5. A solution of HF is found to be 0.25M and have K, value of 6.6x104. a. Write the equilibrium reaction for the ionization of HF. b. Write the equilibrium constant expression for the reaction. c. Give the equilibrium constant of HF. d. Calculate the pH of the solution. e. Calculate the pKa of the solution. f. Calculate the pOH of the solution.

5. A solution of HF is found to be 0.25M and have K, value of 6.6x104. a. Write the equilibrium reaction for the ionization of HF. b. Write the equilibrium constant expression for the reaction. c. Give the equilibrium constant of HF. d. Calculate the pH of the solution. e. Calculate the pKa of the solution. f. Calculate the pOH of the solution.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
Consider the following statements. Write out an example reaction and K expression that is associated with each statement. a. The autoionization of water. b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion. c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion.
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
1. The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. a. Write the chemical equation for the ionization of this acid in water. b. Write the Ka expression for this acid. c. What is the equilibrium concentration of each product and the reactant?
A 0.200M solution of a weak acid, HX, is 9.40% ionized. a. Write the equation for dissociation for this acid. Be sure to include water as one of the reactants. b. Write the Ka expression for HX. c. What are the equilibrium concentrations of the reactants and products? d. What is the value of Ka for this acid? e. What is the pH of HX?
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10.0 g of NaHCO3 is dissolved in a mixture of 1750 mL water and 250 mL of 0.20 M NaOH. a. Calculate the pH of the solution. Answer: b. 250 mL of 0.10 M HCl is added to the solution. Calculate the change in pH (ApH) of the solution.
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1. Give the equation for the dissociation of dimethylamine, (CH3)2NH, in water. b. Write the Kb expression for dimethylamine. c. What are the equilibrium concentrations of all species in a 0.750M solution of dimethylamine? Kb = 5.92 x 10-4 d. What is the pH, pOH and [H+] of this solution? e. What is the % ionization of this solution?
A solution is a mixture of 0.100M weak acid and 0.020M of its conjugate base. The pH of the resulting solution is 5.20. What is the pKa of the weak acid? a. 7.00 b. 4.50 c. 5.90 d. 4.74 e. 8.24