29. Answer BOTH parts of this question. Show ALL arithmetical steps and chemical equations. (a) Calculate the pH of a buffer solution composed of 0.15M HF and 0.15M NaF. (Ka for HF is 6.8 x 10-4). (b) Calculate the ApH caused by the addition of 7.0 ml of 0.10M NaOH to 100ml of the buffer solution obtained in part (a) of this question.

29. Answer BOTH parts of this question. Show ALL arithmetical steps and chemical equations. (a) Calculate the pH of a buffer solution composed of 0.15M HF and 0.15M NaF. (Ka for HF is 6.8 x 10-4). (b) Calculate the ApH caused by the addition of 7.0 ml of 0.10M NaOH to 100ml of the buffer solution obtained in part (a) of this question.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

4) What is the pH of a buffer solution, prepared by mixing of 75 mL 0.1 M CH3COOH solution and 150 mL 0.2 M CH3COONA solution. Ka(CH3COOH) = 1.75 · 10-5 mol/L.
Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.
Calculate the pH of 52.0 mL of the buffer solution (0.10 M HC2H3O2 and 0.20 M NaC2H3O2) to which 33.0 mL of 0.10 M hydrochloric acid is added.
Consider the titration of 90.0 mL of .141 M Ba(OH)2 by .564 M HCl. Calculate the pH of the resulting solution after 11.0 mL and 27.0 mL of HCl have been added
25.0 ml of 0.100M NaOH is titrated with HC2H3O2 and 50.0mL of the acid is used to reach the endpoint. a)Write the chemical equation for the reaction. Include states of matter. b)Calculate the molarity of the acid HC2H3O2. c)What is the starting pH for the base in the titration?
#18. The sample of 25.00 mL of 0.020 M NH3 is titrated with 0.016 M HCl. (a) Show the reaction between NH3 and H+. (b) Find the volume of 0.016 M HCl needed to reach the equivalence point. (c)Show the reaction of hydrolysis of product from the step (a). (d) Calculate the pH at the equivalence point(Ka of NH4+ is 5.6 x 10–10)
Calculate the pH of a buffer made up by adding 0.65 mol of NaC2H3O2 (sodium acetate) to 00L of a 0.88 M solution of HC2H3O2 (acetic acid). (assume no volume change, Ka=1.8x10^-5)
An aqueous solution contains 0.329 M methylamine (CH3NH2).How many mL of 0.305 M perchloric acid would have to be added to 225 mL of this solution in order to prepare a buffer with a pH of 10.700.
Calculate the pH at the equivalence point for the titration of 0.140 M methylamine (CH3NH2) with 0.140 M HCl. The ?b of methylamine is 5.0×10−4.
Chemistry A student conducted a titration experiment in a lab. 50.00 mL of nitric acid (HNO3) (0.090 M) is titrated with the following volume of NaOH (0.1 M). 0.00 mL, 15.00 mL, 23.00 mL and 26.00 mL Calculate the pH of each volume titrated. Sketch a titration curve based on the pH calculated in (a). Write the chemical reaction for the reaction of acid and base in this titration. Predict the titration curve if the same concentration of HNO3 is titrated with 0.0920 M ammonia. Compare the graph you sketched in (b) with the graph you predicted in d) with similarities and differences.
A solution contains 0.351 M HA (Ka = 1.13⋅10−51.13⋅10-5) and 0.744 M NaA. What is the pH of this solution? What is the pH of this solution after 0.186 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.372 mol of HCl are added to 1.00 L of this solution?
Use the References to access important values if needed for this question. A buffer solution is made that is 0.379 M in HCN and 0.379 M in NaCN. If Ka for HCN is 4.00 x 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.090 mol HNO3 is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + Submit Answer ->> Retry Entire Group + 9 more group attempts remaining