A 1 liter solution contains 0.441 M hypochlorous acid and 0.331 M sodium hypochlorite. Addition of 0.364 moles of nitric acid will: (Assume that the volume does not change upon the addition of nitric acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity Submit Submit and Next

A 1 liter solution contains 0.441 M hypochlorous acid and 0.331 M sodium hypochlorite. Addition of 0.364 moles of nitric acid will: (Assume that the volume does not change upon the addition of nitric acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity Submit Submit and Next

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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What is a buffer?
Please don't provide handwritten solution .... What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places.
A 1 liter solution contains 0.427 M hydrofluoric acid and 0.569 M sodium fluoride.Addition of 0.213 moles of potassium hydroxide will:(Assume that the volume does not change upon the addition of potassium hydroxide.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
A 1 liter solution contains 0.567 M acetic acid and 0.425 M potassium acetate.Addition of 0.213 moles of nitric acid will:(Assume that the volume does not change upon the addition of nitric acid.) Raise the pH slightly Lower the pH slightly Raise the pH by several units Lower the pH by several units Not change the pH Exceed the buffer capacity
An aqueous solution contains 0.28 M hydrofluoric acid. One Liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) (Select all that apply.) 0.14 mol HBr0.28 mol NaI0.29 mol NaF0.14 mol KOH0.29 mol HBr An aqueous solution contains 0.28 M ammonia. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) 0.29 mol NH4ClO4 0.14 mol HBr 0.29 mol HBr 0.14 mol Ca(OH)2 0.28 mol Ba(ClO4)2
If you are given sodium acetate and asked to make a 250 mM acetate buffer and titrate it to a final pH of 4.76, will you have to add acid, base, or nothing in order to achieve the proper pH? Why? Please explain the “why” part of the question. Please type answer note write by hend.
Which type of titration will be the pH be acidic at the equivalence point? a) strong acid vs strong base b) strong acid vs weak base c) weak acid vs strong base d) weak acid vs weak base e) none of these
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11. What effect will addition of excess of HCI have on the pH of a solution of NH3? a. increase the pH b. decrease the pH C. no effect d. cannot tell from information given > Answer and brief explanation: 12. A buffer solution may be a mixture of a. a weak acid and its salt b. a weak base and its salt C. an excess of a weak acid with a strong base d. all of the above > Answer and brief explanation: 13. The ammonium ion would be classified as a Bronsted a. acid b. base > Answer and brief explanation:
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 +…
An aqueous solution contains 0.26 M ammonium iodide. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) (Select all that apply.) 0.25 mol NH3 0.26 mol HNO3 0.12 mol HNO3 0.25 mol Nal 0.06 mol Ca(OH)2
A1 liter solution contains 0.395 M hypochlorous acid and 0.526 M potassium hypochlorite. Addition of 0.434 moles of calcium hydroxide will: (Assume that the volume does not change upon the addition of calcium hydroxide.) O Raise the pH slightly Lower the pH slightly |Raise the pH by several units | Lower the pH by several units O Not change the pH Exceed the buffer capacity