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denis23 [38]
3 years ago
9

An aqueous solution of calcium hydroxide is standardized by titration with a 0.112 M solution of hydrobromic acid. If 15.2 mL of

base are required to neutralize 12.4 mL of the acid, what is the molarity of the calcium hydroxide solution?
Chemistry
1 answer:
TiliK225 [7]3 years ago
7 0

Answer:

0.0457 M

Explanation:

The reaction that takes place is:

  • 2HBr + Ca(OH)₂ → CaBr₂ + 2H₂O

First we<u> calculate how many moles of acid reacted</u>, using the <em>HBr solution's concentration and volume</em>:

  • Molarity = Moles / Volume
  • Molarity * Volume = Moles
  • 0.112 M * 12.4 mL = 1.389 mmol HBr

Now we <u>convert HBr moles to Ca(OH)₂ moles</u>, using the stoichiometric ratio:

  • 1.389 mmol HBr * \frac{1mmolCa(OH)_{2}}{2mmolHBr} = 0.6944 mmol Ca(OH)₂

Finally we <u>calculate the molarity of the Ca(OH)₂ solution</u>, using the <em>given volume and calculated moles</em>:

  • 0.6944 mmol Ca(OH)₂ / 15.2 mL = 0.0457 M
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