Be sure to answer all parts.A buffer consists of 0.17 M KHCO3 and 0.65 M K2CO3. Carbonic acid is a diprotic acid withKa1 = 4.5 × 107 and Ka2 = 4.7 × 10-11.(a) Which Ka value is more important to this buffer?ОKal is more important.Ka2 is more important.(b) What is the buffer pH?

Answered: Image /qna-images/answer/9a825bac-4eb4-4084-b0ac-c8f4746d708e.jpg

Answered: Be sure to answer all parts. A buffer…

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...

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2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.
You have 150 mL of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric acid is needed to prepare buffer with pH=9.5?
What ratio of NaCN to HCN is needed to prepare a pH 10.10 buffer? (Ka of HCN is 4.9 × 1010)
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
How many grams of sodium formate, HCOONa, are required to mix with 1.50 Liters of 0.500 M formic acid, HCOOH, in order to prepare a buffer solution with a pH that equals 4.00? pKa(HCOOH) = 3.74 and MM(HCOONa) = 52.01 g/mol
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
Three buffers are prepared with equal concentrations of formic acid and sodium formate (Buffer 1), hydrofluoric acid and sodium fluoride (Buffer 2), and acetic acid and sodium acetate (Buffer 3). Rank the three buffers from highest to lowest pH at which they can buffer a solution (i.e., their buffering pH).(a) 1, 2, 3(b) 3, 2, 1(c) 2, 1, 3(d) 3, 1, 2
2
A chemist creates 0.375 L of a 0.18 M acetic acid (CH3COOH) and 0.29 M sodium acetate (CH3COONa) buffer. Note that the Ka of acetic acid is 1.8 x 10-5. (a) Write the chemical equation for how the buffer responds to the addition of HBr. (b) What is the final pH if 0.0060 mol of HBr are added to the buffer solution?
Be sure to answer all parts. A buffer consists of 0.30 M KHCO3 and 0.69 M K₂CO3. Carbonic acid is a diprotic acid with Kal-4.5 x 107 and K₁2 = 4.7 x 10-¹1. (a) Which K, value is more important to this buffer? Kat is more important. OK₁2 is more important. (b) What is the buffer pH?

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Be sure to answer all parts. A buffer consists of 0.17 M KHCO3 and 0.65 M K2CO3. Carbonic acid is a diprotic acid with Ka1 = 4.5 × 107 and Ka2 = 4.7 × 10-11. (a) Which Ka value is more important to this buffer? О Kal is more important. Ka2 is more important. (b) What is the buffer pH?