Chemistry, 21.06.2019 17:00 sillslola816oxb5h7

An aqueous solution of hydroiodic acid is standardized by titration with a 0.186 m solution of calcium hydroxide. if 26.5 ml of base are required to neutralize 20.3 ml of the acid, what is the molarity of the hydroiodic acid solution? m hydroiodic acid

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Answer from: secondweb448

The molarity of hydroiodic acid in the titration is 0.485 M.

Explanation:

To calculate the molarity of acid, we use the equation given by neutralization reaction:

n_1M_1V_1=n_2M_2V_2

where,

$n_1,M_1\text{ and }V_1$ are the n-factor, molarity and volume of acid which is

$n_2,M_2\text{ and }V_2$ are the n-factor, molarity and volume of base which is Ca(OH)_2

We are given:

$n_1=1\\M_1=?M\\V_1=20.3mL\\n_2=2\\M_2=0.186M\\V_2=26.5mL$

Putting values in above equation, we get:

$1\times M_1\times 20.3=2\times 0.186\times 26.5\\\\M_1=0.485M$

Hence, the molarity of hydroiodic acid is 0.485M.

Answer from: Quest

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