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Pie
3 years ago
5

Be sure to answer all parts. Calculate the pH of the following two buffer solutions: (a) 1.4 M CH3COONa/1.6 M CH3COOH. (b) 0.1 M

CH3COONa/0.2 M CH3COOH.
Which is the more effective buffer? A. 1.4 M CH3COONa/1.6 M CH3COOH B. 0.1 M CH3COONa/0.2 M CH3COOH
Chemistry
1 answer:
aalyn [17]3 years ago
3 0

Answer:

a) pH = 4.68 (more effective)

b) pH =4.44.

Explanation:

The pH of buffer solution is obtained by Henderson Hassalbalch's equation.

The equation is:

pH =pKa +log\frac{[salt]}{[acid]}

a) pKa of acetic acid = 4.74

[salt] = [CH₃COONa] = 1.4 M

[acid] = [CH₃COOH] = 1.6 M

pH = 4.74 + log \frac{1.4}{1.6}= 4.68

This is more effective as there is very less difference in the concentration of salt and acid.

b) pKa of acetic acid = 4.74

[salt] = [CH₃COONa] = 0.1 M

[acid] = [CH₃COOH] = 0.2 M

pH = 4.74 + log \frac{0.1}{0.2}= 4.44

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15 grams of sodium reacts with a certain amount of chlorine to yield 37 grams of sodium chloride, as shown below.
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The density of ammonia gas under certain conditions is 0.625 g/l. calculate its density in g/cm3.
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3 years ago
How many grams of CH4 will be in a 500ml contain at STP?
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Mass of CH₄ = ?

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500 mL (500 mL× 1L/1000 mL= 0.5 L)

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