Use the References to access important values if needed for this question.Design a buffer that has a pH of 10.03 using one of the weak base/conjugate acid systems shown below.C5H5NWeak Base Kb Conjugate AcidCH3NH24.2×10-4CH3NH3+C6H1503N 5.9x10-7 C6H1503NH+1.5x10-9Kapka2.4x10-1110.62CsH5NH*1.7x10-86.7x10-67.775.17How many grams of the bromide salt of the conjugate acid must be combined with how many grams of theweak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams bromide salt of conjugate acid =grams weak base =Submit Answer

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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 16.89QE

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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.
Select from Table 15.1 a conjugate acid-base pair that is suitable for preparing a buffer solution whose concentration of hydronium ions is (a) 4.5 103 M. (b) 5.2 108 M. (c) 8.3 106M. (d) 9.7 1011 M. Explain your choices.
Determine the dominant acid-base equilibrium that results when each of the following pairs of solutions is mixed. Indicate the equilibrium by writing 1 for a strong acid, 3 for a weak acid, 4 for an acidic buffer, 7 for a neutral solution, 10 for a basic buffer, 11 for a weak base, and 13 for a strong base. (a) 10.0 mL of 0.15 M NaOH + 15.0 mL of 0.10 M HNO3 (b) 25.0 mL of 0.10 M HCl + 10.0 mL of 0.25 M NH3 (c) 50.0 mL of 0.050 M NaOH + 50.0 mL of 0.10 M NH3 (d) 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.05 M HCl
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Use the data in Table 15.1 to select a conjugate acid-base pair you could use to make buffer solutions having each of these hydrogen ion concentrations. 3.2 × 10−4 M 5.0 × 10−5 M 7.0 × 10−8 M 6.0 × 10−11 M
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0
Consider a solution formed by mixing 100.0 mL of 0.10 M HA (Ka = 1.0 106), 100.00 mL of 0.10 M NaA. and 100.0 mL of 0.10 M HCl. In calculating the pH for the final solution, you would make some assumptions about the order in which various reactions occur to simplify the calculations. State these assumptions. Does it matter whether the reactions actually occur in the assumed order? Explain.
Which of these combinations is the best to buffer the pH at approximately 9? Explain your choice. CH3COOH/NaCH3COO HCl/NaCl NH3/NH4Cl
Select from Table 15.1 a conjugate acid-base pair that is suitable for preparing a buffer solution whose concentration (molarity) of hydronium ions is (a) 3.55 104. (b) 3.31 106. (c) 4.79 109. (d) 7.08 1011. Explain your choices.
A buffer solution is prepared by adding 0.125 mol ammonium chloride to 500. mL of 0.500-M aqueous ammonia. Calculate the pH of the buffer. If 0.0100 mol HCl gas is bubbled into 500. mL buffer and all of the gas dissolves, calculate the new pH of the solution.

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