# If 37.8 mL of a 0.160 M KOH solution is required to titrate 28.5 mL of a H_2SO_4 solution, what...

## Question:

If 37.8 mL of a 0.160 M {eq}KOH {/eq} solution is required to titrate 28.5 mL of a {eq}H_2SO_4 {/eq} solution, what is the molarity of the {eq}H_2SO_4 {/eq} solution?

{eq}H_2SO_4(aq)+2KOH(aq)\to 2H_2O(l)+K_2SO_4(aq) {/eq}

## Equivalence Point:

The equivalence point is an important point in an acid-base titration experiment, in which the unknown acid/base analyte reactant is neutralized (fully consumed) by the standardized base/acid titrant reactant. This means that the starting molar quantities of the two reactants at this point exactly match the stoichiometry of the balanced acid-base reaction equation. Based on this property you can use the reaction stoichiometry together with the moles of the titrant reactant, to find the moles of the analyte reactant.

## Answer and Explanation: 1

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This is a 2:1 molar ratio acid-base titration reaction between KOH (strong monoprotic base) and sulfuric acid (strong diprotic acid):

{eq}2KOH +...

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Chapter 12 / Lesson 11Learn 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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