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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 83E
Textbook Problem
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Write the reaction and the corresponding Kb equilibrium expression for each of the following substances acting as bases in water.

a. NH3

b. C5H5N

(a)

Interpretation Introduction

Interpretation: The dissociation reaction and the corresponding Kb equilibrium expression for the given substances is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

To determine: The dissociation reaction and the corresponding Kb equilibrium expression for NH3 .

Explanation of Solution

Explanation

The dissociation reaction for NH3 is, NH3(aq)+H2O(l)NH4+(aq)+OH(aq) .

The dissociation reaction for NH3 is,

NH3(aq)+H2O(l)NH4+(aq)+OH(aq)

(b)

Interpretation Introduction

Interpretation: The dissociation reaction and the corresponding Kb equilibrium expression for the given substances is to be stated.

Concept introduction: The state when the reactants involved in a chemical reaction and the products formed in the reaction exist in concentrations having no further tendency to change is known as an equilibrium state of the reaction.

The equilibrium constant for the dissociation reaction of a given base is known as the base dissociation constant and is denoted by the symbol, Kb .

To determine: The dissociation reaction and the corresponding Kb equilibrium expression for C5H5N .

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Chapter 13 Solutions

Chemistry: An Atoms First Approach
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Ch. 13 - Consider two beakers of pure water at different...Ch. 13 - Differentiate between the terms strength and...Ch. 13 - Sketch two graphs: (a) percent dissociation for...Ch. 13 - Consider a solution prepared by mixing a weak acid...Ch. 13 - Explain why salts can be acidic, basic, or...Ch. 13 - Consider two separate aqueous solutions: one of a...Ch. 13 - You are asked to calculate the H+ concentration in...Ch. 13 - Consider a solution prepared by mixing a weak acid...Ch. 13 - Consider a solution formed by mixing 100.0 mL of...Ch. 13 - A certain sodium compound is dissolved in water to...Ch. 13 - Acids and bases can be thought of as chemical...Ch. 13 - Consider two solutions of the salts NaX(aq) and...Ch. 13 - What is meant by pH? True or false: A strong acid...Ch. 13 - Why is the pH of water at 25C equal to 7.00?Ch. 13 - Can the pH of a solution be negative? Explain.Ch. 13 - Is the conjugate base of a weak acid a strong...Ch. 13 - Match the following pH values: 1, 2, 5, 6, 6.5, 8,...Ch. 13 - The salt BX, when dissolved in water, produces an...Ch. 13 - Anions containing hydrogen (for example, HCO3 and...Ch. 13 - Which of the following conditions indicate an...Ch. 13 - Which of the following conditions indicate a basic...Ch. 13 - Why is H3O+ the strongest acid and OH the...Ch. 13 - How many significant figures are there in the...Ch. 13 - In terms of orbitals and electron arrangements,...Ch. 13 - Consider the autoionization of liquid ammonia:...Ch. 13 - The following are representations of acidbase...Ch. 13 - Give three example solutions that fit each of the...Ch. 13 - Derive an expression for the relationship between...Ch. 13 - Consider the following statements. 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If the...Ch. 13 - Trichloroacetic acid (CCl3CO2H) is a corrosive...Ch. 13 - The pH of a 0.063-M solution of hypobromous acid...Ch. 13 - A solution of formic acid (HCOOH, Ka = 1.8 104)...Ch. 13 - A typical sample of vinegar has a pH of 3.0....Ch. 13 - One mole of a weak acid HA was dissolved in 2.0 L...Ch. 13 - You have 100.0 g saccharin, a sugar substitute,...Ch. 13 - Write the reaction and the corresponding Kb...Ch. 13 - Write the reaction and the corresponding Kb...Ch. 13 - Use Table 13-3 to help order the following bases...Ch. 13 - Use Table 13-3 to help order the following acids...Ch. 13 - Use Table 13-3 to help answer the following...Ch. 13 - Use Table 13-3 to help answer the following...Ch. 13 - Calculate the pH of the following solutions. a....Ch. 13 - Calculate [OH], pOH, and pH for each of the...Ch. 13 - What are the major species present in 0.015 M...Ch. 13 - What are the major species present in the...Ch. 13 - What mass of KOH is necessary to prepare 800.0 mL...Ch. 13 - Calculate the concentration of an aqueous Sr(OH)2...Ch. 13 - What are the major species present in a 0.150-M...Ch. 13 - For the reaction of hydrazine (N2H4) in water,...Ch. 13 - Calculate [OH], [H+], and the pH of 0.20 M...Ch. 13 - Calculate [OH], [H+], and the pH of 0.40 M...Ch. 13 - Calculate the pH of a 0.20-M C2H5NH2 solution (Kb...Ch. 13 - Calculate the pH of a 0.050-M (C2H5)2NH...Ch. 13 - What is the percent ionization in each of the...Ch. 13 - Calculate the percentage of pyridine (C5H5N) that...Ch. 13 - The pH of a 0.016-M aqueous solution of...Ch. 13 - Calculate the mass of HONH2 required to dissolve...Ch. 13 - Write out the stepwise Ka reactions for the...Ch. 13 - Write out the stepwise Ka reactions for citric...Ch. 13 - A typical vitamin C tablet (containing pure...Ch. 13 - Arsenic acid (H3AsO4) is a triprotic acid with Ka1...Ch. 13 - Calculate the pH and [S2] in a 0.10-M H2S...Ch. 13 - Calculate [CO32] in a 0.010-M solution of CO2 in...Ch. 13 - Calculate the pH of a 2.0-M H2SO4 solution.Ch. 13 - Calculate the pH of a 5.0 103-M solution of...Ch. 13 - Arrange the following 0.10 M solutions in order of...Ch. 13 - Arrange the following 0.10 M solutions in order...Ch. 13 - Given that the Ka value for acetic acid is 1.8 ...Ch. 13 - The Kb values for ammonia and methylamine are 1.8 ...Ch. 13 - Determine [OH], [H+], and the pH of each of the...Ch. 13 - Calculate the concentrations of all species...Ch. 13 - Calculate the pH of each of the following...Ch. 13 - Calculate the pH of each of the following...Ch. 13 - Sodium azide (NaN3) is sometimes added to water to...Ch. 13 - Papaverine hydrochloride (abbreviated papH+Cl;...Ch. 13 - An unknown salt is either NaCN, NaC2H3O2, NaF,...Ch. 13 - Consider a solution of an unknown salt having the...Ch. 13 - A 0.050-M solution of the salt NaB has a pH of...Ch. 13 - A 0.20-M sodium chlorobenzoate (NaC7H4ClO2)...Ch. 13 - Calculate the pH of a 0.050-M Al(NO3)3 solution....Ch. 13 - Calculate the pH of a 0.10-M CoCl3 solution. The...Ch. 13 - Are solutions of the following salts acidic,...Ch. 13 - Are solutions of the following salts acidic,...Ch. 13 - Place the species in each of the following groups...Ch. 13 - Place the species in each of the following groups...Ch. 13 - Place the species in each of the following groups...Ch. 13 - Using your results from Exercise 133, place the...Ch. 13 - Will the following oxides give acidic, basic, or...Ch. 13 - Will the following oxides give acidic, basic, or...Ch. 13 - Identify the Lewis acid and the Lewis base in each...Ch. 13 - Identify the Lewis acid and the Lewis base in each...Ch. 13 - Aluminum hydroxide is an amphoteric substance. It...Ch. 13 - Zinc hydroxide is an amphoteric substance. 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