Ka = 3.5*10^-6
pKa = - log (Ka)
= - log(3.5*10^-6)
= 5.456
use:
pH = pKa + log {[conjugate base]/[acid]}
= 5.456+ log {6.4*10^-3/4.6*10^-2}
= 4.60
Answer: c
3. What is the pH of a solution that is 0.046 Min HA and also 0.0064...
HA is a weak acid. Its ionization constant, Ka, is 2.4 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.046 M.
(1). The pH of a solution that is 0.2 M in HA and 0.14 M in NaA is ___. Ka = 3.3 x 10-6.
1. Determine the pH of a buffer solution prepared by mixing 25.3mL of 0.35M HA (Ka= 1.6x10-5) with 15.3mL of 0.45M NaA. 2.100 mL of buffer solution that is 0.15M HA (Ka= 6.8x10-5) and 0.20M NaA is mixed with 17.3mL of 0.25M HCl. What is the pH of the resulting solution? 3. Calculate the pH of a solution made by mixing 75.0mL of 0.15M HA (Ka= 2.5x10-5) with 7.5mL of 0.75M NaOH 4. 100 mL of buffer solution that is...
Calculate the pH of each solution. A solution containing 0.0320 M maleic acid and 0.046 M disodium maleate. The Ka values for maleic acid are 1.20 x 10 (Ka1) and 5.37 x 10-7 (Ka2) 1.8 pH A solution containing 0.0306 M succinic acid and 0.019 M potassium hydrogen succinate. The Ka values for succinic acid are 6.21 x 105 (Kal) and 2.31 x 10 (Ka2) pH
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.
A solution contains 0.250 M HA (К.-1.0 added to 1.00 L of this solution? 3. 10" and 0.45 M NaA. what is the pH after 0.30 mole of HC1 is a. 0.52 b. 7.44 c. 5.44 d. 2.10 e. 8.56
1. An acid (HA) has a Ka = 4.7 x 10-6. What is the pH of a solution containing 0.350 M of this acid? a. 3.02 b. 2.94 c. 2.89 d. 0.60 2. For a rate law, the exponents on each concentration term ([A]x, [B]y, etc.) come from the coefficients of the balanced equation. True or False 3. The pH of a 0.025 M aquesous solution of the strong base NaOH is ____. a. 1.60 b. -12.18 c. 12.18 d....
QUESTION 3 What is the pH of a buffer solution composed of HA and A (Ka = 1.38 x 10-4) under these conditions: concentration of HA = 0.62, concentration of A = 0.65
1.A 1.76 M solution of a weak acid HA is found to have a pH of 2.22 Determine Kg of the acid Determine Kb of its conjugate base, A Determine [OH'] in a 2.00 M solution of the weak acid's sodium salt, NaA M Determine the pH of a 2.00 M solution of the sodium salt, NaA 2.The pH of a 1.93 M solution of a weak base B is measured to be 10.82 Determine Kp of the base Determine...
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...