A 1 liter solution contains 0.419 M acetic acid and 0.559 M sodium acetate. Addition of 0.461 moles of potassium hydroxide will: (Assume that the volume does not change upon the addition of potassium hydroxide.) (Select all that apply.) Lower the pH slightly Exceed the buffer capacity Not change the pH ORaise the pH by several units Raise the pH slightly Lower the pH by several units

A 1 liter solution contains 0.419 M acetic acid and 0.559 M sodium acetate. Addition of 0.461 moles of potassium hydroxide will: (Assume that the volume does not change upon the addition of potassium hydroxide.) (Select all that apply.) Lower the pH slightly Exceed the buffer capacity Not change the pH ORaise the pH by several units Raise the pH slightly Lower the pH by several units

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 45P

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Similar questions

Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.
. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?