What is the pH of a 6.85 × 10−3 M weak acid solution, HA, if Ka = 4.5 × 10−6?
Group of answer choices
1.2
4.8
9.1
3.8
6.5
What is the pOH of 4.50 × 10−4M HBr?
Group of answer choices
10.7
6.7
1.7
12.3
3.3
What is the pH of a 9.67 × 10−3M solution of NaOH?
Group of answer choices
13.0
4.6
12.0
9.4
2.0
A 6.5 × 10-2 M solution of a weak acid, HA, has a pH of 3.25. What is the Kb for the conjugate of this weak acid?
Group of answer choices
3.7 × 10-5
2.1 × 10-9
2.7 × 10-10
4.9 × 10-6
1.2 × 10-12
Calculate the equilibrium concentration of the [H+] in a 7.2 × 10-3 M solution of HA that has a Ka of 5.45 × 10-8.
Group of answer choices
3.92 × 10-7
7.35 × 10-3
8.49 × 10-2
2.0 × 10-5
6.30 × 10-8
What is the pH of a 9.25 × 10-2 M solution of NaF, a weakly basic salt?
Group of answer choices
11.89
5.93
8.07
9.82
4.18
Calculate the pH of 5.34 × 10-8 M citric acid, H3C6H5O7.
Group of answer choices
4.27
5.20
3.01
6.84
9.73
I'm very sorry to say that according to the HOMEWORKLIB RULES we are allowed to solve only first question. Please co-operate. Thankyou.
1.
Option 4 (3.8) is the correct answer.
a) A solution contains 0.34 M of a weak acid HA (Ka = 2.0 x 10-7) and 0.17 M NaA. What is the pH after 0.05 M of HCl is added to this solution (assume no volume change) b) The pH of a solution containing 0.1 M of a weak acid HA is 6. Calculate Ka for this acid. Note the acids are unrelated for the two problem parts.
What is the pH of a 0.030 M solution of weak acid HA for which Ka = 6.6 x 10-5?
1) A 0.224 M solution of a weak acid (HA) is made. The Ka for this acid is 7.73 ⋅ 10-5 . -What is the pH of this solution? -What is the pOH of this solution? 2)A 0.238 M solution of a weak base (B:) is made. The Kb for this acid is 7.34⋅10-3. -What is the pOH of this solution? -What is the pH of this solution?
The weak acid HA has a Ka of 1.80×10−5. If a 1.9 M solution of the acid is prepared, what is the pH of the solution?
What is the pH of a 0.44 M solution of a weak acid HA, with a Ka of 3.19×10−12? The equilibrium expression is: HA(aq)+H2O(l)⇌H3O+(aq)+A−(aq)
A 0.013 M solution of a weak acid (HA) has a pH of 4.38. What is the K, of the acid? Ka = 10 (Enter your answer in scientific notation.)
A) the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 1.2×10−3 is 1.89. Find the percent dissociation of this solution. B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.13. Find the percent dissociation of this solution.
The weak acid HA has a Ka of 4.5×10−6. If a 1.4 M solution of the acid is prepared, what is the pH of the solution? The equilibrium expression is: HA(aq)+H2O(l)⇋H3O+(aq)+A−(aq)
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+(aq) + A'(aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, Ka? Answer in scientific notation. Answer: A...
Calculate the Ka of a weak monoprotic acid (HA) if the pH of a 1.0 M solution is 2.3. Ka = ___