1.The hydroxide ion concentration of an aqueous solution of 0.497 M benzoic acid

Question

1.The hydroxide ion concentration of an aqueous solution of 0.497 M benzoic acid, C6H5COOH is [OH-] = _____M?

2.The hydronium ion concentration of an aqueous solution of 0.59 M nitrous acid is [H3O+] =_____M?

3.The pH of an aqueous solution of 0.513 M hydrofluoric acid is____?

4.Calculate the pH of a 0.587 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4)

5.Calculate the pH of a 0.0353 M aqueous solution of hydrofluoric acid (HF, Ka = 7.2×10-4).

6.Calculate the pH of a 0.0709 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

7.The hydronium ion concentration of an aqueous solution of 0.445 M ethylamine (a weak base with the formula C2H5NH2) is [H3O+] =_____M

8.The hydroxide ion concentration, [OH-], of an aqueous solution of 0.445 M triethylamine (a weak base with the formula (C2H5)3N) is___M   

9.The pH of an aqueous solution of 0.445 M aniline (a weak base with the formula C6H5NH2) is ____M

Explanation / Answer

Ka = 6.3x10^-5 = [C6H5COO-][H+] / [C6H5COOH]
6.3x10-5 = x2 / 0.497 - x
x = [H+] = 0.005564M
pH = -log(0.005564M) = 2.254

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