16. The pH of a solution of hydrochloric acid is 2.80. What is the molarity of t

Question

16. The pH of a solution of hydrochloric acid is 2.80. What is the molarity of the acid? A. 6.3 X10-3 M 4.2 X10-3 M 1.6X10-3 M 6.3 X10-2 M 4.2 X 10-2 M 17.The pH of a solution is 4.80. What is the concentration of hydroxide ions in this solution? 4.2 X 109 M 1.6 X 105 M 3.6 X 1012 M 6.3 X 10-10 M 2.0 X 10-8 M A. 18.The pH of a 0.100 M solution of a weak acid, HA, is 3.50. Calculate Ka for the acid 1.0 X 106 2.5 X 104 3.6X105 8.2 X104 7.5 X 10-5 A. 19 Refer to the previous question. Calculate the percent ionization of the acid in the 0.100 M solution of HA with pH 3.50 A. 0.016% 0.078% 0.32% 0.68% 1.6% E. Calculate the value of [H30] in a 0.0100 M HBrQ solution A. 20. 5.0 X 10-6 M 5.0 X 10-5 M 2.5 X 10-7 M 2.5 X 1011 M 5.0 X 10-7 M E. 21.What is the pH of a 0.0100 M HBrQ solution? 3.50 4.70 5.30 5.70 6.30 A. 22.What is the value of [OH] in a 0.0100 M HBrQ solution? 2.0 X109 M 2.0 X 10-8 M A.

Explanation / Answer

16)

we have below equation to be used:

pH = -log [H+]

2.8 = -log [H+]

log [H+] = -2.8

[H+] = 10^(-2.8)

[H+] = 1.6*10^-3 M

[HCl] = [H+] = 1.6*10^-3 M

Answer: C

17)

we have below equation to be used:

pH = -log [H+]

4.8 = -log [H+]

log [H+] = -4.8

[H+] = 10^(-4.8)

[H+] = 1.585*10^-5 M

we have below equation to be used:

[OH-] = Kw/[H+]

Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC

[OH-] = (1.0*10^-14)/[H+]

[OH-] = (1.0*10^-14)/(1.585*10^-5)

[OH-] = 6.3*10^-10 M

Answer: D

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