Consider a 0.50 M solution of HCIO (Ka = 0.011) a.) Calculate the ideal solution

Question

Consider a 0.50 M solution of HCIO (Ka = 0.011) a.) Calculate the ideal solution pH using methods learned in General Chemistry. b.) Write the equilibrium constant expression for this system in terms of activities and then in terms of the concentrations and the mean ionic activity coefficient. For the un-dissociatcd HCIO, assume lambda = 1. c.) Compute, using a recursion method and the DHLL, the non-ideal pH of this solution and compute the % error of the ideal result. d.) Repeat your calculations, this time in a solution of 0.20 M CaCh.

Explanation / Answer

Ka = [H3O+][ClO-]/[HClO] = 0.011 ------- Eq. 1

Now, ICE Table

HClO

H3O+

According to the definition of pH,

x=[H3O+]

pH=log x

Using Eq. 1,

Ka = x2/ 0.5-x

Solving for x simply by qudratic equation, we get x=0.0688

therefore, pH= 1.1624

(B) Equilibrium constnt, Kc = [H3O+][ClO-]/[HClO][H2O]

s activity coeff is 1, so the expression for K is also same as Kc.

(C)

ICE

HClO

H3O+

ClO Initial Concentration 0.5 M 0 M 0 M Change in Concentration -x M +x M +x M Equilibrium Concentration (0. - x) M x M x M

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