3. Calculate the pH of the following solutions. Hint: some parts should require very little math! a. A 0.010 M solution of an acid that completely dissociates in solution. b. A 0.010 M solution of an acid that's conjugate base has a pKb of 8.2. c. A solution that's comprised of 75% acid and 25% conjugate base with a Ka = 1.4 x 10-4 d. A 0.100 M solution of sodium hydroxide.

3. Calculate the pH of the following solutions. Hint: some parts should require very little math! a. A 0.010 M solution of an acid that completely dissociates in solution. b. A 0.010 M solution of an acid that's conjugate base has a pKb of 8.2. c. A solution that's comprised of 75% acid and 25% conjugate base with a Ka = 1.4 x 10-4 d. A 0.100 M solution of sodium hydroxide.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.80QE: Calculate the pH of each of the following solutions. (a) 10.0 mL of 0.300 M hydrofluoric acid plus...

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Similar questions

Explain why a sample of pure water at 40 C is neutral even though [H3O+]=1.7107M . Kw is 2.91014 at 40 C.
Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
A. What is the Kb when the Ka of a solution is 5.47x10^-4? B. the Ka of an acid is determined to be 0.00589. What is the Pka? C. A solution is made where 0.878 moles HCl is added to water that has a total volume of 1855mL. what is the PH of the solution?
Which of the following is true about acids and bases? A. When bases ionize, they donate protons. B. Strong acids and bases are completely ionized in dilute aqueous solutions. C. The dissociation constant of a strong acid is lower than that for a weak acid. D. The pKa of a strong acid will be higher than that for a weak acid.
10. The K₂ of HONH₂ is 1.1 x 10-8. a. Calculate the pH and percent dissociation of a solution containing 0.100 M HONH2. b. Calculate the pH and percent dissociation of a mixture containing 0.100 M HONH2 and 0.100 M HONH3CI. (Assume complete dissociation of HONH3CI.)
2. The Ka for benzoic acid (HC7H5O2), is 6.5 x 10-5. Calcuklate pH of a 0.10 M benzoic acid solution. 3. Calculate the pH of a 0.24 M solution of weak base A-1 that has a Kb of 2.5 x 10-6. Answer numbers 2 and 3 please.
Which of the following acids has the weakest conjugate base? A. pyruvic acid, Ka = 2.8 x 10-3 B. malonic acid, pka = 2.85 OC ascorbic acid, pka - 4.1. OD. benzoic acid, Ka = 6.31 x 10 O E. 3-chlorobenzoic acid, pKą = 3.8
Given the following Ka values, which one belongs to the strongest acid? The weakest acid?a. 6.2 x 10-8b. 1.8 x 10-5c. 7.5 x 10-3d. 4.9 x 10-10e. 6.8 x 10-4
Determining the value of Ka of acid from initial concentration and pH 8) A 0.185 M solution of a weak acid has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid. Write the equation for the dissociation of an acid and define an expression for Ka Draw an ICE table What other information in the problem above can help you determine the value of x? Use that information to solve for the value of x and substitute back into the ICE table to determine equilibrium concentration of products and reactants Substitute the equilibrium concentration of reactants and products into the Ka expression to determine the value of Ka
1. A. Identify the type of solution and calculate the pH for each of the following: i. 0.100 M HONH2 (Kb = 1.1 x 10-8) ii. 0.100 M HONH3Cl iii. Pure H2O iv. A solution containing 0.100 M HONH2 and 0.100 M HONH3Cl B. Calculate the percent ionization of the base in A.i. Predict the relative percent ionization of the base in A.iv. Explain any expected differences. C. Which of the solutions in A is a buffered solution?