Question

What is the pH of a solution of 1.111L of 1.33M HF, ka= 7.2 x 10^-4, and 1.49 moles of NaF?

Answer 1

Question #65482, Chemistry / Inorganic Chemistry

What is the pH of a solution of 1.111 L of 1.33M HF, Ka= 7.2 x 10⁻⁴, and 1.49 moles of NaF?

Answer:

According to Henderson–Hasselbalch equation:

$$pH = pK_a + \log \frac{[A]}{[HA]}$$ $$[HA] = [HF] = 1.33 \, \text{M}$$ $$[A] = [NaF] = \frac{1.49 \, \text{moles}}{1.111 \, \text{L}} = 1.34 \, \text{M}$$ $$pK_a = -\log K_a$$ $$pH = -\log 7.2 \times 10^{-4} + \log \frac{1.34 \, \text{M}}{1.33 \, \text{M}} = 3.14 + 0 = \mathbf{3.14}$$

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