1). Consider a 0.4 M solution of anilinium chloride. The ion anilinium is the co

Question

1). Consider a 0.4 M solution of   anilinium chloride. The ion   anilinium is the conjugate acid of the the weak base aniline.The pKb   of aniline is 9.13  

Part a).   Calculate  [H+] __________ M

Part b). Calculate the concentration of   anilinium ions. __________ M

Part c). Calculate the concentration of   aniline in equilibrium. _________ M

Part d). Calculate [OH] ________ M

Part e). Calculate [Cl-] ________ M

Part f). Calculate the pH _______ M

2). Calculate the pH and the concentration [Na+] =of all species in   3.5×102   molar sodium cyanide solution.

[Na+] = ___ M

H+] = ___M

pH = ___M

[OH] =___M

[CN] = ___M

[HCN]= ___M

Explanation / Answer

1). Consider a 0.4 M solution of   anilinium chloride. The ion   anilinium is the conjugate acid of the the weak base aniline.The pKb   of aniline is 9.13  

BHCl --> BH+ + Cl-

BH+ ---> B + H+

Ka = [B][H+]/[BH+]

Kw/Kb = x*x/(0.4-x)

(10^-14)/(10^-9.13) = x*x/(0.4-x)

x = 0.002316

[B] = [H+]= x= 0.002316

[BH+] = 0.4-0.002316 = 0.3977

Part a).   Calculate  [H+] __________ M

[H+] = 0.002316

Part b). Calculate the concentration of   anilinium ions. __________ M

[BH+] = 0.4-0.002316 = 0.3977 M

Part c). Calculate the concentration of   aniline in equilibrium. _________ M

[B] = [H+]= x= 0.002316 M

Part d). Calculate [OH] ________ M

[OH-] = (10^-14) / (0.002316) = 4.31*10^-12

Part e). Calculate [Cl-] ________ M

[Cl-] = 0.4 M

Part f). Calculate the pH _______ M

pH = -log(0.002316) = 2.64

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