7. a vinegar solution of unknown concentration was prepared by diluting 10.00 ml of vinegar to a total volume of 50.00 ml with deionized water. a 25.00-ml sample of the diluted vinegar solution required 20.24 ml of 0.1073 m naoh to reach the equivalence point in the titration. calculate the concentration of acetic acid (in m) in the original vinegar solution (i.e., before dilution).

10.00 mL of 0.4344 M vinegar solution is diluted to 50.00 mL. Then, 25.00 mL required 20.24 mL of 0.1073 M NaOH to reach the equivalence point.

What is titration?

Titration is the slow addition of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization, which is often indicated by a color change. In a broad sense, titration is a technique to determine the concentration of an unknown solution.

Step 1: Write the balanced neutralization equation.

NaOH + CH₃COOH = NaCH₃COO + H₂O

Step 2: Calculate the concentration of acetic acid that reacted with NaOH.

20.24 mL (Vb) of 0.1073 M (Cb) NaOH react with 25.00 mL (Va) of acetic acid of unknown concentration (Ca). We can calculate the concentration of the acid using the following expression.

Ca × Va = Cb × Vb

Ca = Cb × Vb / Va

Ca = 0.1073 M × 20.24 mL / 25.00 mL = 0.08687 M

Step 3: Calculate the initial concentration of acetic acid.

10.00 mL (V1) of acetic acid of unknown concentration (C1) is diluted to 50.00 mL (V2) of 0.08687 M (C2) acetic acid. We can calculate the initial concentration using the dilution rule.

C1 × V1 = C2 × V2

C1 = C2 × V2 / V1

C1 = 0.08687 M × 50.00 mL / 10.00 mL = 0.4344 M

10.00 mL of 0.4344 M vinegar solution is diluted to 50.00 mL. Then, 25.00 mL required 20.24 mL of 0.1073 M NaOH to reach the equivalence point.

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