1. An acid-base titration is performed in which 26.05 mL of 0.1000M H₂SO4 solution was needed to reach the endpoint of a 25mL NaOH solution with unknown concentration. The chemical reaction involved in this titration is as follows: H₂SO4 (a) + 2NaOH(aq) → H₂O + Na2SO4 (0) Calculate for the molarity of the NaOH solution. 2. Suppose a titration needed 27.15 mL of 0.2497M HCl solution to completely react 25.00mL of Ba(OH)2 solution of unknown concentration. Identify and balance the chemical equation involved, then calculate for the concentration of the Ba(OH)2 solution.
1. An acid-base titration is performed in which 26.05 mL of 0.1000M H₂SO4 solution was needed to reach the endpoint of a 25mL NaOH solution with unknown concentration. The chemical reaction involved in this titration is as follows: H₂SO4 (a) + 2NaOH(aq) → H₂O + Na2SO4 (0) Calculate for the molarity of the NaOH solution. 2. Suppose a titration needed 27.15 mL of 0.2497M HCl solution to completely react 25.00mL of Ba(OH)2 solution of unknown concentration. Identify and balance the chemical equation involved, then calculate for the concentration of the Ba(OH)2 solution.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter15: Equilibria Of Other Reaction Classes
Section: Chapter Questions
Problem 11E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...
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