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AnnZ [28]
2 years ago
5

A 0.187 M weak acid solution has a pH of 3.99. Find Ka for the acid. Express your answer using two significant figures.

Chemistry
1 answer:
Anna35 [415]2 years ago
3 0

Answer:

5.56 × 10⁻⁸

Explanation:

Step 1: Given data

  • Concentration of the weak acid (Ca): 0.187 M
  • pH of the solution: 3.99

Step 2: Calculate the concentration of H⁺

We will use the following expression.

pH = -log [H⁺]

[H⁺] = antilog -pH = antilog -3.99 = 1.02 × 10⁻⁴ M

Step 3: Calculate the acid dissociation constant (Ka)

We will use the following expression.

Ka = \frac{[H^{+}]^{2} }{Ca} = \frac{(1.02 \times 10^{-4})^{2} }{0.187} = 5.56 \times 10^{-8}

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