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chemistry principles and practice

Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions

A saturated solution of milk of magnesia, Mg(OH)2, has a pH of 10.52. What is the hydronium ion concentration of the solution? What is the hydroxide ion concentration? Is the solution acidic or basic?
Find [OH-] and the pH of the following solutions.(a) 0.25 g barium hydroxide, Ba(OH)2, dissolved in enough water to make 0.655 L of solution(b) A 3.00 L solution of KOH is prepared by diluting 300.0 mL 0.149 M KOH with water.
Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases.(a) Hydrazoic acid, HN3(b) Citric acid, H2C6H6O7(c) Squaric acid, H2C4O4
Write the chemical equation for the ionization of the following weak acids. Assume only one hydrogen ionizes in all cases.(a) Malic acid, H2C4H4O5(b) Maleic acid, H2C4H2O4(c) Malonic acid, H2C3H2O4
HCN, a deadly gas that smells like bitter almonds, is formed by the reaction of H2SO4 and KCN. It was used in some states to execute criminals in the gas chamber. Measurements performed (carefully) on a 0.0050 M solution of HCN indicate that it is 0.035% ionized. Calculate Ka.
A solution is prepared by dissolving 0.121 g uric acid, C5H3N4O3H (molar mass = 168 g/mol), and diluting to make exactly 10 mL of solution. Each uric acid molecule has only one hydrogen ion that dissociates. Conductivity measurements indicate that the acid is 4.2% ionized. Calculate Ka for uric
Measurements of conductivity of solutions of two acids, A and B, produced the following data. Characterize each acid as strong or weak.
Assuming that the conductivity of an acid solution is proportional to the concentration of H3O+, sketch plots of conductivity versus concentration for HCl and HF over the 0- to 0.020 M concentration range.
Consider the solution formed when 50.0 mg butyric acid, C3H7COOH, a bad-smelling organic acid (formed when butter turns rancid), is dissolved in water to make 1.00 mL of solution. Th e pH of the solution is 2.52. Calculate Ka and pKa for butyric acid.
When 1.00 g thiamine hydrochloride (also called vitamin B1 hydrochloride) is dissolved in water and then diluted to exactly 10.00 mL, the pH of the resulting solution is 4.50. The formula weight of thiamine hydrochloride is 337.28. Calculate Ka and pKa for this acid.
If a 0.0100 M solution of caproic acid, thought to be at least partially responsible for the unique (and generally considered foul) smell of goats, has a pH of 3.43, what is Ka and pKa?
Lactic acid, CH3CH(OH)COOH, forms in muscles as a by-product of their contraction. If the pH of a 0.0376 M solution is 2.66, what is Ka and pKa for lactic acid?
The pH of a 0.10 M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
A 0.10 M solution of chloroacetic acid, ClCH2COOH, has a pH of 1.95. Calculate Ka for the acid.
Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.(a) 0.20 M C6H5COOH(b) 1.50 M HCOOH(c) 0.0055 M HCN(d) 0.075 M HNO2
Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.(a) 1.25 M HOCl(b) 0.80 M HF(c) 0.14 M CH3COOH(d) 0.25 M HCOOH
Use the Ka values in Table 15.6 to calculate the pH of the following solutions.(a) 0.33 M HNO2(b) 0.016 M phenol, C6H5OH(c) 0.25 M HF(d) 0.010 M HCOOHTable 15.6
Use the Ka values in Table 15.6 to calculate the pH of the following solutions.(a) 0.050 M HI(b) 0.85 M HF(c) 0.15 M CH3COOH(d) 0.017 M C6H5COOHTable 15.6
What is the fraction of acid ionized in each acid in Exercise 15.61?Exercise 15.61Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.(a) 0.20 M C6H5COOH(b) 1.50 M HCOOH(c) 0.0055 M HCN(d) 0.075 M HNO2
What is the fraction of acid ionized in each acid in Exercise 15.62?Exercise 15.62Write the iCe table and set up the equation needed to solve for the concentration of the hydrogen ion in the following solutions.(a) 1.25 M HOCl(b) 0.80 M HF(c) 0.14 M CH3COOH(d) 0.25 M HCOOH
What is the fraction of acid ionized in each acid in Exercise 15.63?Exercise 15.63Use the Ka values in Table 15.6 to calculate the pH of the following solutions.(a) 0.33 M HNO2(b) 0.016 M phenol, C6H5OH(c) 0.25 M HF(d) 0.010 M HCOOH
What is the fraction of acid ionized in each acid in Exercise 15.64?Exercise 15.64Use the Ka values in Table 15.6 to calculate the pH of the following solutions.(a) 0.050 M HI(b) 0.85 M HF(c) 0.15 M CH3COOH(d) 0.017 M C6H5COOHTable 15.6
Write the chemical equation for the ionization of caffeine, a weak base. The chemical formula of caffeine is C8H10N4O2.
Like many narcotic drugs, cocaine is a weak base. Its chemical formula is C17H21NO4. Write the chemical equation for the ionization of this weak base in aqueous solution.
Hydrazine, N2H4, is weak base with Kb = 1.3 × 10-6. Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a 0.10 M solution.
Hydroxylamine, NH2OH, is a weak base with Kb = 8.7 × 10-9. Fill in the iCe table and write the equation needed to solve for the concentration of hydroxide ion in a 0.10 M solution.
Coniine (2-propylpiperidine) is a weak base. It has the formula C8H17N. Calculate the pH of a 0.500 M solution of coniine (pKb = 3.1). Coniine is extracted from the plant Conium maculatum, also called hemlock. This harmless-looking relative of the carrot produces a deadly poison that killed the
Morphine, C17H19O3N, is a weak base with Kb = 1.6 × 10-6. It is a prescription drug used to deaden pain; the average dose is 10 mg. Calculate the pH of a 0.0010 M solution.
Calculate the [OH-] and the pH of a 0.024 M methylamine solution; Kb = 4.2 × 10-4.
Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the base ionization constant for the following ions.(a) Formate ion(b) Nitrite ionTables 15.6
Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the base ionization constant for the following ions.(a) Chlorite ion(b) Fluoride ionTable 15.6Table 15.8
Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the acid ionization constant for the following ions.(a) Hydroxylammonium ion(b) Ammonium ionTable 15.6Table 15.8
Write the chemical equation and use the data in Tables 15.6 and 15.8 to calculate the acid ionization constant for the following ions.(a) Pyridinium ion(b) Hydrazinium ionTable 15.6Table 15.8
Find the value of Kb for the conjugate base of the following organic acids.(a) Picric acid used in the manufacture of explosives;Ka = 0.16(b) Trichloroacetic acid used in the treatment of warts;Ka = 0.20
Consider sodium acrylate, NaC3H3O2. Ka for acrylic acid (its conjugate acid) is 5.5 × 10-5.(a) Write a balanced net ionic equation for the reaction that makes aqueous solutions of sodium acrylate basic.(b) Calculate Kb for the reaction in (a).(c) Find the pH of a solution prepared by dissolving
Rank the following species in order of increasing acidity: NH+4, H2O, HF, HSO-4.
Rank the following species in order of increasing acidity: HF, HCl, NH+4, NH3.
Rank the following species in order of increasing acidity: CH3COOH, H2O, HCOOH, F-.
Rank the following species in order of increasing acidity: HCl, NH3, HF, Na+.
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.(a) 0.050 M NaF(b) 0.100 M KCl(c) 0.080 M NH4Br
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.(a) 0.150 M NaHSO4(b) 0.050 M Na3PO4(c) 0.100 M KBr
Write the iCe table and the equation needed to calculate the hydrogen ion concentration in 0.060 M pyridinium iodide.
Write the iCe table and the equation needed to calculate the hydrogen ion concentration in 1.5 M ammonium chloride.
Calculate the pH of each of the following solutions.(a) 0.010 M sodium acetate(b) 0.125 M ammonium nitrate(c) 0.400 M potassium chlorite
Calculate the pH of each of the following solutions.(a) 0.25 M potassium nitrite(b) 0.50 M sodium formate(c) 0.015 M sodium fluoride
State whether 1 M solutions of the following salts in water would be acidic, basic, or neutral.(a) FeCl3(b) BaI2(c) NH4NO2(d) Na2HPO4(e) K3PO4
State whether solutions of the following salts in water would be acidic, basic, or neutral.(a) 0.1 M NH3(b) 0.1 M Na2CO3(c) 0.1 M NaCl(d) 0.1 M CH3CO2H(e) 0.1 M NH4Cl(f) 0.1 M NaCH3CO2(g) 0.1 M NH4CH3CO2
Explain how to calculate the pH of a solution that is 0.20 M CH3COOH and 0.050 M HI.
Explain how to calculate the pH of a solution that is 0.050 M HCl and 0.15 M HF.
Explain how to calculate the pH of a solution that is 0.10 M acetic acid and 0.20 M HCN.
Explain how to calculate the pH of a solution that is 0.050 M formic acid and 0.050 M phenol.
Hypofluorous acid, HOF, is known, but fluorous acid, HOFO, is not. Which acid would you expect to be stronger?
Without referring to a table in this chapter, match the acid with its acid ionization constant. You should give the formulas of these acids.
Which of each pair of acids is stronger? Why?(a) GeH4, AsH3(b) HNO2, HNO3
Which of each pair of acids is stronger? Why?(a) H3AsO3, H3AsO4(b) PH3, H2S
Which of each pair of acids is stronger? Why?(a) HClO3, HClO4(b) H2S, H2Se
Which of each pair of acids is stronger? Why?(a) HClO, HClO2(b) H2S, H2O
State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted–Lowry, and Lewis.
State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted–Lowry, and Lewis.
State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted–Lowry, and Lewis.
State whether each of the following reactions is an acidbase reaction, according to the definitions of Arrhenius, Brønsted–Lowry, and Lewis.
Decide whether each of the following substances should be classified as a Lewis acid or a Lewis base.(a) BCl3(b) H2NNH2, hydrazine(c) The reactants in
Identify the Lewis acid and the Lewis base in each reaction.
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.
Choose from among the labels strongly acidic, weakly acidic, neutral, weakly basic, and strongly basic to estimate the pH of the following solutions.
Calculate the fraction of benzoic acid, a useful food preservative, which is ionized in 0.010- and 0.0010 M solutions.
Phenol (C6H5OH, also called carbolic acid) has a pKa of 9.89. It is used to preserve body tissues and is quite toxic. Calculate the fraction of the acid ionized in 0.010 M and 0.0010 M phenol.
Calculate the volume of 0.083 M HNO2 that must be dissolved to make 1.00 L of a solution with a pH of 4.75.
Calculate the volume of 0.10 M acetic acid needed to prepare 5.0 L of acetic acid solution with a pH of 4.00.
Calculate the mass of benzoic acid, C6H5COOH, which must be dissolved to prepare 1.00 L of a solution with a pH of 3.50.
Calculate the volume of 14.3 M HCl that must be used to prepare 100.0 L of a solution with a pH of 3.50.
A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to exactly 500 mL. Calculate the pH of the resulting solution.
Liquid HF undergoes an autoionization reaction:(a) Is KF an acid or a base in this solvent?(b) Perchloric acid, HCIO4, is a strong acid in liquid HF. Write the chemical equation for the ionization reaction.(c) Ammonia is a strong base in this solvent. Write the chemical equation for the
Pure liquid ammonia ionizes in a manner similar to that of water.(a) Write the equilibrium for the autoionization of liquid ammonia.(b) Identify the conjugate acid form and the base form of the solvent.(c) Is NaNH2 an acid or a base in this solvent?(d) Is ammonium bromide an acid or a base in
Calculate the pH of 0.050 M solutions of the following solutes.(a) Benzoic acid(b) Sodium benzoate
Calculate the pH of 0.25 M solutions of the following solutes.(a) Hydrofluoric acid(b) Potassium fluoride
Determine whether each of the following reactions favors the reactants, products, or neither.
Determine whether each of the following reactions favors the reactants, products, or neither.
A solution is made by diluting 10.0 mL of concentrated ammonia (28% by weight; density = 0.90 g/mL) to exactly 1 L. Calculate the pH of the solution.
An aqueous solution contains formic acid and formate ion. Determine the direction in which the pH will change if each of the following chemicals is added to the solution.(a) HCl(b) NaHSO4(c) CH3COONa(d) KBr(e) H2O
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution.(a) Calculate the pH and pOH in the fi nal solution.(b) Why
Calculate the pH of a solution prepared by adding 10.0 g sodium benzoate to 100 mL of 0.10 M KOH.
Calculate the pH of a solution prepared by adding exactly 10.0 mL of a 14.8 M KOH solution to 200 mL of water, then adding water until the volume of solution is exactly 250 mL.
Calculate the pH of a solution prepared by mixing 10 mL of 1.0 M NaOH with 100 mL of 0.10 M ammonia.
When perchloric acid ionizes, it makes the perchlorate ion, ClO-4 . Draw the Lewis electron dot symbol for the perchlorate ion.
Picric acid, or 2,4,6-trinitrophenol, has the following structure:Not only is it an acid, it is also an explosive.(a) Based on what you know of oxyacids, which hydrogen ionizes from the picric acid molecule?(b) Picric acid has a Ka of 0.380. What is the pH of a 0.100 M solution of picric acid? You
Acids in the news.(a) Chemists often talk about the United States senator who addressed the public about acid rain and said: “I too abhor the effects of acid rain and I pledge the United States Senate will fight to reduce acidity of rain until pH is zero!” Is battling acid rain by reducing the
Calculate the equivalence-point volume in the titration of 50.00 mL of 0.0884 M nitric acid with 0.0980 M NaOH. The titration curve for this system appears in Figure 16.2.StrategyUse the concentration and volume of the acid (both given) to calculate the number of moles of acid. Then use the
Calculate the number of millimoles of HCl needed to neutralize 10.0 mL of 0.15 M Ba(OH)2.StrategyFirst, write the chemical equation for the neutralization. Calculate the amount of barium hydroxide, and use the stoichiometric relationship to calculate the amount of HCl.
Calculate the pH in the titration of 20.00 mL of 0.125 M HCl after the addition of(a) 0,(b) 2.00,(c) 10.00, and(d) 20.00 mL of 0.250 M NaOH.StrategyFirst, calculate the amounts (mmol) of acid and base. The analyte and the titrant (acid and base) react with each other, and this reaction goes to
Estimate the pH of a solution formed by mixing(a) 100 mL of 0.2 M HCl with 50 mL of 0.2 M NaOH(b) 100 mL of 0.2 M HCl with 100 mL of 0.2 M NaOHStrategyWrite the net ionic equation, calculate numbers of millimoles of each species, and fill in the sRf table. Look at the species on the f line to
Calculate the pH of a solution that is 0.40 M sodium acetate and 0.20 M acetic acid.Ka for acetic acid is 1.8 × 10-5.StrategyThe solution contains a weak acid and its conjugate base, so it is a buffer. Use the Henderson–Hasselbalch equation to solve for the pH of a buffer system. The analytical
Calculate the mass of ammonium chloride that must be added to 500.0 mL of 0.32 M NH3 to prepare a pH 8.50 buffer; Kb for NH3 is 1.8 × 10-5.Strategy We need to calculate the amount of the acid (NH4+ ions from NH4Cl) that we must add to prepare an ammonium/ammonia buffer of pH 8.50. It will be
Calculate the change in pH observed when 1.50 mL of 0.0670 M H3O+ is added to(a) 100.0 mL of an unbuffered HCl solution of pH 4.74(b) 100.0 mL of a pH 4.74 buffer that is 0.120 M acetic acid and 0.120 M sodium acetate (the pKa for acetic acid is 4.74 ).(a) Calculate the change in pH observed when
Calculate the pH during the titration of 20.0 mL of 0.500 M formic acid ( Ka = 1.8 × 10-4) with 0.500 M NaOH. Calculate the pH after 0, 10.0, 20.0, and 30.0 mL of NaOH have been added, and sketch the titration curve.StrategyFirst, write the chemical equation for the titration and calculate the
Choose an indicator for the titration of acetic acid in a sample of red wine vinegar with sodium hydroxide (in the burette). Justify your choice.StrategyFirst, sketch the general shape of the titration curve. Choose the pH range where the pH is changing most quickly, which is just beyond the
Calculate the concentrations of all species in 0.500 M sulfurous acid.StrategyLook at the values for Ka1 and Ka2. If Ka1 is much greater than Ka2, then Ka1 will dominate the equilibrium, and calculations are similar to those of a monoprotic weak acid with Ka equal to Ka1.
Write the equilibria of 0.10 M sodium hydrogen sulfite, and determine whether its pH is greater than or less than 7.StrategyFirst, write the chemical reactions in which the amphoteric species acts as an acid, and the reaction in which it acts as a base. Next, write the expression for the

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