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17 Nov 2019

Chlorous acid, HClO2, has a dissociation constant of Ka = 1.20 x 10–2 .

Calculate the degree of dissociation for a 0.0766m solution of this acid:

(a) using the Debye–Hückel limiting law

(b) assuming that the mean ionic activity coefficient is one.

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Nestor Rutherford
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6 Sep 2019
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Related questions

Estimate the mean activity coefficient and activity of NaCl in a solution that is a.) 0.020 mol kg!1 NaCl b.) 0.020 mol kg!1 NaCl and 0.035mol kg!1 Ca(NO3)2 . (Use the Debye-Hückel limiting law for each calculation.)

A weak acid has a dissociation constant of Ka = 0.025.

(a) Calculate the degree of dissociation for a 0.094 m solution of this acid using the Debye-Huckel limiting law.

(b) Calculate the degree of dissociation for a 0.094 m solution of this acid that is also 0.200 m KCl from the Debye-Huckel limiting law using an iterative calculation until the answer is constant in the second decimal place.

(c) Repeat the calculation (b) using the value of \(\gamma\pm\) = 0.718 for KCl.

This problem is from the Engel-Reid Physical Chemistry textbook, 3rd edition. Problem 10.5. Chegg does not have solutions for this chapter...

The acid dissociation constant for HClO2 is Ka = 1.1 x 10-2. You add 1.08 g of HClO2 to 427 ml of 0.0150 M NaClO2 solution. What are the equilibrium concentrations of H3O+, ClO2- and HClO2? Also, what is the pH assuming ideal behavior? Take Kw equal to 1.0 x 10-14.

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