A buffer is made by adding 0.300 mol CH3COOH (acetic acid) and 0.300 mol CH3COONa (sodium acetate) to enough water to make 1.00 L of solution. Calculate the pH after 0.020 mol of NaOH is added to this buffer. (You may again ignore change in volume as a result of the addition.) Reference data: pK₂ of acetic acid is 4.74 (A) 4.74 (B) 4.68 (C) 4.80 (D) 3.60 (E) 12.0

A buffer is made by adding 0.300 mol CH3COOH (acetic acid) and 0.300 mol CH3COONa (sodium acetate) to enough water to make 1.00 L of solution. Calculate the pH after 0.020 mol of NaOH is added to this buffer. (You may again ignore change in volume as a result of the addition.) Reference data: pK₂ of acetic acid is 4.74 (A) 4.74 (B) 4.68 (C) 4.80 (D) 3.60 (E) 12.0

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

An analytical chemist Is titrating 248.1 mL of a 0.3600M solution of diethylamine ((C,H,) NH) with a 0.5000M solution of HNO,. The p K, of diethylamine 3' is 2.89. Calculate the pH of the base solution after the chemist has added 191.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. 3. Round your answer to 2 decimal places. do PH = Ar Explanation Check 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility i 3:20 Chp ぐう esc ( backs & # $ 8. 9. 4 1
An analytical chemist is titrating 173.3 mL of a 0.1600M solution of diethylamine ((C₂H)2NH) with a 0.05100M solution of HCIO4. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 602.7 mL of the HCIO solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HCIO solution added. Round your answer to 2 decimal places.
An analytical chemist is titrating 75.2 mL of a 0.5800 M solution of trimethylamine ((CH3)N) with a 0.2600M solution of HNO3. The p K₂ of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 197.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X 5 4
A compound has an ionisable groups with a pKa of 2.6. A 200 mL volume of a 0.15 M solution of this compound had an initial pH 2.4. The concentration of the conjugate acid in the initial buffer was 0.092 M. The concentration of the conjugate base in the initial buffer was 0.058 M. What is the final pH of the buffer AFTER you added 5 mL of 1 M NaOH?
To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should be measured (HCO3-+CO2), this was determined by acidifying the sample and measuring the volume of CO2 released. The concentration of H2CO3 was 28.5 mmol/L, the pH of the blood at 37 ℃ is 7.48 with a pka of 6.10, what is the concentration of HCO3- in mmol/L in the blood? a) 27.36b) 22.77c) 28.50d) 29.60
Given that the Ka for acetic acid is 1.8 x 10-5. What is the pH of a buffer solution made from 0.20 M sodium acetate and 0.10 M acetic acid?
An analytical chemist is titrating 199.8 mL of a 0.1100M solution of trimethylamine ((CH3), N) with a 0.2200 M solution of HNO3. The pK, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 61.2 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 X S 图 dh
If the pKA of R-COOH is 3.73 and the pH of an R-COOH/R-COO– solution is 3.88, which of the following is TRUE? Note: R-COO– is supplied as the neutral R-COONa salt. [R-COOH] = [R-COO–] [R-COOH] > [R-COO–] It is not possible to make a buffer from R-COOH and R-COO– for this particular pH. [R-COOH] >> [R-COO–] [R-COOH] < [R-COO–]
A chemistry graduate student is given 100. mL of a 1.70M diethylamine ((C2H5)2NH): NH solution. Diethylamine is a weak base with K = 1.3 × 10³. What mass of (C₂Hs)2NH2Br should the student dissolve in the (C2H3)2NH solution to turn it into a buffer with pH = 11.12? You may assume that the volume of the solution doesn't change when the (C2H5)2NH2Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10
The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.
A formic acid buffer solution contains 0.18 M HCOOHHCOOH and 0.13 M HCOO−HCOO− . The pKa of formic acid is 3.75. What is the pH of the buffer?