A 1 liter solution contains 0.356 M hydrofluoric acid and 0.474 M potassium fluoride. Addition of 0.178 moles of sodium hydroxide will: (Assume that the volume does not change upon the addition of sodium hydroxide.) (Select all that apply.) Not change the pH Lower the pH by several units Raise the pH slightly Lower the pH slightly Raise the pH by several units Exceed the buffer capacity

A 1 liter solution contains 0.356 M hydrofluoric acid and 0.474 M potassium fluoride. Addition of 0.178 moles of sodium hydroxide will: (Assume that the volume does not change upon the addition of sodium hydroxide.) (Select all that apply.) Not change the pH Lower the pH by several units Raise the pH slightly Lower the pH slightly Raise the pH by several units Exceed the buffer capacity

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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A 1 liter solution contains 0.306 M hydrofluoric acid and 0.408 M potassium fluoride. Addition of 0.337 moles of calcium hydroxide will: (Assume that the volume does not change upon the addition of calcium hydroxide.) (Select all that apply.) ORaise the pH slightly Not change the pH O Lower the pH by several units Lower the pH slightly Raise the pH by several units Exceed the buffer capacity
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Part A Review Constants | Periodic Table Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH, COO). Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base: H++ CH3COO→CH3COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid: OH +…
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