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qaws [65]
3 years ago
12

Which of the following has the best buffering capacity. (Buffering capacity can be thought of as the amount of strong acid or ba

se that must be added to a buffered solution to change its pH by 1)? Select one: a. 0.4 M CH3COONa/ 0.2 M CH3COOH b. None of these are appropriate concentrations for buffers c. they all have the same buffering capacity d. 0.4 M CH3COONa/ 0.6 M CH3COOH Correct e. 0.3 M CH3COONa/ 0.6 M CH3COOH
Chemistry
1 answer:
OleMash [197]3 years ago
7 0

Answer:

The buffer d has the best buffering capacity.

Explanation:

It is possible to obtain the pH of a buffer using Henderson-Hasselbalch formula:

pH = pka + log₁₀ [A⁻]/[HA]

For CH₃COOH/CH₃COONa buffer:

pH = 4,8 + log₁₀ [CH₃COONa]/[CH₃COOH]

a. pH of this buffer is:

pH = 4,8 + log₁₀ [0,4]/[0,2]

pH = 5,1

As buffering capacity can be thought of as the amount of strong acid that must be added to a buffered solution to change its pH by 1:

For a pH of 4,1:

4,1 = 4,8 + log₁₀ [0,4-x]/[0,2+x]

Where x are the moles of strong acid added.

0,200 = [0,4-x]/[0,2+x]

0,0400 + 0,2x = 0,4 - x

<em>x = 0,3 mol</em>

d. pH of this buffer is:

pH = 4,8 + log₁₀ [0,4]/[0,6]

pH = 4,62

For a pH of 3,62:

3,62 = 4,8 + log₁₀ [0,4-x]/[0,6+x]

Where x are the moles of strong acid added.

0,066 = [0,4-x]/[0,6+x]

0,0396 + 0,066x = 0,4 - x

<em>x = 0,338 mol</em>

e. pH of this buffer is:

pH = 4,8 + log₁₀ [0,3]/[0,6]

pH = 4,5

For a pH of 3,5:

3,5 = 4,8 + log₁₀ [0,3-x]/[0,6+x]

Where x are the moles of strong acid added.

0,050 = [0,3-x]/[0,6+x]

0,030 + 0,05x = 0,3 - x

<em>x = 0,257 mol</em>

Thus, <em>buffer d needs more strong acid to change its pH. That means that have the best buffering capacity</em>

You can do the same process using strong base (Increasing pH in 1) and you will obtain the same results!

I hope it helps!

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Answer:

0.147 mol

Explanation:

Step 1: Calculate the volumetric concentration (Cv)

We will use the following expression.

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We will use the following expression.

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M = 180 g / 98.08 g/mol × 0.100 L = 18.4 M

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3 years ago
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Answer:

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Explanation:

Hello.

In this case, since the acid is monoprotic and the KOH has one hydroxyl ion only, we can see that at the equivalence point the moles of both of them are the same:

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Thus, since we are given 1.70 g of the acid, we compute the moles of acid that were titrated:

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Calculate the molarity of a solution made by dissolving 4.0 g of calcium bromide, CaBr2, in enough water to give 200 mL of solut
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A race car travels on a circular track at an average rate of 125 mi/h. The radius of the track is 0.320 miles. What is the centr
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<h3><u>Answer;</u></h3>

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