1 Basic Concepts About Matter 2 Measurements In Chemistry 3 Atomic Structures And The Periodic Table 4 Chemical Bonding: The Ionic Bond Model 5 Chemical Bonding: The Covalent Bond Model 6 Chemical Calculations: Formula Masses, Moles, And Chemical Equations 7 Gases, Liquids, And Solids 8 Solutions 9 Chemical Reactions 10 Acids, Bases, And Salts 11 Nuclear Chemistry 12 Saturated Hydrocarbons 13 Unsaturated Hydrocarbons 14 Alcohols, Phenols And Ethers 15 Aldehydes And Ketones 16 Carboxylic Acids, Esters, And Other Acid Derivatives 17 Amines And Amides 18 Carbohydrates 19 Lipids 20 Proteins 21 Enzymes And Vitamins 22 Nucleic Acids 23 Biochemical Energy Production 24 Carbohydrate Metabolism 25 Lipid Metabolism 26 Protein Metabolism Chapter10: Acids, Bases, And Salts
10.1 Arrhenium Acid-base Theory 10.2 Bronsted-lowry Acid-base Theory 10.3 Mono-, Di-, And Triprotic Acids 10.4 Strengths Of Acids And Bases 10.5 Ionization Constants For Acids And Bases 10.6 Salts 10.7 Acid-base Neutralization Chemical Reactions 10.8 Self-ionization Of Water 10.9 The Ph Concept 10.10 The Pka Method For Expressing Acid Strength 10.11 The Ph Of Aqueous Salt Solutions 10.12 Buffers 10.13 The Henderson-hasselbalch Equation 10.14 Electrolytes 10.15 Equivalents And Milliequivalents Of Electrolytes 10.16 Acid-base Titrations Chapter Questions Section: Chapter Questions
Problem 10.1EP: In Arrhenius acidbase theory, what ion is responsible for the properties of a. acidic solutions b.... Problem 10.2EP: What term is used to describe the formation of ions, in aqueous solution, from a. a molecular... Problem 10.3EP: Classify each of the following as a property of an Arrhenius acid or the property of an Arrhenius... Problem 10.4EP: Classify each of the following as a property of an Arrhenius acid or the property of an Arrhenius... Problem 10.5EP: Write equations depicting the behavior of the following Arrhenius acids and bases in water. a. HI... Problem 10.6EP: Write equations depicting the behavior of the following Arrhenius acids and bases in water. a. HBr... Problem 10.7EP: Indicate whether the first listed reactant in each of the following BrnstedLowry acidbase reactions... Problem 10.8EP: Indicate whether the first listed reactant in each of the following BrnstedLowry acidbase reactions... Problem 10.9EP: Write chemical equations that show the indicated behavior in aqueous solution for each of the... Problem 10.10EP: Write chemical equations that show the indicated behavior in aqueous solution for each of the... Problem 10.11EP: Indicate whether or not the two members of each of the following pairs of substances constitute a... Problem 10.12EP: Indicate whether or not the two members of each of the following pairs of substances constitute a... Problem 10.13EP: Write the formula of each of the following. a. conjugate base of H2SO3 b. conjugate acid of CN c.... Problem 10.14EP: Write the formula of each of the following. a. conjugate base of NH4+ b. conjugate acid of OH c.... Problem 10.15EP: Identify the conjugate acidbase pairs associated with the following acidbase reaction. HC2H3O2 + H2O... Problem 10.16EP: Identify the conjugate acidbase pairs associated with the following acidbase reaction. HC3H5O3 + H2O... Problem 10.17EP: The ion HCO3 is an amphiprotic ion. Write the chemical equation to describe its behavior in aqueous... Problem 10.18EP: The ion HPO42 is an amphiprotic ion. Write the chemical equation to describe its behavior in aqueous... Problem 10.19EP: Classify each of the following acids as monoprotic, diprotic, or triprotic. a. HClO3 (chloric acid)... Problem 10.20EP: Classify each of the following acids as monoprotic, diprotic, or triprotic. a. H2SO4 (sulfuric acid)... Problem 10.21EP Problem 10.22EP: For each of the acids in Problem 10-19 indicate how many acidic hydrogen atoms and how many... Problem 10.23EP: Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution... Problem 10.24EP: Write chemical equations showing the individual proton-transfer steps that occur in aqueous solution... Problem 10.25EP Problem 10.26EP: The formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why. Problem 10.27EP: Pyruvic acid, which is produced in metabolic reactions, has the structure Would you predict that... Problem 10.28EP: Oxaloacetic acid, which is produced in metabolic reactions, has the structure Would you predict that... Problem 10.29EP: Classify each of the acids in Problem 10-19 as a strong acid or a weak acid. a. HClO3 (chloric acid)... Problem 10.30EP: Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric... Problem 10.31EP: For each of the following pairs of acids, indicate whether the first member of the pair is a... Problem 10.32EP: For each of the following pairs of acids, indicate whether the first member of the pair is a... Problem 10.33EP: For each of the following pairings of acid and base indicate whether both the acid and the base are... Problem 10.34EP: For each of the following pairings of acid and base indicate whether both the acid and the base are... Problem 10.35EP: The HCl in a 0.10 M HCl solution is 100% dissociated. What are the molar concentrations of HCl,... Problem 10.36EP: The HNO3 in a 0.50 M HNO3 solution is 100% dissociated. What are the molar concentrations of HNO3,... Problem 10.37EP: The following four diagrams represent aqueous solutions of four different acids with the general... Problem 10.38EP: Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid? Problem 10.39EP: Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the... Problem 10.40EP: Which of the terms weak, strong, monoprotic, diprotic, and triprotic characterize(s) each of the... Problem 10.41EP: Write the acid ionization constant expression for the ionization of each of the following monoprotic... Problem 10.42EP: Write the acid ionization constant expression for the ionization of each of the following monoprotic... Problem 10.43EP Problem 10.44EP: Write the base ionization constant expression for the ionization of each of the following bases. In... Problem 10.45EP Problem 10.46EP: Using the acid ionization constant information given in Table 10-3, indicate which acid is the... Problem 10.47EP: A 0.00300 M solution of an acid is 12% ionized. Calculate the acid ionization constant Ka. Problem 10.48EP: A 0.0500 M solution of a base is 7.5% ionized. Calculate the base ionization constant Kb. Problem 10.49EP: Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following... Problem 10.50EP: Is the monoprotic acid Y or the monoprotic acid Z the stronger acid in each of the following... Problem 10.51EP: Classify each of the following substances as an acid, a base, or a salt. a. HBr b. NaI c. NH4NO3 d.... Problem 10.52EP: Classify each of the following substances as an acid, a base, or a salt. a. AlPO4 b. KOH c. HNO3 d.... Problem 10.53EP Problem 10.54EP: Indicate whether or not both members of each of the following pairs of substances are salts. a. LiOH... Problem 10.55EP Problem 10.56EP: Write a balanced equation for the dissociation into ions of each of the following soluble salts in... Problem 10.57EP: Indicate whether each of the following reactions is an acidbase neutralization reaction. a.... Problem 10.58EP: Indicate whether each of the following reactions is an acidbase neutralization reaction. a.... Problem 10.59EP: Without writing an equation, specify the molecular ratio in which each of the following acidbase... Problem 10.60EP: Without writing an equation, specify the molecular ratio in which each of the following acidbase... Problem 10.61EP: Write a balanced chemical equation to represent each of the following acidbase neutralization... Problem 10.62EP: Write a balanced chemical equation to represent each of the following acidbase neutralization... Problem 10.63EP Problem 10.64EP: Write a balanced molecular equation for the preparation of each of the following salts, using an... Problem 10.65EP Problem 10.66EP: What is the molar hydronium ion concentration in aqueous solutions with the following hydroxide ion... Problem 10.67EP: Indicate whether each of the solutions in Problem 10-65 is acidic, basic, or neutral. a. 3.5 103 M... Problem 10.68EP Problem 10.69EP Problem 10.70EP Problem 10.71EP Problem 10.72EP: Indicate whether each of the solutions in Problem 10-70 is acidic, basic, or neutral. a. 2.4 103 b.... Problem 10.73EP: Selected information about five solutions, each at 24C, is given in the following table. Fill in the... Problem 10.74EP: Selected information about five solutions, each at 24C, is given in the following table. Fill in the... Problem 10.75EP: Calculate the pH of solutions with the following hydronium ion concentrations. a. 1.00 105 M b.... Problem 10.76EP: Calculate the pH of solutions with the following hydronium ion concentrations. a. 1.00 103 M b.... Problem 10.77EP: Calculate the pH of solutions with the following hydroxide ion concentrations. a. 1.00 104 M b.... Problem 10.78EP: Calculate the pH of solutions with the following hydroxide ion concentrations. a. 1.00 106 M b.... Problem 10.79EP: What is the [H3O+] value in solutions with each of the following pH values? a. 5.00 b. 7.00 c. 3.45... Problem 10.80EP: What is the [H3O+] value in solutions with each of the following pH values? a. 4.00 b. 6.00 c. 4.34... Problem 10.81EP Problem 10.82EP: What is the molar hydronium ion concentration in solutions with each of the following pH values? a.... Problem 10.83EP Problem 10.84EP: Indicate whether each of the following samples is acidic, basic, or neutral. a. butter, pH 6.1 b.... Problem 10.85EP: Selected information about five solutions, each at 24C, is given in the following table. Fill in the... Problem 10.86EP Problem 10.87EP: Consider the following four solutions: (1) apple juice, pH 3.8, (2) pickle juice, pH 3.5, (3)... Problem 10.88EP: Consider the following four biological solutions: (1) bile, pH 8.0, (2) blood, pH 7.4, (3) urine, pH... Problem 10.89EP: For each of the following pairs of solutions, indicate whether the first listed solution has a... Problem 10.90EP Problem 10.91EP: Calculate the pKa value for each of the following acids. a. Nitrous acid (HNO2), Ka = 4.5 104 b.... Problem 10.92EP: Calculate the pKa value for each of the following acids. a. Phosphoric acid (H3PO4), Ka = 7.5 103... Problem 10.93EP: Acid A has a pKa value of 4.23, and acid B has a pKa value of 3.97. Which of the two acids is... Problem 10.94EP: Acid A has a pKa value of 5.71, and acid B has a pKa value of 5.30. Which of the two acids is... Problem 10.95EP: If a weak acid has a pKa value of 8.73, what is the value of Ka for the acid? Problem 10.96EP: If a weak acid has a pKa value of 7.21, what is the value of Ka for the acid? Problem 10.97EP: Classify each of the following salts as a strong acid strong base salt, a strong acidweak base salt,... Problem 10.98EP: Classify each of the following salts as a strong acidstrong base salt, a strong acidweak base salt,... Problem 10.99EP Problem 10.100EP: Identify the ion (or ions) present in each of the salts in Problem 10-98 that will undergo... Problem 10.101EP Problem 10.102EP Problem 10.103EP: Both ions in the salt ammonium cyanide (NH4CN) hydrolyze in aqueous solution. Explain why this... Problem 10.104EP: Both ions in the salt ammonium acetate (NH4C2H3O2) hydrolyze in aqueous solution. Explain why this... Problem 10.105EP: Arrange the following 0.10 M aqueous solutions in order of increasing pH: HCl, NaCl, HCN, and NaCN. Problem 10.106EP: Arrange the following 0.10 M aqueous solutions in order of increasing pH: HF, NaF, HNO3, and NaNO3. Problem 10.107EP: Predict whether each of the following pairs of substances could function as a buffer system in... Problem 10.108EP: Predict whether each of the following pairs of substances could function as a buffer system in... Problem 10.109EP: Identify the two active species in each of the following buffer systems. a. HCN and KCN b. H3PO4 and... Problem 10.110EP: Identify the two active species in each of the following buffer systems. a. HF and LiF b. Na2HPO4... Problem 10.111EP Problem 10.112EP: Write an equation for each of the following buffering actions. a. the response of a HPO42/PO43... Problem 10.113EP Problem 10.114EP Problem 10.115EP Problem 10.116EP: A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the... Problem 10.117EP: The following four diagrams represent aqueous solutions containing a weak acid (HA) and/or its... Problem 10.118EP: Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer... Problem 10.119EP: Identify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal... Problem 10.120EP: Identify the buffer system(s)the conjugate acidbase pair(s)present in a solution that contains equal... Problem 10.121EP Problem 10.122EP Problem 10.123EP: What is the pH of a buffer that is 0.230 M in a weak acid and 0.500 M in the acids conjugate base?... Problem 10.124EP: What is the pH of a buffer that is 0.250 M in a weak acid and 0.260 M in the acids conjugate base?... Problem 10.125EP: What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base?... Problem 10.126EP: What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base?... Problem 10.127EP: Classify each of the following compounds as a strong electrolyte or a weak electrolyte. a. H2CO3 b.... Problem 10.128EP: Classify each of the following compounds as a strong electrolyte or a weak electrolyte. a. H3PO4 b.... Problem 10.129EP: Indicate whether solutions of each of the following substances contain ions, molecules, or both. a.... Problem 10.130EP: Indicate whether solutions of each of the following substances contain ions, molecules, or both. a.... Problem 10.131EP: How many ions, per formula unit, are produced when each of the following soluble salts (strong... Problem 10.132EP: How many ions, per formula unit, are produced when each of the following soluble salts (strong... Problem 10.133EP: Write a balanced chemical equation for the dissociation in water of each of the salts listed in... Problem 10.134EP Problem 10.135EP: Four different substances of the generalized formula HA were dissolved in water, with the results... Problem 10.136EP: Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte? Problem 10.137EP: Indicate the number of equivalents in each of the following molar quantities of ions. a. 1 mole Na+... Problem 10.138EP: Indicate the number of equivalents in each of the following molar quantities of ions. a. 1 mole K+... Problem 10.139EP: Indicate the number of equivalents in each of the following molar quantities of ions. a. 2 moles K+... Problem 10.140EP: Indicate the number of equivalents in each of the following molar quantities of ions. a. 4 moles Na+... Problem 10.141EP: A solution contains 48 mEq of Ca2+ ion. Based on this information, a. how many Eq of Ca2+ ion are... Problem 10.142EP Problem 10.143EP Problem 10.144EP: A solution is 0.0030 M in H2PO4 ion. What is this ion concentration in mEq/L? Problem 10.145EP Problem 10.146EP Problem 10.147EP: How many mEq of HCO3 are present in a solution that also contains 75 mEq of Na+, 83 mEq K+, 10 mEq... Problem 10.148EP: How many mEq of Ca2+ are present in a solution that also contains 75 mEq of Na+, 83 mEq K+, 35 mEq... Problem 10.149EP: Determine the molarity of a NaOH solution when each of the following amounts of acid neutralizes... Problem 10.150EP: Determine the molarity of a KOH solution when each of the following amounts of acid neutralizes 25.0... Problem 10.26EP: The formula for tartaric acid is preferably written as H2C4H4O6 rather than as C4H6O6. Explain why.
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Concept explainers
27) The cycle of copper reactions illustrates important principles of chemical reactions. The cycle begins with elemental copper, which in a first reaction is oxidized to copper(II) cation. Copper(II) is then carried through different solid forms. In the last step, copper(II) cation is reduced, the copper metal is regenerated, and the cycle is closed. The five key steps are (see attached picture). Assume that you want to carry out a sequence of cycle reactions.
How many grams of zinc metal are needed to completely regenerate 2.63g of copper in the fifth step in the cycle?
Transcribed Image Text: 3Cu2 (aq)4H20 2NO
Cu(OH)2(s)
1. ЗСи(s) + 2NO; + 8H-
2+
2. Cu (aq) 20H (aq)
Cu(OH)2 (s) CuO (s) H20
4. CuO(s)2H Cu2
Cu2 (aq)Zn(s)
(aq)H2O
Zn2 (aq)Cu(s)
Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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