CH3COOH dissociates as:
CH3COOH -----> H+ + CH3COO-
1*10^-2 0 0
1*10^-2-x x x
Ka = [H+][CH3COO-]/[CH3COOH]
Ka = x*x/(c-x)
Assuming x can be ignored as compared to c
So, above expression becomes
Ka = x*x/(c)
so, x = sqrt (Ka*c)
x = sqrt ((1.8*10^-5)*1*10^-2) = 4.243*10^-4
since x is comparable c, our assumption is not correct
we need to solve this using Quadratic equation
Ka = x*x/(c-x)
1.8*10^-5 = x^2/(1*10^-2-x)
1.8*10^-7 - 1.8*10^-5 *x = x^2
x^2 + 1.8*10^-5 *x-1.8*10^-7 = 0
This is quadratic equation (ax^2+bx+c=0)
a = 1
b = 1.8*10^-5
c = -1.8*10^-7
Roots can be found by
x = {-b + sqrt(b^2-4*a*c)}/2a
x = {-b - sqrt(b^2-4*a*c)}/2a
b^2-4*a*c = 7.203*10^-7
roots are :
x = 4.154*10^-4 and x = -4.334*10^-4
since x can't be negative, the possible value of x is
x = 4.15*10^-4
So, [H+] = x = 4.15*10^-4 M
use:
pH = -log [H+]
= -log (4.15*10^-4)
= 3.37
Answer: 3.37
29. What is the pH of a 0,010 M solution of acetic acid? K, for acetic...
What is the pH of a solution that is 0.785 M in acetic acid and 0.451 M is sodium acetate. The Ka for acetic acid is 1.8 x 10-5 . A. 4.74 B. 4.50 C. 4.74 D. 4.98 E. 5.50
What is the pH of a solution prepared by mixing: 0.30 moles of acetic acid (Ka = 1.8 X 10-5) 0.15 moles of sodium hydroxide in 1.0 L of solution A. 4.44 B. 13.18 C. none of the above D. 0.82 E. 4.74
(C))3.75 moo (D) 4.75 (E) 5.75 bios nA oir 9. Ka of acetic acid is 1.8 x 10. What is the pH of a solution 0.1M acetic acid and 0.05M sodium acetate? (A) 4.44 oasd A (B) 4.74 (C) 4.96 (D) 5.04 (E) 5.56 10. A buffer solution containing 0.5M acetic acid and 0.5M sodium acetate hais a pH ot 4.745. 5ml 2M sodium hydroxide is added to 995ml of the buffer solution. What is final pH? (A) 4.569 (C))3.75...
QUESTION 14 What is the pH of a solution that is 0.1 Min acetic acid, HC2H302, and 0.3 Min sodium acetate, NaC2H302, at 25°C? Ko of acetic acid is 1.8 x 10-5 25.23 1.53 Oc 4.74 d. 2.29 6.08
e) 8.67 1. IM in What is 0.3 M in 25°c ? acetic acid, HC2H302 3 the pH of a solution that sodium acetate.. Na C 2 H 3 Oz at Ka of acetic acid is 1.8 x 10-5 a) 5.23 b) 1.53 c) 4.74 d) 2.29 e) 6.08
What is the pH of a 0.150 M solution of acetic acid, which has an acid dissociation constant of 1.8 E-5? A. 5.57 B. -5.57 C. 7.35 D. 9.18 E. 2.78
pH of solution of acetic acid (K, - 1.8 10-5) is 3. What is concentration of the acid? 0.018 M 0.056 M 0.006 M O 1.8 M
What is the pH of a 0.067 M solution of acetic acid, whose K-5 = 1.8 x 10? 0 Respond with the correct number of significant figures in scientific notation (Use Enotation and only 1 digit before decimal e.g. 2.5e5 for 2.5 x 10") Type your response
A buffer containing acetic acid and sodium acetate has a pH of 5.55. The K, value for CH3CO,H is 1.80 x 10. What is the ratio of the concentration of CH3CO H to CH3CO,t? [CH,CO,H1 CH2C0, 1 = Calculate the pH of a solution that has an ammonium chloride concentration of 0.054 M and an ammonia concentration of 0.053 M. Kb = 1.8 x 10-5 pH = What is the pH of 0.35 M acetic acid to 1.00 L of...
1) What is the pH of a 0.085 M solution of acetic acid, HC2H3O2? At 25 degrees C, the Ka of acetic acid is 1.8 x 10^-5. 2) 17.4 mL of 4.0 M HCl are diluted with water to make 1.5 L of solution. What should be the pH of the final solution?