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Citrus2011 [14]
3 years ago
15

QUESTION 51 Buffer capacity is best defined as: OA) Buffer capacity is the amount of acid or base that can be added to a buffer

without destroying its effectivene OB) Buffer capacity is the amount of acid that can be added until all of the base is used up O C) Buffer capacity is the amount of base that can be added until all of the acid is used up OD) Buffer capacity is the amount of acid that can be added until all of the acid is used up O E) Butter capacity is the amount of base that can be added until all of the base is used up QUESTION 52 Which of the following acids (listed with Ka values) and their conjugate base would form a buffer with a pH of 2 94? A)HC7H502. Ka = 65 x 10-5 OB) HF ka 9.9 10-4 OC) HCIO. Ka = 2.9 * 10-8 DHCN. K = 49 10-10 E) HCIO2. K - 41 10-2 Click Save and Submit to save and submit. Click Save AT Answers to see all ans .
Chemistry
1 answer:
Schach [20]3 years ago
4 0

Answer:

The best definition is: "Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness"

Explanation:

A buffer is a solution that is somewhat resist to pH changes by reacting with acids and bases that may be added into the solution. It's capacity is the amounto of acid or base that can be added into solution without much change in pH.

So the best definition is: "Buffer capacity is the amount of acid or base that can be added to a buffer without destroying its effectiveness"

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The stronger acid is HBrO3.

Explanation:

It has an additional oxygen making it more electronegative, in turn making it a stronger acid.

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3. Determine the pH of each of the following solutions. (Hint: See Sample Problem B.) a. 1.0 x 10-2 M HCI c. 1.0 x 10-MHI b. 1.0
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Answer:

a. pH = 2 b. pH = 3 c. pH = 1 d. Unanswerable

Explanation:

pH = -log[H+] OR pH = -log{H3O+]

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pOH = -log[OH-]

1. Determine what substance you are working with, (acid/base)

2. Determine whether or not that acid or base is strong or weak.

a. 1.0 x 10^-2M HCl

HCl is a strong acid, therefore it will dissociate completely into H+ and Cl- with all ions going to the H+, therefore, the concentration of HCl and concentration of H+ are going to be equal, meaning we simply take the negative logarithm of the concentration of HCl and that would equal pH

pH = -log[H+]

pH = -log(1.0x10^-2)

pH = 2

b. 1.0 x 10^-3M HNO3

HNO3 like part a, is a strong acid, therefore it would simply require you to take the negative logarithm of the concentration of the compound itself, to find its pH.

pH = -log[H+]

pH = -log(1.0 x 10^-3)

pH = 3

c. 1.0 x 10^-1M HI

Like the previous parts, HI is a strong acid

pH = -log[H+]

pH = -log(0.10)

pH = 1

d. HB isn't an element, nor is it a compound so that would be unanswerable.

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