An unknown weak acid with a concentration of 0.078 M has a pH of 1.80. What...
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
Question 47 of 52 Submit An unknown weak acid with a concentration of 0.084 M has a pH of 1.80. What is the Ka of the weak acid? 1 2 3 C +/- x 100
Question 22 of 25 Submit An unknown weak acid with a concentration of 0.071 M has a pH of 1.80. What is the Ka of the weak acid?
What is the conjugate acid of the Brønsted-Lowry base, (CH3)3N O of 1 point earned 3 attempts remaining What is the conjugate acid of the Brønsted-Lowry base, CsH5NH2? O of 1 point earned 3 attempts remaining What is the conjugate acid of the Brønsted-Lowry base, HCO3"? O of 1 point earned 3 attempts remaining What is the conjugate acid of the Brønsted-Lowry base, H2PO4" O of 1 point earned 3 attempts remaining What is the conjugate base of the Brønsted-Lowry...
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...
A bery weak acid that is 0.424 M in concentration has a pH of 3.21. What is the Kb of the acid?
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, K ? Answer in scientific...
Determine the pH of each of the following solutions. (a) 0.416 M hypobromous acid (weak acid with Ka = 2.5e-09). pH = ___________ (b) 0.644 M ascorbic acid (weak acid with Ka = 8e-05). pH = ___________ (c) 0.703 M pyridine (weak base with Kb = 1.7e-09). pH = ___________
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?
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?