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ChemistryChemistry: An Atoms First Approach2nd Edition
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Explain why the following are done, both of which are related to acid–base chemistry. a. Power plants burning coal with high sulfur content use scrubbers to help eliminate sulfur emissions. b. A gardener mixes lime (CaO) into the soil of his garden.

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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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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 34Q
Textbook Problem
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Explain why the following are done, both of which are related to acid–base chemistry.

a. Power plants burning coal with high sulfur content use scrubbers to help eliminate sulfur emissions.

b. A gardener mixes lime (CaO) into the soil of his garden.

(a)

Interpretation Introduction

Interpretation: An explanation regarding the given statements is to be stated.

Concept introduction: The power plants that burn large amounts of coal use scrubbers for eliminating sulfur emissions.

Lime is added to the soil because of its positive affects that increase the fertility of the soil.

To determine: An explanation regarding the given statement, “Power plants burning coal with high sulfur content use scrubbers to help eliminate sulfur emissions”.

Explanation of Solution

Explanation

The power plants burning coal with high sulfur content use scrubbers to help eliminate the sulfur emissions to prevent the formation of sulfuric acid (acid rain).

The sulfur on its emission into the environment undergoes a reaction with the atmospheric oxygen, leading to the formation of sulfur dioxide...

(b)

Interpretation Introduction

Interpretation: An explanation regarding the given statements is to be stated.

Concept introduction: The power plants that burn large amounts of coal use scrubbers for eliminating sulfur emissions.

Lime is added to the soil because of its positive affects that increase the fertility of the soil.

To determine: An explanation regarding the given statement, “A gardener mixes lime (CaO) into the soil of his garden”.

The addition of lime (CaO) into the soil increases the pH of the soil making it less acidic.

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Chemistry: An Atoms First Approach
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Ch. 13 - Define each of the following: a. Arrhenius acid b....Ch. 13 - Define or illustrate the meaning of the following...Ch. 13 - Define or illustrate the meaning of the following...Ch. 13 - How is acid strength related to the value of Ka?...Ch. 13 - Two strategies are followed when solving for the...Ch. 13 - Two strategies are also followed when solving for...Ch. 13 - Table 13-4 lists the stepwise Ka values for some...Ch. 13 - For conjugate acidbase pairs, how are Ka and Kb...Ch. 13 - What is a salt? List some anions that behave as...Ch. 13 - For oxyacids, how does acid strength depend on a....
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. Write out an...Ch. 13 - Which of the following statements is(are) true?...Ch. 13 - Consider the following mathematical expressions....Ch. 13 - Consider a 0.10-M H2CO3 solution and a 0.10-M...Ch. 13 - Of the hydrogen halides, only HF is a weak acid....Ch. 13 - Explain why the following are done, both of which...Ch. 13 - Write balanced equations that describe the...Ch. 13 - Write the dissociation reaction and the...Ch. 13 - For each of the following aqueous reactions,...Ch. 13 - For each of the following aqueous reactions,...Ch. 13 - Classify each of the following as a strong acid or...Ch. 13 - Consider the following illustrations: Which beaker...Ch. 13 - Use Table 13-2 to order the following from the...Ch. 13 - Use Table 13-2 to order the following from the...Ch. 13 - You may need Table 13-2 to answer the following...Ch. 13 - You may need Table 13-2 to answer the following...Ch. 13 - Calculate the [OH] of each of the following...Ch. 13 - Calculate the [H+] of each of the following...Ch. 13 - Values of Kw as a function of temperature are as...Ch. 13 - At 40.C the value of Kw is 2.92 1014. a....Ch. 13 - Calculate the pH and pOH of the solutions in...Ch. 13 - Calculate [H+] and [OH] for each solution at 25C....Ch. 13 - Fill in the missing information in the following...Ch. 13 - Fill in the missing information in the following...Ch. 13 - The pH of a sample of gastric juice in a persons...Ch. 13 - The pOH of a sample of baking soda dissolved in...Ch. 13 - What are the major species present in 0.250 M...Ch. 13 - A solution is prepared by adding 50.0 mL of 0.050...Ch. 13 - Calculate the pH of each of the following...Ch. 13 - Calculate the pH of each of the following...Ch. 13 - Calculate the concentration of an aqueous HI...Ch. 13 - Calculate the concentration of an aqueous HBr...Ch. 13 - How would you prepare 1600 mL of a pH = 1.50...Ch. 13 - A solution is prepared by adding 50.0 mL...Ch. 13 - What are the major species present in 0.250 M...Ch. 13 - What are the major species present in 0.250 M...Ch. 13 - Calculate the concentration of all species present...Ch. 13 - Calculate the percent dissociation for a 0.22-M...Ch. 13 - For propanoic acid (HC3H5O2, Ka = 1.3 105),...Ch. 13 - A solution is prepared by dissolving 0.56 g...Ch. 13 - Monochloroacetic acid, HC2H2ClO2, is a skin...Ch. 13 - A typical aspirin tablet contains 325 mg...Ch. 13 - Calculate the pH of a solution that contains 1.0 M...Ch. 13 - A solution is made by adding 50.0 mL of 0.200 M...Ch. 13 - Calculate the percent dissociation of the acid in...Ch. 13 - Using the Ka values in Table 13-2, calculate the...Ch. 13 - A 0.15-M solution of a weak acid is 3.0%...Ch. 13 - An acid HX is 25% dissociated in water. 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. Write...Ch. 13 - Would you expect Fe3+ or Fe2+ to be the stronger...Ch. 13 - Use the Lewis acid-base model to explain the...Ch. 13 - A 10.0-mL sample of an HCl solution has a pH of...Ch. 13 - Which of the following represent conjugate...Ch. 13 - A solution is tested for pH and conductivity as...Ch. 13 - The pH of human blood is steady at a value of...Ch. 13 - Hemoglobin (abbreviated Hb) is a protein that is...Ch. 13 - A 0.25-g sample of lime (CaO) is dissolved in...Ch. 13 - At 25C, a saturated solution of benzoic acid (Ka =...Ch. 13 - Calculate the pH of an aqueous solution containing...Ch. 13 - Acrylic acid (CH29CHCO2H) is a precursor for many...Ch. 13 - Classify each of the following as a strong acid,...Ch. 13 - The following illustration displays the relative...Ch. 13 - Quinine (C20H24N2O2) is the most important...Ch. 13 - Codeine (C18H21NO3) is a derivative of morphine...Ch. 13 - A codeine-containing cough syrup lists codeine...Ch. 13 - The equilibrium constant Ka for the reaction...Ch. 13 - Rank the following 0.10 M solutions in order of...Ch. 13 - Is an aqueous solution of NaHSO4 acidic, basic, or...Ch. 13 - Calculate the value for the equilibrium constant...Ch. 13 - Students are often surprised to learn that organic...Ch. 13 - For solutions of the same concentration, as acid...Ch. 13 - Complete the table for each of the following...Ch. 13 - Consider a 0.60-M solution of HC3H5O3, lactic acid...Ch. 13 - Consider a 0.67-M solution of C2H5NH2 (Kb = 5.6 ...Ch. 13 - Rank the following 0.10 M solutions in order of...Ch. 13 - Consider 0.25 M solutions of the following salts:...Ch. 13 - Calculate the pH of the following solutions: a....Ch. 13 - Consider 0.10 M solutions of the following...Ch. 13 - The pH of 1.0 108 M hydrochloric acid is not...Ch. 13 - Calculate the pH of a 1.0 107-M solution of NaOH...Ch. 13 - Calculate [OH] in a 3.0 107-M solution of Ca(OH)2.Ch. 13 - Consider 50.0 mL of a solution of weak acid HA (Ka...Ch. 13 - Making use of the assumptions we ordinarily make...Ch. 13 - Calculate the pH of a 0.200-M solution of C5H5NHF....Ch. 13 - Determine the pH of a 0.50-M solution of NH4OCl....Ch. 13 - Calculate [OH] in a solution obtained by adding...Ch. 13 - What mass of NaOH(s) must be added to 1.0 L of...Ch. 13 - Consider 1000. mL of a 1.00 104-M solution of a...Ch. 13 - Calculate the mass of sodium hydroxide that must...Ch. 13 - Consider the species PO43, HPO42, and H2PO4. Each...Ch. 13 - Calculate the pH of a 0.10-M solution of sodium...Ch. 13 - Will 0.10 M solutions of the following salts be...Ch. 13 - a. The principal equilibrium in a solution of...Ch. 13 - A 0.100-g sample of the weak acid HA (molar mass =...Ch. 13 - A sample containing 0.0500 mole of Fe2(SO4)3 is...Ch. 13 - A 2.14 g sample of sodium hypoiodite is dissolved...Ch. 13 - Isocyanic acid (HNCO) can be prepared by heating...Ch. 13 - A certain acid, HA, has a vapor density of 5.11...Ch. 13 - An aqueous solution contains a mixture of 0.0500 M...Ch. 13 - For the following, mix equal volumes of one...

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