Ionic Equilibrium
Q. What is the pH of a 0.1 M solution of sodium bicarbonate (NaHCO3)? (2022) 2022
-
A.
8.00
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B.
9.00
-
C.
7.00
-
D.
6.00
Solution
NaHCO3 is a weak base, pH ≈ 8.00 due to its bicarbonate ion acting as a weak base.
Correct Answer: A — 8.00
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Q. What is the pH of a 0.1 M solution of sulfuric acid (H2SO4)?
Solution
H2SO4 is a strong acid; it dissociates completely, so [H+] = 0.1 M; pH = -log(0.1) = 1.
Correct Answer: B — 2
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Q. What is the pH of a buffer solution made from 0.1 M acetic acid and 0.1 M sodium acetate? (2023)
-
A.
4.74
-
B.
5.00
-
C.
5.74
-
D.
6.00
Solution
Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]) = 4.74 + log(1) = 4.74.
Correct Answer: A — 4.74
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Q. What is the pH of a solution formed by mixing 25 mL of 0.1 M HCl with 25 mL of 0.1 M NaOH? (2020) 2020
Solution
HCl and NaOH neutralize each other, resulting in a neutral solution with pH = 7.
Correct Answer: A — 7
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Q. What is the pH of a solution that is 0.01 M in both HCl and NaOH?
Solution
HCl and NaOH neutralize each other, resulting in a neutral solution with pH = 7.
Correct Answer: C — 7
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Q. What is the pH of a solution when 0.1 M of Na2CO3 is dissolved in water? (2023)
-
A.
10.3
-
B.
11.0
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C.
11.5
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D.
12.0
Solution
Na2CO3 is a salt of a weak acid (H2CO3) and a strong base (NaOH). The pH can be estimated using the hydrolysis of CO3^2- which gives a pH around 11.0.
Correct Answer: B — 11.0
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Q. What is the pH of a solution with 0.01 M of a weak acid with a Ka of 1.0 x 10^-5? (2023) 2023
-
A.
4.00
-
B.
5.00
-
C.
3.00
-
D.
6.00
Solution
Using the formula for weak acids, pH = 0.5(pKa - logC) = 0.5(4.00 - log(0.01)) = 5.00.
Correct Answer: B — 5.00
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Q. What is the pH of a solution with [H+] = 0.00001 M?
Solution
pH = -log(0.00001) = 5.
Correct Answer: B — 6
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Q. What is the pH of a solution with [H+] = 1 x 10^-7 M? (2023)
Solution
pH = -log[H+] = -log(1 x 10^-7) = 7.
Correct Answer: A — 7
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