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Suppose you are titrating vinegar, which is an acetic acid solution, of unknown strength with sodium hydroxide according to the equation HC2H3O2 + NaOH → H2O + NaC2H3O2 If you require 32.17 mL of 0.116 M NaOH solution to titrate 10.0 mL of HC2H3O2 solution, what is the concentration of acetic acid in the vinegar? (M)

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Answer:

0.373 M

Explanation:

The reaction is

  • HC₂H₃O₂ + NaOH → H₂O + NaC₂H₃O₂

So 1 mol of acetic acid reacts with 1 mol of sodium hydroxide.

First we calculate the moles of NaOH:

  • 0.116 M * 32.17 mL = 3.732 mmol NaOH

Because the stoichiometric ratio is 1:1 :

  • 3.732 mmol NaOH = 3.732 mmol Acetic Acid

Now we calculate the concentration of acetic acid, dividing the moles by the volume:

  • 3.732 mmol Acetic Acid / 10.0 mL = 0.373 M
dsdrajlin

32.17 mL of 0.116 M NaOH are required to titrate 10.0 mL of 0.373 M acetic acid.

What is titration?

Titration is a common laboratory method of quantitative chemical analysis to determine the concentration of an identified analyte.

Let's consider the neutralization reaction between acetic acid and sodium hydroxide.

HC₂H₃O₂ + NaOH → H₂O + NaC₂H₃O₂

We can calculate the concentration of acetic acid in vinegar using the following expression.

Ca × Va = Cb × Vb

Ca = Cb × Vb / Va

Ca = 0.116 M × 32.17 mL / 10.0 mL = 0.373 M

where,

  • Ca is the concentration of the acid.
  • Va is the volume of the acid.
  • Cb is the concentration of the base.
  • Vb is the volume of the base.

32.17 mL of 0.116 M NaOH are required to titrate 10.0 mL of 0.373 M acetic acid.

Learn more about titration here: https://brainly.com/question/13031875

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