3. Consider the titration Ba(OH)2 (aq) + 2 HNO3 (aq)→ Ba(NO3)2 (aq) + 2 H2O (1).Theequivalence point is reached when 18.91 mL of 0.200 M HNO3 is titrated into 25.00 mLof the Ba(OH)2 solution. Calculate the molarity of the Ba(OH)2 solution. Be sure toaccount 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 indeionized water. The equivalence point of the titration is reached when 7.05 mL of KOHsolution 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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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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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