3. Suppose you had titrated your vinegar sample with barium hydroxide instead of sodium hydroxide: Ba(OH)2(aq)+2CH3COOH(aq)⟶Ba(C

Question

3. Suppose you had titrated your vinegar sample with barium hydroxide instead of sodium hydroxide:

Ba(OH)2(aq)+2CH3COOH(aq)⟶Ba(CH3COO)2(aq)+2H2O(l)

Consider a 0.586 M aqueous solution of barium hydroxide,

What volume (in mL) of 0.586 M Ba(OH)2 solution are required to neutralize 10 ml of vinegar containing 2.78 g of acetic acid?

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Ngọc Hoa 3 years 2021-08-08T11:20:05+00:00 1 Answers 106 views 0

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  1. kimchi2
    0
    2021-08-08T11:21:50+00:00
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    Answer:

    39.6 mL

    Explanation:

    Step 1: Write the balanced neutralization reaction

    Ba(OH)₂(aq) + 2 CH₃COOH(aq) ⟶ Ba(CH₃COO)₂(aq) + 2 H₂O(l)

    Step 2: Calculate the moles corresponding to 2.78 g of CH₃COOH

    The molar mass of CH₃COOH is 60.05 g/mol.

    2.78 g × 1 mol/60.05 g = 0.0463 mol

    Step 3: Calculate the moles of Ba(OH)₂ needed to react with 0.0463 moles of CH₃COOH

    The molar ratio of Ba(OH)₂ to CH₃COOH is 1:2. The moles of Ba(OH)₂ needed are 1/2 × 0.0463 mol = 0.0232 mol.

    Step 4: Calculate the volume of 0.586 M solution that contains 0.0232 moles of Ba(OH)₂

    0.0232 mol × 1 L/0.586 mol = 0.0396 L = 39.6 mL

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )