A solution with a pOH of 4.30 has a [H^+] of _____ 6.8 times 10^-9 M. 3.2 times

Question

A solution with a pOH of 4.30 has a [H^+] of _____ 6.8 times 10^-9 M. 3.2 times 10^-4 M. 4.8 times 10^-5 M. 2.0 times 10^-10 M. 4.3 M. A 0.100 M monoprotic weak acid solution has a pH of 3.00. What is the pK_a of this acid? 5.00 0.10 3.00 9.99 6.00 Which of the following is the K_a expression for the conjugate acid of trimethylamine, (CH_3)_3 N? k_a = [(CH_3)_3 NH^+] [OH^-]/[(CH_3)_2 N] K_a = [(CH_3)_3 NH]]H_2 O]/[(CH_3)_3 NH^+] [OH^-] K_a = [(CH_3)_3 NH^+] [OH^-]/[CH_3)_3 NH] [H_2 O] K_a = [(CH_3)_3 N] [H^+]/[(CH_3)_3 NH^+] [H_2 O] K_a = [(CH_3)_3 N] [H^+]/[(cH_3)_3 NH^+] What is the pH of a 0.20 M ammonia solution? (The K_b value for ammonia is 1.8 times 10^-5.) 11.28 9.26 4.74 9.56 2.72 What is the actual concentration of the molecular form of HF in a 1.00 M HF solution given that K_a of HF is 6.8 times 10^-4 ? 2.6 times 10^-2 M 0.97 M 1.59 M 6.8 times 10^-4 M 1.0 M What is the percent dissociation of 0.150 M triethylamine ? (The K_b value for triethylamine is 5.25 times 10^-4 .) 5.92% 5.75 times 10^-3 % 39.4% 5.90 times 10^-3% 5.75% Which one of the following sails forms aqueous solutions with pH = 7? Na_2 S NaBR NaCLO_2 NaNO_2 NaCO_3

Explanation / Answer

45. pH + pOH = 14

pH = 14-pOH

= 14-4.30

= 9.7

pH = -log[H+]

[H+] = antilog(-pH)

= antilog(-9.7)

= 2.0*10-10M

Option d.

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