetic acid (abbreviated...Ch. 19 - Buffers that are based on...Ch. 19 - NaCl is purified by adding HCl to a saturated...Ch. 19 - Scenes A to D represent tiny portions of 0.10 M...Ch. 19 - Prob. 19.146PCh. 19 - Prob. 19.147PCh. 19 - Prob. 19.148P
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