We have 500.0 mL of a buffer solution that is 0.661 M in NH3 and 0.304 M in NH4Cl. We add 500.0 mL of a solution 0.245 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution
We have 500.0 mL of a buffer solution that is 0.661 M in NH3 and 0.304 M in NH4Cl. We add 500.0 mL of a solution 0.245 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution
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
Chapter15: Solutions Of Acids And Bases
Section: Chapter Questions
Problem 15.121QE: A solution is made by diluting 25.0 mL of concentrated HCl (37% by weight; density = 1.19 g/mL) to...
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We have 500.0 mL of a buffer solution that is 0.661 M in NH3 and 0.304 M in NH4Cl. We add 500.0 mL of a solution 0.245 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
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