A student carried out a titration using H2SO4 and KOH.  The balanced equation for the reaction is:H2SO4 (aq) + 2 KOH (aq)  -->  K2SO4 (aq)  +  2 H2O (l)The student determined that 0.227 mol KOH were used in the reaction.  How many moles of H2SO4 would have been needed to react with all of this KOH?Enter a numerical value in the correct number of significant figures.  Do not enter units and do not use scientific notation.

Question
Asked Apr 1, 2019

A student carried out a titration using H2SO4 and KOH.  The balanced equation for the reaction is:

H2SO4 (aq) + 2 KOH (aq)  -->  K2SO4 (aq)  +  2 H2O (l)

The student determined that 0.227 mol KOH were used in the reaction.  How many moles of H2SO4 would have been needed to react with all of this KOH?

Enter a numerical value in the correct number of significant figures.  Do not enter units and do not use scientific notation.

check_circleExpert Solution
Step 1

The equation for the neutralization reaction is,

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Step 2

From the equation, 1 mole of H2SO4 required to react with 2 moles of KOH.

 

Therefore ½ moles of H2SO4 required to react with 1 moles of KOH.

Step 3

Number of moles required to react with 0.227...

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