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.

The molarity of phosphoric acid is 0.05 M

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:

             ........(1)

where,

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

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

Given values:

Plugging values in equation 1:

Hence, the molarity of phosphoric acid is 0.05 M

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.