Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 17, Problem 15PS
A buffer is composed of formic acid and its conjugate base, the formate ion.
- (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M?
- (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
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The drawing below represents a buffer composed of equal concentrations of a weak
acid, HX, and its conjugate base, X-'. The heights of the columns are proportional to
the concentrations of the components of the buffer. (a) Which of the three drawing
(1), (2), or (3) represents the buffer after the addition of a strong acid? Explain. (b)
Which of the three represents the buffer after the addition of a strong base? Explain.
HX X
HX X-
HX X
HX X
(1)
(2)
(3)
Copyright © 2006 Pearson Prentice Hall, Inc.
(a) Calculate the pH of a buffer solution containing 0.40 mole of KF and 0.50 mol of HF in 1.50 liter solution. (Ka of HF is 7.2*10–4); 15.0 mL of 1.00 M HCl is added to the original buffer in question (a).
(b) Show the equation of reaction which take place when HCl is added.
(c) What will the pH of the buffer solution in question (a) be after the addition of 15.0 mL of 1.00 M HCl.
Consider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.)
(a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid?
(only need help witn c and d)
Chapter 17 Solutions
Chemistry & Chemical Reactivity
Ch. 17.1 - You have a 0.30 M solution of formic acid (HCO2H)...Ch. 17.1 - 1. What is the pH of the solution that results...Ch. 17.2 - What is the pH of a buffer solution composed of...Ch. 17.2 - Use the Henderson-Hasselbalch equation to...Ch. 17.2 - Using an acetic acid/sodium acetate buffer...Ch. 17.2 - Calculate the pH of 0.500 L of a buffer solution...Ch. 17.2 - 1. Which choice would be a good buffer...Ch. 17.2 - 2. If an acetic acid/sodium acetate buffer...Ch. 17.2 - Prob. 3RCCh. 17.2 - 4. To prepare a buffer containing CH3CO2H and...
Ch. 17.3 - The titration of 0.100 M acetic acid with 0.100 M...Ch. 17.3 - Calculate the pH after 75.0 mL of 0.100 M HO has...Ch. 17.3 - 1. What is the pH after 25.0 ml of 0.100 M NaOH...Ch. 17.3 - 2. What is the pH at the equivalence point in the...Ch. 17.3 - Prob. 3RCCh. 17.3 - Phosphate ions are abundant in cells, both as the...Ch. 17.3 - A typical total phosphate concentration in a cell,...Ch. 17.4 - The barium ion concentration, [Ba2+], in a...Ch. 17.4 - Calculate the solubility of AgCN in moles per...Ch. 17.4 - Calculate the solubility of Ca(OH)2 in moles per...Ch. 17.4 - Calculate the solubility of BaSO4 (a) in pure...Ch. 17.4 - 12. Calculate the solubility of Zn(CN)2 at 25°C...Ch. 17.4 - What is the Ksp expression for silver carbonate?...Ch. 17.4 - 2. Using Ksp values, predict which salt in each...Ch. 17.4 - What is the solubility of PbSO4 in water at 25C?...Ch. 17.4 - 4. What is the solubility of PbSO4 in water at...Ch. 17.4 - Prob. 5RCCh. 17.5 - Solid Pbl2 (Ksp = 9.8 109) is placed in a beaker...Ch. 17.5 - Prob. 2CYUCh. 17.5 - Prob. 3CYUCh. 17.5 - 1. Will SrSO4 precipitate from a solution...Ch. 17.6 - Silver nitrate (0.0050 mol) is added to 1.00 L of...Ch. 17.6 - 1. Iron(II) chloride (0.025 mol) is added to 1.00...Ch. 17.7 - Calculate the value of the equilibrium constant,...Ch. 17.7 - 1. What is the equilibrium constant for the...Ch. 17.7 - Prob. 1QCh. 17.7 - What is the minimum volume of 0.0071 M NaCN(aq)...Ch. 17.7 - Use the formation constant of [Au(CN)2] in...Ch. 17.7 - Silver undergoes similar reactions as those shown...Ch. 17.7 - Write a balanced chemical equation for the...Ch. 17 - Does the pH of the solution increase, decrease or...Ch. 17 - Does the pH of the solution increase, decrease, or...Ch. 17 - What is the pH of a solution that consists of 0.20...Ch. 17 - What is the pH of 0.15 M acetic acid to which 1.56...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the solution that results from...Ch. 17 - What is the pH of the buffer solution that...Ch. 17 - Lactic acid (CH3CHOHCO2H) is found in sour milk,...Ch. 17 - What mass of sodium acetate, NaCH3CO2, must he...Ch. 17 - What mass of ammonium chloride, NH4Cl, must be...Ch. 17 - Calculate the pH of a solution that has an acetic...Ch. 17 - Calculate the pH of a solution that has an...Ch. 17 - What must the ratio of acetic acid to acetate ion...Ch. 17 - What must the ratio of H2PO4 to HPO42 be to have a...Ch. 17 - A buffer is composed of formic acid and its...Ch. 17 - A buffer solution is composed of 1.360 g of KH2PO4...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Which of the following combinations would be the...Ch. 17 - Describe how to prepare a buffer solution from...Ch. 17 - Describe how to prepare a buffer solution from NH3...Ch. 17 - Determine the volume (in mL) of 1.00 M NaOH that...Ch. 17 - Determine the volume (in mL) of 1.00 M HC1 that...Ch. 17 - A buffer solution was prepared by adding 4.95 g of...Ch. 17 - You dissolve 0.425 g of NaOH in 2.00 L of a buffer...Ch. 17 - A buffer solution is prepared by adding 0.125 mol...Ch. 17 - What is the pH change when 20.0 mL of 0.100 M NaOH...Ch. 17 - Phenol, C6H5OH, is a weak organic acid. Suppose...Ch. 17 - Assume you dissolve 0.235 g of the weak acid...Ch. 17 - You require 36.78 mL of 0.0105 M HCl to reach the...Ch. 17 - A titration of 25.0 mL of a solution of the weak...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - Without doing detailed calculations, sketch the...Ch. 17 - You titrate 25.0 mL of 0.10 M NH3 with 0.10 M HCl....Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Using Figure 17.11, suggest an indicator to use in...Ch. 17 - Name two insoluble salts of each of the following...Ch. 17 - Prob. 38PSCh. 17 - Using the solubility guidelines (Figure 3.10),...Ch. 17 - Predict whether each of the fallowing is insoluble...Ch. 17 - For each of the following insoluble salts, (1)...Ch. 17 - Prob. 42PSCh. 17 - When 1.55 g of solid thallium(I) bromide is added...Ch. 17 - At 20 C, a saturated aqueous solution of silver...Ch. 17 - When 250 mg of SrF2, strontium fluoride, is added...Ch. 17 - Calcium hydroxide, Ca(OH)2, dissolves in water to...Ch. 17 - You add 0.979 g of Pb(OH)2 to 1.00 L of pure water...Ch. 17 - You place 1.234 g of solid Ca(OH)2 in 1.00 L of...Ch. 17 - Estimate the solubility of silver iodide in pure...Ch. 17 - What is the molar concentration of Au+(aq) in a...Ch. 17 - Prob. 51PSCh. 17 - Estimate the solubility of lead(II) bromide (a) in...Ch. 17 - The Ksp value for radium sulfate, RaSO4, is 4.2 ...Ch. 17 - If 55 mg of lead(II) sulfate is placed in 250 mL...Ch. 17 - Prob. 55PSCh. 17 - Prob. 56PSCh. 17 - Calculate the molar solubility of silver...Ch. 17 - Calculate the solubility of silver bromide, AgBr,...Ch. 17 - Compare the solubility, in milligrams per...Ch. 17 - What is the solubility, in milligrams per...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Calculate the solubility, in moles per liter, of...Ch. 17 - Which insoluble compound in each pair should be...Ch. 17 - Which compound in each pair is more soluble in...Ch. 17 - You have a solution that has a lead(II) ion...Ch. 17 - Sodium carbonate is added to a solution in which...Ch. 17 - If the concentration of Zn2+ in 10.0 mL of water...Ch. 17 - You have 95 mL of a solution that has a lead(II)...Ch. 17 - Prob. 69PSCh. 17 - Will a precipitate of Mg(OH)2 form when 25.0 mL of...Ch. 17 - Zinc hydroxide is amphoteric (Section 16.10). Use...Ch. 17 - Solid silver iodide, AgI, can be dissolved by...Ch. 17 - What amount of ammonia (moles) must be added to...Ch. 17 - Can you dissolve 15.0 mg of AuCl in 100.0 mL of...Ch. 17 - What is the solubility of AgCl (a) in pure water...Ch. 17 - Prob. 76PSCh. 17 - Prob. 77GQCh. 17 - Prob. 78GQCh. 17 - Prob. 79GQCh. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - Calculate the hydronium ion concentration and the...Ch. 17 - For each of the following cases, decide whether...Ch. 17 - Prob. 83GQCh. 17 - A sample of hard water contains about 2.0 103 M...Ch. 17 - What is the pH of a buffer solution prepared from...Ch. 17 - Prob. 86GQCh. 17 - Describe the effect on the pH of the following...Ch. 17 - What volume of 0.120 M NaOH must be added to 100....Ch. 17 - A buffer solution is prepared by dissolving 1.50 g...Ch. 17 - What volume of 0.200 M HCl must be added to 500.0...Ch. 17 - What is the equilibrium constant for the following...Ch. 17 - Calculate the equilibrium constant for the...Ch. 17 - Prob. 93GQCh. 17 - The solubility product constant for calcium...Ch. 17 - In principle, the ions Ba2+ and Ca2+ can be...Ch. 17 - A solution contains 0.10 M iodide ion, I, and 0.10...Ch. 17 - A solution contains Ca2+ and Pb2+ ions, both at a...Ch. 17 - Prob. 98GQCh. 17 - Prob. 99GQCh. 17 - Prob. 100GQCh. 17 - Each pair of ions below is found together in...Ch. 17 - Each pair of ions below is found together in...Ch. 17 - The cations Ba2+ and Sr2+ can be precipitated as...Ch. 17 - You will often work with salts of Fe3+, Pb2+, and...Ch. 17 - Aniline hydrochloride, (C6H5NH3)Cl, is a weak...Ch. 17 - The weak base ethanolamine. HOCH2CH2NH2, can be...Ch. 17 - For the titration of 50.0 mL of 0.150 M...Ch. 17 - A buffer solution with it pH of 12.00 consists of...Ch. 17 - To have a buffer with a pH of 2.50, what volume of...Ch. 17 - What mass of Na3PO4 must be added to 80.0 mL of...Ch. 17 - You have a solution that contains AgNO3, Pb(NO3)2,...Ch. 17 - Prob. 112ILCh. 17 - Suggest a method for separating a precipitate...Ch. 17 - Prob. 114SCQCh. 17 - Prob. 115SCQCh. 17 - Two acids, each approximately 0.01 M in...Ch. 17 - Composition diagrams, commonly known as alpha...Ch. 17 - The composition diagram, or alpha plot, for the...Ch. 17 - The chemical name for aspirin is acetylsalicylic...Ch. 17 - Prob. 120SCQ
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- Calculate the pH of these buffers.arrow_forwardWhat is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.arrow_forwardConsider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forward
- Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardA buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forward
- What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.arrow_forward8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.arrow_forwardWhich of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.arrow_forward
- Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.arrow_forwardIs it possible to prepare a buffer solution using a strong acid and a salt of its conjugate base? Why?arrow_forwardConsider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d pleasearrow_forward
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