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 7CR
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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• Row 2: Your answer is incorrect.
Row 4: Your answer is incorrect.
The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at
equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the
formulas of the species that will act as neither acids nor bases in the 'other' row.
You will find it useful to keep in mind that NH, is a weak base.
1.3 mol of HI is added to
1.0 L of a 1.3MNH,
solution.
0.22 mol of HNO, is added
to 1.0 1. of a solution that is
1.1M in both NH, and
NH Br.
✔ acids: NH, H,O
bases: 11,0, NHL,
other: I
acids: NH H
bases: NH,
other: NO, Br
a
S
da
X
0.0.
As the pH increases, the solubility of which one of the following would increase?
**Please explain why that is the case or how the reaciton is taking place to understand why the solubility increases**
1. Lead(II) hydroxide
2. barium chloride
3. sodium hydroxide
3. magnesium sulfide
4. aluminum chloride
In an experiment to determine the amount of aspirin in a tablet, one of the
bottles of NaOH used was accidentally left open for 24 hours, which lead to
it reacting with carbon dioxide. What will be the effect on the calculated
amount of aspirin compared to the actual amount in the tablet and the
concentration of the NaOH solution?
Calculated amount increases since NaOH concentration will be lower than original.
Calculated amount increases since NaOH concentration will be higher than original.
Calculated amount decreases since NaOH concentration will be lower than original.
Calculated amount decreases since NaOH concentration will be higher than original.
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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