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Sedbober [7]
3 years ago
14

7. A student titrated a 15.00-mL sample of a solution containing a weak, monoprotic acid with NaOH. The titration required 17.73

mL of 0.1036 M NaOH to reach the equivalence point. Calculate the concentration (in M) of the weak acid in the sample.
Chemistry
1 answer:
stellarik [79]3 years ago
4 0

Answer:  The concentration of the weak acid in the sample is 0.1224 M

Explanation:

The balanced chemical reaction is :

HA+NaOH\rightarrow NaA+H_2O

To calculate the volume 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 HA

n_2,M_2\text{ and }V_2 are the n-factor, molarity and volume of base which is NaOH.

We are given:

n_1=1\\M_1=?\\V_1=15.00mL\\n_2=1\\M_2=0.1036M\\V_2=17.73mL

Putting values in above equation, we get:

1\times M_1\times 15.00=1\times 0.1036\times 17.73\\\\M_1=0.1224

Thus the concentration (in M) of the weak acid in the sample is 0.1224

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