An aqueous solution of hydroiodic acid is standardized by titration with a 0.108 M solution of barium hydroxide.If 21.8 mL of base are required to neutralize 17.8 mL of the acid, what is the molarity of the hydroiodic acid solution?M hydroiodic acid

given :- molarity of Ba(OH)2 solution = 0.108 M volume of Ba(OH)2 solution = 21.8 mL volume of HI…

Answered: An aqueous solution of hydroiodic acid…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter4: Chemical Reactions In Solution

Section: Chapter Questions

Problem 4.91QE

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The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.
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A 10.0-mL sample of potassium iodide solution was analyzed by adding an excess of silver nitrate solution to produce silver iodide crystals, which were filtered from the solution. KI(aq)+AgNO3(aq)KNO3(aq)+AgI(s) If 2.183 g of silver iodide was obtained, what was the molarity of the original KI solution?
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An aqueous solution of hydroiodic acid is standardized by titration with a 0.108 M solution of barium hydroxide. If 21.8 mL of base are required to neutralize 17.8 mL of the acid, what is the molarity of the hydroiodic acid solution?