Answered: 245. What is the final pH of a 1.0 L…

245. What is the final pH of a 1.0 L solution containing 0.25 M HF, 0.75 M NaF, and 0.10 moles of KOH? Ka of HF is 7.1 x 10-4 a. 2.8 b. 3.9 c. 3.4 d. 2.3 e. 4.3

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 102CWP: Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 ...

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

245. What is the final pH of a 1.0 L solution containing 0.25 M HF, 0.75 M NaF, and 0.10 moles of
KOH? Ka of HF is 7.1 x 10-4
a. 2.8 b. 3.9 c. 3.4 d. 2.3 e. 4.3

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Consider the following acids and bases: HCO2H Ka = 1.8 104 HOBr Ka = 2.0 109 (C2H5)2NH Kb = 1.3 103 HONH2 Kb = 1.1 108 Choose substances from the following list that would be the best choice to prepare a pH = 9.0 buffer solution. a. HCO2H b. HOBr c. KHCO2 d. HONH3NO3 e. (C2H5)2NH f. (C2H5)2NH2Cl g. HONH2 h. NaOBr
3. A stock buffer solution is made by mixing 1 L of 0.5 M HF and 1 L of 0.5 M NaF. You take a 400 mL aliquot of this solution and add 300 mL of 0.1 M NaOH. What is the final pH? The K₂ of HF is 6.3 × 10-4. a. 2.9 b. 3.8 c. 3.2 d. 4.2 e. 3.5
Please don't provide handwritten solution ....
What is the pH of the solution when 20.0 mL of 0.155 M of NH3(aq) is titrated with 15.0 mL of 0.225 M of HCl(aq)? The Kb of NH3 is 1.8 x 10-5. a. 9.58 b. 6.07 c. 7.23 d. 2.10
4. The Ka of acetic acid is 1.8 x 10 -5. Calculate the pH of a solution which is composed of 0.250 M HCH 3CO 2 and 0.250 M NaCH 3CO 2. a. 1.8 x 10-5 b. 7.20 c. 0.60 d. 0.25 e. 4.74
If the Ka of a weak acid is 4.89 x 10-4, then what would the pH of a buffer system be if equal amounts with equal concentrations of the anion and acid forms were mixed together? A. 3.31 B. 7.62 C. 10.7 D. Not enough information has been given to solve this problem.
7. 25 mL of 0.10 M H₂SO4 is titrated with 20 mL of 0.50 M NaOH. What is the final pH? A. 5.02 B. 7.01 C. 11.12 D. 13.05
14. What is the pH of a solution of 50.0 mL of 0.200 M KOH titrated with 20.0 mL of 0.050 M HCI? a. 11.95 b. 2.05 C. 0.89 d. 13.11
68) A 25.0-mL sample of 0.150 M HN3 is titrated with a 0.150 M NaOH solution. What is the pH after 13.3 mL of base is added? The Ka of HN3 acid is 1.9 × 10-5. A. 4.45 B.1.34 C.3.03 D.4.78 E.4.66
Which values represents the most basic solution, highest pH? A. [H3O+] = 1 x 10-1⁰ B. [OH-] = 1.4 x 10-4 C. pOH = 6.7 D. pH = 4.2
17. What is the pH of the solution produced when 50 mL of 0.25 M HCl is added to 250.0 mL of 0.1 M ammonia? [Given pKa of NH4 is 9.245] a. 4.755 b. 8.944 C. 9.245 d. 9.546
6. Consider a solution that has 0.00500 M HCl and 0.100 M HF. Ka of HF = 7.2x10-4. a. What is the pH of this solution? b. Suppose the solution was like that in A but also had 0.1 M HOI. (i.e. total solution was a mix of 0.00500 M HCl, 0.100 M HF, and 0.1 M HOI). Ka of HOI = 2.0x10-¹¹. Does this solution have an appreciably different pH than the solution in part a? Support your answer with relevant calculations. HINT: Work from strongest acid to the weakest acid.