What volume (in mL) of 0.0992 M NaOH solution is required to reach the endpoint in the complete...

Question:

What volume (in mL) of 0.0992 M {eq}NaOH {/eq} solution is required to reach the endpoint in the complete titration of a 15.0 mL sample of 0.107 M {eq}H_3PO_4 {/eq}?

Equivalence Point:

An acid-base titration experiment seeks to determine the unknown molarity of some acidic/basic analyte reactant. It is titrated with a basic/acidic titrant reactant of known molarity. The reaction continues until you have combined the reactants in stoichiometric quantities. This is the equivalence point of the titration and here there is no limiting reactant. The data here is used to determine the analyte moles, which leads to the analyte molarity. The equivalence point is often referred to as the endpoint, according to the change in color of some indicator chemical at some pH value. The pH value is commonly assumed to be the actual equivalence point pH.

Answer and Explanation: 1

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NaOH is a strong monoprotic base. Phosphoric acid is a weak triprotic acid. The balanced reaction equation is:


{eq}\rm 3NaOH + H_3PO_4 \rightarrow...

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Equivalence Point: Definition & Calculation

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Chapter 12 / Lesson 11
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Learn about equivalence point and end point in titrations. Examine how to find equivalence points in a variety of ways, and discover the steps to do so.


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