3. Consider the titration Ba(OH)2 (aq) + 2 HNO3 (aq)→ Ba(NO3)2 (aq) + 2 H2O (1).The equivalence point is reached when 18.91 mL of 0.200 M HNO3 is titrated into 25.00 mL of the Ba(OH)2 solution. Calculate the molarity of the Ba(OH)2 solution. Be sure to account for the stoichiometry of the reaction.
3. Consider the titration Ba(OH)2 (aq) + 2 HNO3 (aq)→ Ba(NO3)2 (aq) + 2 H2O (1).The equivalence point is reached when 18.91 mL of 0.200 M HNO3 is titrated into 25.00 mL of the Ba(OH)2 solution. Calculate the molarity of the Ba(OH)2 solution. Be sure to account for the stoichiometry of the reaction.
Question
Transcribed Image Text:3. Consider the titration Ba(OH)2 (aq) + 2 HNO3 (aq)→ Ba(NO3)2 (aq) + 2 H2O (1).The
equivalence point is reached when 18.91 mL of 0.200 M HNO3 is titrated into 25.00 mL
of the Ba(OH)2 solution. Calculate the molarity of the Ba(OH)2 solution. Be sure to
account for the stoichiometry of the reaction.
4. In a titration of KOH solution, 0.0742 g of KHP is weighed into a flask and dissolved in
deionized water. The equivalence point of the titration is reached when 7.05 mL of KOH
solution is added to the KHP solution.
a) How many moles of KHP are in the solution?
b) How many moles of KOH will have to be titrated to neutralize the KHP?
c) What is the molarity of the KOH solution?
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