Question

g 10.00 mL of phosphoric acid (H3PO4) are titrated with 0.1000 M sodium hydroxide. 15.00 mL of the sodium hydroxide solution are used in this experiment. Determine the molarity of phosphoric acid.

Answer 1

Answer: The molarity of phosphoric acid is 0.05 M

Step-by-step explanation:

A neutralization reaction is defined as the reaction in which an acid reacts with a base to form a salt and water molecule.

At equivalence, moles of acid becomes equal to the moles of base. The equation for the neutralization follows:

`n_1M_1V_1=n_2M_2V_2` ........(1)

where,

`n_1, M_1\text{ and }V_1` are the n-factor, molarity and volume of acid that is
`H_3PO_4`

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

Given values:

`n_1=3\\M_1=?M\\V_1=10.00mL\\n_2=1\\M_2=0.1000M\\V_2=15.00mL`

Plugging values in equation 1:

`3* M_1* 10.00=1* 0.1000* 15.00\\\\M_1=(1* 0.1000* 15.00)/(3* 10.00)\\\\M_1=0.05M`

Hence, the molarity of phosphoric acid is 0.05 M