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erastova [34]
4 years ago
12

Suppose you perform a titration of an unknown weak acid solution. You start with 4.00 mL of the weak acid and find that it takes

17.6 mL of 0.0500 M NaOH to reach the equivalence point. What is the concentration of the unknown weak acid solution?
Chemistry
1 answer:
Veseljchak [2.6K]4 years ago
4 0

Answer:

0.220 M

Explanation:

<em>In the equivalence point, [H⁺] = [OH⁻]</em>.

This means we can use the formula C₁V₁=C₂V₂

Where

  • C₁ = 0.0500 M
  • V₁ = 17.6 mL
  • C₂ = ?
  • V₂ = 4.00 mL

So we <u>compute the given data in the formula</u> to calculate C₂:

  • 0.0500 M * 17.6 mL = C₂ * 4.00 mL
  • C₂ = 0.220 M
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