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QveST [7]
3 years ago
15

What is the pH of a buffer solution when the concentrations of both buffer components (the weak acid and its conjugate base) are

equal? What happens to the pH when the buffer contains more of the weak acid than the conjugate base? More of the conjugate base than the weak acid?
Chemistry
1 answer:
Ksivusya [100]3 years ago
8 0

Explanation:

Considering the Henderson- Hasselbalch equation for the calculation of the pH of the buffer solution as:

pH=pKa+log[base]/[acid]

When the the concentrations of both buffer components (the weak acid and its conjugate base) are equal:

[base] = [acid]

So, pH=pKa+log1 = pKa

<u>pH is equal to pKa of weak acid of buffer system .</u>

When buffer contains more of weak acid than conjugate base:

[base] < [acid]

log [base]/[acid] = Negative,

So,

<u>When more of acid component is present, the pH is more acidic. (It decreases)</u>

When buffer contains more of conjugate base than weak acid:

[base] > [acid]

log [base]/[acid] = Positive,

So,

<u>When more of acid component is present, the pH is more acidic. (It increases)</u>

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4 0
3 years ago
Suppose now that you wanted to determine the density of a small crystal to confirm that it is boron. From the literature, you kn
Phantasy [73]

Answer:

the volume of  CHCI3 = 7.87 ml

the volume of  CHBr3 = 12.13 ml

Explanation:

From the given information:

We all know that 1 g/cm^3 = 1 g/ml

The density of boron = 2.34 g/ml

The Volume of the liquid mixture  = 20 ml

Recall that:

Density = mass/volume

Mass = Density × Volume

Mass = 2.34 g/ml × 20 ml

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Suppose the volume of  CHCI3 be Y and the Volume of CHBr3 be 20 - Y

Then :

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Y = -11/ - 1.398

Y = 7.87 ml

Therefore, the volume of CHCI3  7.87 ml

the volume of  CHBr3 = 20 - Y

= 20 - 7.87

= 12.13 ml

3 0
3 years ago
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