Concept explainers
(a)
Interpretation: The solubility of
Concept introduction: The constant
(b)
Interpretation: The concentration of
Concept introduction: The constant
(c)
Interpretation: The concentration of
Concept introduction: The constant
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Chapter 16 Solutions
Study Guide for Zumdahl/Zumdahl/DeCoste’s Chemistry, 10th Edition
- Write equations for the stepwise formation of each of the following complex ions. a. CoF63 b. Zn(NH3)42+arrow_forwardCu2+(aq) + H2O(l) ⇌ CuOH+(aq) + H+(aq) Keq = 1.2 x 10−8 A 1.00 M solution of copper(II) nitrate is created and the system shown above reaches equilibrium. What happens to the pH of the system if more CuOH+ is added after reaching equilibrium? The pH of the system will not change because of the small size of K. The pH of the system will increase because of the increased concentration of CuOH+. The pH of the system will increase as the reverse reaction proceeds at a faster rate to reestablish equilibrium. The pH of the system will decrease as the forward reaction proceeds at a faster rate to reestablish equilibrium.arrow_forward理 E The equilibrium concentration of hydroxide ion in a saturated cobalt(II) hydroxide solution isarrow_forward
- Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? The flask will be colorless. The flask will be pink. The flask will be white from KCl precipitation. There is insufficient information to solve this problemarrow_forwardPotassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? The flask will be colorless. The flask will be pink. The flask will be white from KCl precipitation. There is insufficient information to solve this problemarrow_forwardPotassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? a. The flask will be pink b. The flask will be colorless c. The flask will be white from KCl precipitation d. There is insufficient information to solve this problemarrow_forward
- Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH?arrow_forwardPotassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction. HIn + H2O ⇌ In− + H3O+ If the HIn species is "acid color" or colorless for the phenolphthalein, and the In− species is "base color" or pink for this particular indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH? A. The flask will be colourless B. The flask will be pink C. The flask will be white from KCI precipitation D. There is insufficient information to solve this problemarrow_forwardWhat is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16arrow_forward
- What is the equilibrium expression for the following reaction? Zn(s) + 2NaOH(aq) + 2H2O(ℓ) ⇌ Na2Zn(OH)4(aq) + H2(g)arrow_forwardCo(H2O)62+(aq) + 4 Cl–(aq)⇄CoCl42–(aq) + 6 H2O What happens to the equilibrium using Le Chateliers principle when DI water is added to this? What about when silver nitrate was added? Any precipitate formed? If so, what is the precipitate?arrow_forwardWhat is the equilibrium molar concentration of Cu+ in a solution prepared by adding 0.1558 mol of CuNO3 to a solution of CN-? The final volume of the solution was 1.00 L and the concentration of CN- was 2.7046 M before equilibrium was established.Cu+(aq) + 2CN-(aq)↔[Cu(CN)2]-(aq) Kf = 1.00e16 a) 2.79E-18 b) 9.05E-17 c) 2.09E-18 d) 3.71E-18arrow_forward
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning