Question

# Use pH, pOH, [H3O+], and [OH–] relationships. (a) The hydroxide ion concentration in an aqueous solution...

Use pH, pOH, [H3O+], and [OH–] relationships. (a) The hydroxide ion concentration in an aqueous solution of HCl is 3.4×10-13 M. Calculate [H3O+], pH, and pOH for this solution.

[H3O+] = 2.9x10^-4 M pH = 1.54 pOH = 12.46

(b) The pOH of an aqueous solution of HNO3 is 9.30. Calculate [H3O+], [OH-], and pH for this solution. [H3O+] = 2x10^-5 M [OH-] = 5x10^-10 M pH = 4.70

There is a error somewhere thank you for your help and can you give step by step aprreciate it

(a) The hydroxide ion concentration in an aqueous solution of HCl is 3.4×10-13 M. Calculate [H3O+], pH, and pOH for this solution.

pOH = -loG(OH) = -log(3.4*10-13) = 12.468; you are correct,

pH= 14-pOH = 14-12.468 = 1.532 you are also correct

[H+] = 10^-pH = 10^-1.532 = 0.029376; 2.9*10^-2 ithink you may be wrong in this one

(b) The pOH of an aqueous solution of HNO3 is 9.30. Calculate [H3O+], [OH-], and pH for this solution.

OH- = 10^-pOH = 10^-9.3 = 5.0118*10^-10, correct

pH = 14-pOH = 14-9.3= 4.7

H+ = 10^-pH = 10^-4.7 = 1.995*10^-5 also correct, since it is approx 2*10^-5

[H3O+] = 2x10^-5 M [OH-] = 5x10^-10 M pH = 4.70

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