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andre [41]
2 years ago
7

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

14.2 mL of 0.0500 M NaOH to reach the equivalence point. What is the concentration of the unknown weak acid solution
Chemistry
1 answer:
timofeeve [1]2 years ago
8 0

Answer:

0.1775 M

Explanation:

The reaction that takes place is:

  • HA + NaOH → NaA + H₂O

Where HA is the unknown weak acid.

At the equivalence point <em>all HA moles are converted by NaOH</em>. First we <em>calculate how many NaOH moles reacted</em>, using the<em> given concentration and volume</em>:

  • 0.0500 M NaOH * 14.2 mL = 0.71 mmol NaOH

That means that in 4.00 mL of the weak acid solution, there were 0.71 weak acid mmoles. With that in mind we can now <u>calculate the concentration</u>:

  • 0.71 mmol HA / 4.00 mL = 0.1775 M
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