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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?

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Answer:

0.220 M

Explanation:

In the equivalence point, [H⁺] = [OH⁻].

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 compute the given data in the formula to calculate C₂:

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

The concentration of the unknown weak acid solution is 0.220 M

Equivalent point:

Since the volume is 4.00 mL of the weak acid, and it takes  17.6 mL of 0.0500 M NaOH to reach the equivalence point.

We know that

In the equivalence point, [H⁺] = [OH⁻].

here the given formula C₁V₁=C₂V₂ is used

Here

C₁ = 0.0500 M

V₁ = 17.6 mL

C₂ = ?

V₂ = 4.00 mL

So, the C₂ is

0.0500 M * 17.6 mL = C₂ * 4.00 mL

C₂ = 0.220 M

Hence, The concentration of the unknown weak acid solution is 0.220 M

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