Introductory Chemistry: A Foundation
9th Edition
ISBN: 9781337399425
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 17, Problem 85AP
. What is meant by the solubility product for a sparingly soluble salt? Choose a sparingly soluble salt and show how the salt ionizes when dissolved in water, and write the expression for its solubility product.
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7.
A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant of
ammonia, NH3, is 1.815x10-5
A student worker is asked to prepare a buffer solution with NH3 and ammonium salt. However, after the student did a thorough search,
no ammonium salt is found. After the student reported the result to the professor, the professor told the student the buffer can be
prepared with ammonia and a strong acid.
Can you help this student out?
The pH of the buffer to be prepared is 10.08. The molarity of the ammonia in the buffer is 0.4717 M. The molarity of the ammonia solution
found in the laboratory is 1.201 M, the strong acid solution is 0.9948 M HNO3. The volume of the buffer solution to be prepared is 500.0
mL.
Please answer the following questions.
A.
B.
What is the molarity of the ammonium ion in the buffer?
Please provider your answer below.
Check answer
How many mL of 0.9948 M HNO3 solution is needed?
Please provider your answer below.
0² 0₂
$…
An aqueous solution contains 0.26 M ammonium nitrate.
One liter of this solution could be converted into a buffer by the addition of:
(Assume that the volume remains constant as each substance is added.)
0.06 mol Ba(OH)2
0.26 mol HCI
0.26 mol Ca(NO3)2
0.26 mol NH3
0.12 mol HCI
Why does changing the temperature of the reaction site shift a chemical equilibrium?
What is the most important buffer in medicine? Why is it the most important?
Hydrochloric acid, if concentrated enough, can “eat” through metal. How? Describe the
reaction that occurs?
Chapter 17 Solutions
Introductory Chemistry: A Foundation
Ch. 17.2 - Most modern refrigerators have an internal...Ch. 17.2 - Many conditions need to be met to produce a...Ch. 17.5 - Prob. 17.1SCCh. 17.6 - Prob. 17.2SCCh. 17.7 - Prob. 17.3SCCh. 17.7 - Prob. 17.4SCCh. 17.7 - Exercise 17.5 For the exothermic reaction...Ch. 17.9 - Prob. 17.6SCCh. 17.9 - Prob. 17.7SCCh. 17.9 - The Kspvalue for lead chromate, PbCrO4, is...
Ch. 17 - Consider an equilibrium mixture of four chemicals...Ch. 17 - The boxes shown below represent a set of initial...Ch. 17 - For the reaction H2+I22HI, consider two...Ch. 17 - Given the reaction A+BC+D, consider the following...Ch. 17 - Consider the reaction A+BC+D. A friend asks the...Ch. 17 - Prob. 6ALQCh. 17 - The value of the equilibrium constant, K, is...Ch. 17 - You are browsing through the Handbook of...Ch. 17 - What do you suppose happens to the Ksp, value of a...Ch. 17 - . Consider an equilibrium mixture consisting of...Ch. 17 - . Equilibrium is microscopically dynamic but...Ch. 17 - In Section 17.3 of your text, it is mentioned that...Ch. 17 - Prob. 13ALQCh. 17 - . Consider the figure below in answering the...Ch. 17 - For a chemical reaction to take place, some or all...Ch. 17 - For the simple reaction 2H2(g)+O2(g)2H2O(l)list...Ch. 17 - How do chemists envision reactions taking place in...Ch. 17 - When molecules collide, a certain minimum energy...Ch. 17 - How does a catalyst work to speed up a chemical...Ch. 17 - Why are enzymes important? For example, what is...Ch. 17 - How does equilibrium represent the balancing of...Ch. 17 - Consider the equilibrium process depicted in Fig....Ch. 17 - When writing a chemical equation for a reaction...Ch. 17 - . How do chemists recognize a system that has...Ch. 17 - . What does it mean to say that a state of...Ch. 17 - . Consider an initial mixture of N2 and H2 gases...Ch. 17 - . In general terms. what does the equilibrium...Ch. 17 - . There is only one value of the equilibrium...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Suppose that for the reaction...Ch. 17 - . Ammonia. a very important industrial chemical....Ch. 17 - . At high temperatures, elemental nitrogen and...Ch. 17 - . Suppose that for the reaction...Ch. 17 - . What is a homogeneous equilibrium system? Give...Ch. 17 - . True or false? The position of a heterogeneous...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Indicate whether the stated equilibrium...Ch. 17 - . In your own words, describe what Le Châtelier’s...Ch. 17 - . Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose...Ch. 17 - . For an equilibrium involving gaseous substances,...Ch. 17 - . What is the effect on the equilibrium position...Ch. 17 - . For the reaction system...Ch. 17 - . For the reaction system P4(s)+6F2(g)4PF3(g)which...Ch. 17 - . Suppose the reaction system...Ch. 17 - . Consider the general reaction...Ch. 17 - . Hydrogen gas and chlorine gas in the presence of...Ch. 17 - . Hydrogen gas, oxygen gas, and water vapor are in...Ch. 17 - . The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is...Ch. 17 - . Old fashioned “smelling salts” consist of...Ch. 17 - . Plants synthesize the sugar dextrose according...Ch. 17 - . Consider the exothermic reaction...Ch. 17 - . Suppose are action has the equilibrium constant...Ch. 17 - . Suppose a reaction has the equilibrium constant...Ch. 17 - . For the reaction Br2(g)+5F2(g)2BrF5(g)the system...Ch. 17 - . Consider the reaction...Ch. 17 - . For the reaction 2CO(g)+O2(g)2CO2(g)it is found...Ch. 17 - . For the reaction CO2(g)+H2(g)CO(g)+H2O(g)the...Ch. 17 - . The equilibrium constant for the reaction...Ch. 17 - . For the reaction 2H2O(g)2H2(g)+O2(g)K=2.4103at a...Ch. 17 - . For the reaction 3O2(g)2O3(g)The equilibrium...Ch. 17 - . For the reaction N2O4(g)2NO(g)the equilibrium...Ch. 17 - . Explain how the dissolving of an ionic solute in...Ch. 17 - . What is the special name given to the...Ch. 17 - . Why does the amount of excess solid solute...Ch. 17 - . Which of the following will affect the total...Ch. 17 - . Write the balanced chemical equation describing...Ch. 17 - . Write the balanced chemical equation describing...Ch. 17 - . K for copper(II)hydroxide, Cu(OH)2, has a value...Ch. 17 - Prob. 60QAPCh. 17 - . A saturated solution of nickel(II) sulfide...Ch. 17 - . Most hydroxides are not very soluble in water....Ch. 17 - . The solubility product constant, Ksp, for...Ch. 17 - . Calcium sulfate, CaSO4, is only soluble in water...Ch. 17 - . Approximately 1.5103of iron(II) hydroxide....Ch. 17 - . Chromiurn(III) hydroxide dissolves in water only...Ch. 17 - . Magnesium fluoride dissolves in water to the...Ch. 17 - . Lead(II) chloride, PbCl2(s), dissolves in water...Ch. 17 - . Mercury(I) chloride, Hg2Cl2, was formerly...Ch. 17 - . The solubility product of iron(III) hydroxide is...Ch. 17 - . Before two molecules can react, chemists...Ch. 17 - . Why does an increase in temperature favor an...Ch. 17 - . The minimum energy required for molecules to...Ch. 17 - . A(n) _______ speeds up a reaction without being...Ch. 17 - . Equilibrium may be defined as the ________ of...Ch. 17 - . When a chemical system has reached equilibrium,...Ch. 17 - . What does it mean to say that all chemical...Ch. 17 - . What does it mean to say that chemical...Ch. 17 - . At the point of chemical equilibrium, the rate...Ch. 17 - . Equilibria involving reactants or products in...Ch. 17 - . According to Le Châtelier’s principle, when a...Ch. 17 - . Addition of an inert substance (one that does...Ch. 17 - . When the volume of a vessel containing a gaseous...Ch. 17 - . Consider the following reaction at some...Ch. 17 - . What is meant by the solubility product for a...Ch. 17 - . For a given reaction at a given temperature, the...Ch. 17 - . Many sugars undergo a process called...Ch. 17 - . Suppose K=4.5103at a certain temperature for the...Ch. 17 - . For the reaction CaCO3(s)CaO(s)+CO2(g)the...Ch. 17 - Prob. 90APCh. 17 - . Teeth and bones are composed, to a first...Ch. 17 - . Under what circumstances can we compare the...Ch. 17 - . How does the collision model account for the...Ch. 17 - Prob. 94APCh. 17 - . Explain why the development of a vapor pressure...Ch. 17 - Prob. 96APCh. 17 - Prob. 97APCh. 17 - . For the reaction N2(g)+3Cl2(g)2NCl3(g)an...Ch. 17 - . Gaseous phosphorus pentachloride decomposes...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Consider the following generic reaction:...Ch. 17 - Prob. 103APCh. 17 - . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124...Ch. 17 - Prob. 105APCh. 17 - . For the reaction N2(g)+3H2(g)2NH3(g)K=1.3102at a...Ch. 17 - . The equilibrium constant for the reaction...Ch. 17 - Prob. 108APCh. 17 - Prob. 109APCh. 17 - Prob. 110APCh. 17 - . Mercuric sulphide, HgS, is one of the least...Ch. 17 - Prob. 112APCh. 17 - . For the reaction N2(g)+3H2(g)2NH3(g), list the...Ch. 17 - . What does the activation energy for a reaction...Ch. 17 - Prob. 115APCh. 17 - Prob. 116APCh. 17 - Prob. 117APCh. 17 - Prob. 118APCh. 17 - Prob. 119APCh. 17 - Prob. 120CPCh. 17 - . Suppose that for a hypothetical reaction:...Ch. 17 - Prob. 122CPCh. 17 - . The reaction H2(g)+I2(g)2HI(g)has Kp=45.9at 763...Ch. 17 - Prob. 124CPCh. 17 - Prob. 125CPCh. 17 - . Consider the following exothermic reaction at...Ch. 17 - Prob. 1CRCh. 17 - Prob. 2CRCh. 17 - Prob. 3CRCh. 17 - How is the strength of an acid related to the...Ch. 17 - Prob. 5CRCh. 17 - How is the pH scale defined? What range of pH...Ch. 17 - 7. Describe a buffered solution. Give three...Ch. 17 - Prob. 8CRCh. 17 - Prob. 9CRCh. 17 - . Explain what it means that a reaction has...Ch. 17 - . Describe how we write the equilibrium expression...Ch. 17 - Prob. 12CRCh. 17 - Prob. 13CRCh. 17 - . In your own words, paraphrase Le Châtelier’s...Ch. 17 - Prob. 15CRCh. 17 - Prob. 16CRCh. 17 - . a. Write the conjugate acid for each of the...Ch. 17 - . Identify the Brønsted-Lowry conjugate acid-base...Ch. 17 - Prob. 19CRCh. 17 - Prob. 20CRCh. 17 - Prob. 21CRCh. 17 - Prob. 22CRCh. 17 - Prob. 23CRCh. 17 - . The solubility product of magnesium carbonate,...
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- 7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?arrow_forwardWhich of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.arrow_forwardUse Le Chátelier's principle to explain what happens to the equilibrium H2O(l)H+(aq)+OH(aq) when a few drops of HCl are added to pure water.arrow_forward
- Calculate the pH of these buffers.arrow_forwardC. Titration of Strong Base with Weak Acids a. Titration Curves for Weak Acids with strong base To generate the titration curves for weak acids titrated with strong base, we have to to employ four distinctly different types of calculations to compute values for a weak acid. 1. At the beginning, the solution contains only a weak acid and the pH is calculated from the concentration of the given solute and its dissociation constant. 2. After several increments of titrant have been added but not including, the equivalence point, the solution consists of a series of buffers. The pH of each buffer is calculated from the analytical concentrations of the conjugate base and the concentrations of the weak acid. 3. At the equivalence point, the solution contains only the conjugate of the weak base or the salt being titrated, and the pH is calculated from the concentration of this product. 4. Beyond the equivalence point, the excess of strong base titrant suppressesarrow_forwardAn aqueous solution contains 0.18 M ammonium nitrate.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added.) more than one can be selected. 0.08 mol HBr 0.18 mol HBr 0.17 mol NH3 0.17 mol Ba(NO3)2 0.04 mol Ba(OH)2arrow_forward
- An aqueous solution contains 0.22 M ammonium chloride. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.22 mol HBr 0.10 mol HBr 0.10 mol KOH O 0.21 mol NH3 O 0.21 mol CaCl,arrow_forwardIn a laboratory experiment, a student has 1 L of solution containing a weak base at a concentration of 0.300 M. In order to create a buffer, a strong acid is added, which converts some of the base in the solution to its conjugate weak acid to create a buffer. If the student wants to create the most effective buffer that can be equally resistant to both acids and bases how many moles of strong acid should the student add to the buffer? (Please provide your answer to 3 decimal places.)arrow_forwarda buffer solution is prepared by mixing the solution of a weak acid with its salt.Write two expressions that show what happens when two substances are dissolved in water. b) Based on the answer you gave to the above question explain why the pH of a buffer solution does not change even if we add a little acid.arrow_forward
- A buffer solution contains 0.221 M hydrocyanic acid and 0.453 M potassium cyanide. If 0.0495 moles of nitric acid are added to 225 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding nitric acid) PHarrow_forwardA buffer solution contains a mixture of a weak acid and a weak base, typically the conjugate base of the weak acid. For example, a buffer solution commonly used in chemistry laboratories contains both acetic acid (, a weak acid) and sodium acetate (, the sodium salt of the conjugate base of acetic acid). Some other examples of buffers are ( is a weak acid and is a weak base) and ( is a weak acid and is a weak base). Identify buffer solutions from the following list.Choose all that apply. A. 0.22 M perchloric acid + 0.23 M potassium perchlorate. B. 0.15 M sodium hydroxide + 0.29 M sodium bromide. C. 0.31 M ammonia + 0.33 M ammonium nitrate. D. 0.10 M hydrofluoric acid + 0.16 M potassium fluoride. E. 0.38 M potassium chloride + 0.27 M potassium bromide.arrow_forwardExpress the solubility equilibrium of the generally insoluble salt CuOH.arrow_forward
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