The pH of an aqueous solution of 0.237 M ammonium chloride,NH4Cl(aq), is(Assume thatK₁ (NH3) = 1.80 × 10-5.)This solution isSubmit Answer↑Retry Entire Group2 more group attempts remaining

We have to calculate the pH of ammonium chloride solution

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The pH of an aqueous solution of 0.237 M ammonium chloride, NH4Cl(aq), is (Assume that Kb (NH3) = 1.80 × 10-5.) This solution is

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

The pH of an aqueous solution of 0.237 M ammonium chloride,
NH4Cl(aq), is
(Assume that
K₁ (NH3) = 1.80 × 10-5.)
This solution is
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