Q. What is the pH of a 0.1 M solution of sodium bicarbonate (NaHCO3)?
-
A.
7.5
-
B.
8.4
-
C.
9.0
-
D.
6.0
Solution
NaHCO3 is a weak base; its pH is around 8.4.
Correct Answer: B — 8.4
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Q. What is the pH of a 0.1 M solution of sodium bicarbonate (NaHCO3)? (2022) 2022
-
A.
8.00
-
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 containing 0.1 M acetic acid and 0.1 M sodium acetate?
-
A.
4.74
-
B.
5.74
-
C.
6.74
-
D.
7.74
Solution
Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]). Here, pKa ≈ 4.74, so pH = 4.74 + log(1) = 4.74.
Correct Answer: A — 4.74
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Q. What is the pH of a buffer solution containing 0.2 M acetic acid and 0.1 M sodium acetate?
-
A.
4.76
-
B.
5.00
-
C.
5.74
-
D.
6.00
Solution
Using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]) = 4.76 + log(0.1/0.2) = 5.74
Correct Answer: C — 5.74
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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 buffer solution made from 0.2 M acetic acid and 0.2 M sodium acetate?
-
A.
4.76
-
B.
5.76
-
C.
6.76
-
D.
7.76
Solution
Using the Henderson-Hasselbalch equation, pH = pKa + log([A-]/[HA]) = 4.76.
Correct Answer: A — 4.76
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Q. What is the pH of a neutral solution at 25°C?
Solution
At 25°C, the pH of a neutral solution is 7.
Correct Answer: B — 7
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Q. What is the pH of a neutral solution at 25°C? (2023) 2023
Solution
At 25°C, the pH of a neutral solution is 7.
Correct Answer: B — 7
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Q. What is the pH of a neutral solution of hydrogen ions?
Solution
A neutral solution has a pH of 7.
Correct Answer: B — 7
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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 formed by mixing equal volumes of 0.1 M HCl and 0.1 M NaOH?
Solution
HCl and NaOH neutralize each other completely, resulting in a neutral solution with a pH of 7.
Correct Answer: A — 7
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Q. What is the pH of a solution that has a hydrogen ion concentration of 1 x 10^-5 M?
Solution
pH is calculated as pH = -log[H+]. For [H+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.
Correct Answer: A — 5
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Q. What is the pH of a solution that has a hydronium ion concentration of 1 x 10^-5 M?
Solution
pH is calculated as pH = -log[H3O+]. For [H3O+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.
Correct Answer: A — 5
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Q. What is the pH of a solution that has a hydroxide ion concentration of 1.0 x 10^-3 M?
Solution
pOH = -log[OH-] = -log(1.0 x 10^-3) = 3. Therefore, pH = 14 - pOH = 14 - 3 = 11.
Correct Answer: A — 11
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Q. What is the pH of a solution that has a [H+] concentration of 1 x 10^-7 M?
Solution
pH = -log[H+] = -log(1 x 10^-7) = 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 that is 0.1 M in both acetic acid and sodium acetate?
-
A.
4.76
-
B.
5.76
-
C.
6.76
-
D.
7.76
Solution
Using Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]); pKa of acetic acid = 4.76, so pH = 4.76 + log(1) = 4.76
Correct Answer: A — 4.76
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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
-
C.
11.5
-
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 a hydrogen ion concentration of 0.001 M? (2022)
Solution
pH = -log[H+]. pH = -log(0.001) = 3.
Correct Answer: A — 3
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Q. What is the pH of a solution with a hydrogen ion concentration of 1 x 10^-3 M? (2019)
Solution
pH = -log[H+] = -log(1 x 10^-3) = 3.
Correct Answer: B — 3
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Q. What is the pH of a solution with a hydrogen ion concentration of 1 x 10^-7 M?
Solution
pH = -log[H+] = -log(1 x 10^-7) = 7.
Correct Answer: A — 7
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Q. What is the pH of a solution with a hydroxide ion concentration of 0.001 M?
Solution
pOH = -log[OH-] = -log(0.001) = 3; pH = 14 - pOH = 14 - 3 = 11
Correct Answer: B — 12
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Q. What is the pH of a solution with a hydroxide ion concentration of 1.0 x 10^-4 M?
Solution
To find the pH, first calculate pOH = -log[OH-] = 4, then use pH + pOH = 14, so pH = 14 - 4 = 10.
Correct Answer: A — 10
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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^-6 M?
Solution
Using the formula pH = -log[H+], we find pH = -log(1 x 10^-6) = 6.
Correct Answer: A — 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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Q. What is the pH range of acidic solutions? (2023)
-
A.
0-7
-
B.
7-14
-
C.
14-20
-
D.
None of the above
Solution
Acidic solutions have a pH range of 0 to 7.
Correct Answer: A — 0-7
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Q. What is the pH range of normal human urine? (2022)
-
A.
4.5 - 5.5
-
B.
6.0 - 7.0
-
C.
7.5 - 8.0
-
D.
8.5 - 9.0
Solution
Normal human urine typically has a pH range of 6.0 to 7.0, which can vary based on diet and health.
Correct Answer: B — 6.0 - 7.0
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