Science
ChemistryIntroductory Chemistry: A Foundation7. 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?

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?

BuyFind

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425
BuyFind

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781337399425

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Chapter 17, Problem 7CR
Textbook Problem

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?

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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 - Exercise 17.1 Write the equilibrium expression for...Ch. 17.6 - Exercise 17.2 Write the equilibrium expression for...Ch. 17.7 - Exercise 17.3 Novelty devices for predicting rain...Ch. 17.7 - Exercise 17.4 For each of the following reactions,...Ch. 17.7 - Exercise 17.5 For the exothermic reaction...Ch. 17.9 - Exercise 17.6 Write the balanced equation for the...Ch. 17.9 - Exercise 17.7 Calculate the Kspvalue for barium...Ch. 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 - Consider the following statements: “Consider the...Ch. 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 - . Explain why the development of a vapour pressure...Ch. 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 - . Kspfor magnesium carbonate, MgCO3, has a value...Ch. 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 - . As you know from Chapter 7, most metal carbonate...Ch. 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 - . How does an increase in temperature result in an...Ch. 17 - . Explain why the development of a vapor pressure...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 17 - . Write the equilibrium expression for each of the...Ch. 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 - . Suppose the reaction system...Ch. 17 - . The reaction PCl3(l)+Cl2(g)PCl5(s)liberates 124...Ch. 17 - . For the process CO(g)+H2O(g)CO2(g)+H2(g)it is...Ch. 17 - . For the reaction N2(g)+3H2(g)2NH3(g)K=1.3102at a...Ch. 17 - . The equilibrium constant for the reaction...Ch. 17 - . As you learned in Chapter 7, most metal...Ch. 17 - . The three common silver halides (AgCI, AgBr, and...Ch. 17 - . Approximately 9.0104gof silver chloride....Ch. 17 - . Mercuric sulphide, HgS, is one of the least...Ch. 17 - . Approximately 0.14 g of nickel(II) hydroxide....Ch. 17 - . For the reaction N2(g)+3H2(g)2NH3(g), list the...Ch. 17 - . What does the activation energy for a reaction...Ch. 17 - . What are the catalyss in living cells called?...Ch. 17 - . When a reaction system has reached chemical...Ch. 17 - . Ammonia, a very important industrial chemical,...Ch. 17 - . For the reaction 2CO2(g)2CO(g)+O2(g)an analysis...Ch. 17 - . Suppose a reaction has the equilibrium constant...Ch. 17 - . At a particular temperature, a 3.50-L flask...Ch. 17 - . Suppose that for a hypothetical reaction:...Ch. 17 - . For the reaction: 3O2(g)2O3(g)K=1.8107at a...Ch. 17 - . The reaction H2(g)+I2(g)2HI(g)has Kp=45.9at 763...Ch. 17 - . For the reaction: H2(g)+F2(g)2HF(g)K=2.1103at a...Ch. 17 - . For the following endothermic reaction at...Ch. 17 - . Consider the following exothermic reaction at...Ch. 17 - How are the Arrhenius and Brønsted-Lowry...Ch. 17 - Describe the relationship between a conjugate...Ch. 17 - Acetic acid is a weak acid in water. What does...Ch. 17 - How is the strength of an acid related to the...Ch. 17 - Explain how water is an amphoteric substance....Ch. 17 - How is the pH scale defined? What range of pH...Ch. 17 - 7. Describe a buffered solution. Give three...Ch. 17 - Explain the collision model for chemical...Ch. 17 - Sketch a graph for the progress of a reaction...Ch. 17 - . Explain what it means that a reaction has...Ch. 17 - . Describe how we write the equilibrium expression...Ch. 17 - Although the equilibrium constant for a given...Ch. 17 - . Compare homogeneous and heterogeneous...Ch. 17 - . In your own words, paraphrase Le Châtelier’s...Ch. 17 - . Explain how dissolving a slightly soluble salt...Ch. 17 - . Choose 10 species that might be expected to...Ch. 17 - . a. Write the conjugate acid for each of the...Ch. 17 - . Identify the Brønsted-Lowry conjugate acid-base...Ch. 17 - . For each of the following, calculate the...Ch. 17 - . Calculate the pH and pOH values for each of the...Ch. 17 - . Write the equilibrium constant expression for...Ch. 17 - . Suppose that for the following reaction...Ch. 17 - . Write expressions for Kspfor each of the...Ch. 17 - . The solubility product of magnesium carbonate,...

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