17.28 A buffer contains 0.15 mol of propionic acid (C2H;COOH) and 0.10 mol of sodium propionate (C2H5COONA)in 1.20L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NAOH? (c) What is the pH of the buffer after the addition of 0.01 mol of HI?

17.28 A buffer contains 0.15 mol of propionic acid (C2H;COOH) and 0.10 mol of sodium propionate (C2H5COONA)in 1.20L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NAOH? (c) What is the pH of the buffer after the addition of 0.01 mol of HI?

Name: 17.28 17.28 A buffer contains 0.15 mol of propionic acid (C2H;COOH)and
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Description: 17.28 17.28 A buffer contains 0.15 mol of propionic acid (C2H;COOH)and 0.10 mol of sodium propionate (C2H5COONA)in 1.20L.(a) What is the pH of this buffer? (b) What is the pH of thebuffer after the addition of 0.01 mol of NAOH? (c) What isthe pH of t

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
The following diagram represents a buffer composed ofequal concentrations of a weak acid, HA, and its conjugatebase, A-. The heights of the columns are proportionalto the concentrations of the components of the buffer.(a) Which of the three drawings, (1), (2), or (3), representsthe buffer after the addition of a strong acid? (b) Which ofthe three represents the buffer after the addition of a strongbase? (c) Which of the three represents a situation thatcannot arise from the addition of either an acid or a base?
A buffer is prepared by adding 10.0 g of ammonium chloride(NH4Cl) to 250 mL of 1.00 M NH3 solution. (a) Whatis the pH of this buffer? (b) Write the complete ionic equationfor the reaction that occurs when a few drops of nitricacid are added to the buffer. (c) Write the complete ionicequation for the reaction that occurs when a few drops ofpotassium hydroxide solution are added to the buffer.
The pH of a buffer solution containing 0.35 M acetic acid and 0.39 M sodium acetate where the pKa of acetic acid is 4.75 is_________________
A titration experiment is set up where 41.84 mL of 0.4334 M ethylamine, C2H5NH2, is titrated using 1.3218 M HNO3 (the HNO3 is placed in the burette). What should be the pH of the titration reaction after 37.54 mL of HNO3 is added?
How many moles of sodium hydroxide would have to be added to 150 mL of a 0.479 M hypochlorous acid solution, in order to prepare a buffer with a pH of 7.210? ____ moles
What is the pH of a buffer made from 0.580 mol of CH₃NH₂ (Kb = 4.4 × 10⁻⁴) and 0.120 mol of CH₃NH₃I?
Acid Base Equilibria: TitrationWhat is the pH of the buffer 0.10 M Na2HPO4/0.15 M KH2PO4?
A. What is the pH of a buffer prepared by adding 0.607 molof the weak acid HA to 0.406 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10-7 B. What is the pHafter 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. C. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0g disodium hydrogen phosphate, Na2HPO4, in a 500 mL of solution. What is the pH of thebuffer?
How many grams of sodium acetate must be added to 2.00L of 0.105M acetic acid to make a buffer that has a pH of 4.90? (Ignore volume changes due to the addition of the NaC2H3O2).
A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is the pKa of the solution would it be considered a buffer

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