10. A 0.10 M aqueous solution of a A) 1.0 x 10 B) 1.0 x 104 HA has a pH of 4.00.

Question

10. A 0.10 M aqueous solution of a A) 1.0 x 10 B) 1.0 x 104 HA has a pH of 4.00. What is the value of K. fot HA? ,0 x 107 D) 1.0 × 10.6 E) 1.0 × 108 CO + x CoI-o.coo 11. Which are the Bronsted-Lowry bases in the following equilibrium? D) H:O and OH- E) CH,COO and OH- A) H20 and CH COOH B) CH,COo and CH COOH C) HO, CHsCOOH, and OH- 12. If K 0.133 for A2 +2B 2AB, what is the value of K for the reaction A) 0.133 B) -0.133 56.5 D) 0.266 E) 3.76 13. Which of the following solutions is acidic? A) B) C) [OH1> 1.0 x 107 M [H30')=1.0 x 1010 M [OH] = 1.0 x 107M D) HO 11.0x 107 M E) [OH] 1.0 x 1010 M d at 25°C. What is the acid-ionization 14. A 0.060 M solution of a weak monoprotic acid is 3.0% ionize constant, K, for this acid? A) 1.8% 10-3 B) 9.0×10- C) 5.6×10-s D) 30×10-2 E) 6,0 x 10s 15. Identify the conjugate base of HCOs

Explanation / Answer

10)

use:
pH = -log [H+]
4 = -log [H+]
[H+] = 1*10^-4 M
HA dissociates as:

HA          ----->     H+   + A-
0.1                 0         0
0.1-x               x         x


Ka = [H+][A-]/[HA]
Ka = x*x/(c-x)
Ka = 1*10^-4*1*10^-4/(0.1-1*10^-4)
Ka = 1.001*10^-7
Answer: 1.0*10^-7

11)
Base is the compound which accepts H+
In forward reaction, CH3COO- accepts H+. So, it is a base
In backward reaction, OH- accepts H+. So, it is a base
Answer: E

12)
For:
A2 + 2B <—> 2 AB
Kc1 = [AB]^2 / [A2] [B]^2
= 0.133

so, for:
4 AB   <—> 2 A2 + 4B
Kc2 = [A2]^2 [B]^4 / [AB]^4
= (1/Kc1)^2
= (1/0.133)^2
= 56.5
Answer: 56.5

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