Determine the pH of a solution is 0.15M HClO_2 (K_a = 1.1 times 10^-2 M) and 0.1

Question

Determine the pH of a solution is 0.15M HClO_2 (K_a = 1.1 times 10^-2 M) and 0.15 M HClO (K_a = 2.9 times 10^-8 M). 1.39 4.18 3.55 9.82 12.55 Determine the pH of a solution formed by mixing 25.0 mL of 0.44 M HF and 25.0 mL of 0.44 M NaOH at 25 degree C. The K_a of HF is 3.5 times 10^-5 M. 5.10 11.44 10.20 8.90 2.56 A solution contains 0.012 M in Al^3+ and 0.24 M in NaF. K_f for AlF_6^3- is 7 times 10^19 M^-6 What is [Al^3+] when the system acheives equilibrium? 1.3 times 10^-17 M 7.6 times 10^-18 M 3.1 times 10^-22 M 1.9 times 10^-21 M Calculate Delta S_rxn degree for the following reaction. The S degree for each species is shown below the reaction. C_2H_2(g) + 2H_2(g) rightarrow C_2H_6(g) S degree (J/mol middot K) 200.9 130.7 229.2 -303.3 J/K -229.2 J/K -233.1 J/K +560.8 J/K +102.4 J/K

Explanation / Answer

11. A

On equilibrium
HClO2 + H2O<<<>>>ClO2- + H3O+

H3O+=H+

Ka1 = [H+] [ClO2-] / [HClO2]

1.1 e-2 = [X] [X] / [0.15 -X]

1.1 e-2 [0.15 -X]= [X] [X]

1.65 e-3 -1.1 e-2 X= X2

X2 + 1.1 e-2 X- 1.65 e-3 = 0

x = 0.03549=[H+]

pH=-log[H+]= 1.39

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