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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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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