Chapter 9: Q35P (page 209)

A buffer was prepared by dissolving 0.100 mole of the weak acid $H A (K_{a} = 1.00 \times 10^{- 5})$ plus 0.050 mole of its conjugate base ${Na}^{+} A^{-}$ in 1.00 L. Find the pH

Short Answer

Expert verified

The solution of $pH = 4.70$

Step by step solution

Define buffer:

A buffer is a solution that can withstand pH changes when adding acid or basic nutrients . $pH = {pK}_{a} + \log_{10} \frac{[A^{-}]}{[HA]}$

Find pHa:

$Find {pK}_{a} pH = {pK}_{a} + \log ([A^{-}]) / [HA] {pK}_{a} = - \log (K_{a}) = - \log (1 \times 10^{- 5}) = 5.00 Substitute above value in pH pH = {pK}_{a} + \log ([A^{-}]) / [HA] pH = 5.00 + \log (0.05 / 0.1) The solution is pH = 4.70$

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A buffer was prepared by dissolving 0.100 mole of the weak acid $H A (K_{a} = 1.00 \times 10^{- 5})$ plus 0.050 mole of its conjugate base ${Na}^{+} A^{-}$ in 1.00 L. Find the pH

Short Answer

Step by step solution

Define buffer:

Find pHa:

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A buffer was prepared by dissolving 0.100 mole of the weak acid HA(Ka=1.00×10-5)plus 0.050 mole of its conjugate baseNa+A-in 1.00 L. Find the pH

Short Answer

Step by step solution

Define buffer:

Find pHa:

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Making Measurements

Inorganic Chemistry

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Nuclear Chemistry

Chemical Analysis

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Study anywhere. Anytime. Across all devices.

A buffer was prepared by dissolving 0.100 mole of the weak acid $H A (K_{a} = 1.00 \times 10^{- 5})$ plus 0.050 mole of its conjugate base ${Na}^{+} A^{-}$ in 1.00 L. Find the pH