What is the molarity of an aqueous phosphoric acid solution if 10.33 mL is compl

Question

What is the molarity of an aqueous phosphoric acid solution if 10.33 mL is completely neutralized by 17.24 mL of 0.1301 M NaOH? Write a balanced molecular equation for the reaction. Be sure to include the appropriate phases for all reagents and products. What is the molarity of an aqueous phosphoric acid solution if 10.33 mL is completely neutralized by 17.24 mL of 0.1301 M NaOH? Write a balanced molecular equation for the reaction. Be sure to include the appropriate phases for all reagents and products.

Explanation / Answer

The balanced reaction is given as:

H3PO4 (aq) + 3NaOH (aq) = Na3PO4 (aq) + 3H2O (l)

using the formula , M1 V1 / n1 = M2 V2 / n2

where M is molarity , V is volume and n is the stoichiometric coffecients .

So putting all the values we get :

(M1 x 10.33) / 1 = ( 0.1301 x 17.24) / 3

M1 = 0.0724 M

So the molarity of acid will be 0.0724 M

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