Astudent titrated a 25.00-ml sample of a solution containing an unknown weak, diprotic acid (h2a) with n2oh. if the titration required 17.73 ml of 0.1036 m n2oh to completely neutralize the acid, calculate the concentration (in m) of the weak acid in the sample.
(a) 9.184 x 10 m
(b) 3.674 x 10-2 m
(c) 7.304 x 10-2 m
(d) 7.347 x 10-2 m
(e) 1.469 x 101 m

The concentration of weak acid is

Explanation:

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

where,

are the n-factor, molarity and volume of acid which is

are the n-factor, molarity and volume of base which is NaOH.

We are given:

Putting values in above equation, we get:

Hence, the concentration of weak acid is

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