Problem: A solution contains 1.00 mole of acetic acid and has pH = 2.50. How many grams of NaCH3COO·3H2O (of MW 136) should be dissolved in the solution to raise the pH to 4.00?1. 10 g2. 35 g3. 20 g4. 15 g5. 24 g

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FREE Expert Solution
FREE Expert Solution

The original solution is composed of 0.100 mol acetic acid (CH3COOH). NaCH3COO3H2O will be added to raise the pH to 4.00.

CH3COOH is a weak acid (and based on the Bronsted-Lowry definition, an acid is a proton (H+) donor. Once CH3COOH loses its proton, its conjugate base is formed).

CH3COOH(aq) +  H2O(l)  ⇌    CH3COO-(aq)    +  H3O+(aq)
    (weak acid)            (base)         (conjugate base)    (conjugate acid)

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Problem Details

A solution contains 1.00 mole of acetic acid and has pH = 2.50. How many grams of NaCH3COO·3H2O (of MW 136) should be dissolved in the solution to raise the pH to 4.00?

1. 10 g

2. 35 g

3. 20 g

4. 15 g

5. 24 g

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