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aleksandrvk [35]
3 years ago
10

Problem PageQuestion A chemistry student weighs out of acetic acid into a volumetric flask and dilutes to the mark with distille

d water. He plans to titrate the acid with solution. Calculate the volume of solution the student will need to add to reach the equivalence point. Round your answer to significant digits.
Chemistry
1 answer:
zalisa [80]3 years ago
3 0

Answer:

7.92 mL

Explanation:

There is some info missing. I think this is the original question.

<em>A chemistry student weighs out 0.0617g of acetic acid (HCH₃CO₂) into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1300 M NaOH solution. </em>

<em> Calculate the volume of solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits.</em>

<em />

First, we will calculate the moles of acetic acid (MW 60.05 g/mol).

0.0617 g × (1 mol/60.05 g) = 1.03 × 10⁻³ mol

Let's consider the neutralization reaction between HCH₃CO₂ and NaOH.

HCH₃CO₂ + NaOH ⇄ NaCH₃CO₂ + H₂O

The molar ratio of HCH₃CO₂ to NaOH is 1:1. The moles of NaOH are 1.03 × 10⁻³ moles.

The volume of 0.1300 M NaOH that contains 1.03 × 10⁻³ mol is:

1.03 × 10⁻³ mol × 1000 mL/0.1300 mol = 7.92 mL

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