The pH of hydrochloric acid, HCl (aq), with a concentration of 0.15 mol dm-3 is
0.15
0.82
-0.82
1.00
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The pH of hydrochloric acid, HCl (aq), with a concentration of 0.15 mol dm-3 is
0.15
0.82
-0.82
1.00
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What is the pH of a 0.008 mol dm-3 solution of sodium hydroxide, NaOH, at 25 °C?
(Kw = 1.00 x 10-14 mol2 dm-6 at 25 °C)
2.10
11.90
12.90
10.90
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The pH curve represents which type of titration?
Strong alkali being added to weak acid
Strong acid being added to weak alkali
Weak acid being added to strong alkali
Weak acid being added to weak alkali
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Which statement about buffers is correct?
A buffer resists small changes in pH
A buffer can be formed from sodium hydroxide and an excess of ethanoic acid
Buffers are able to resist changes in pH when strong acids and alkalis are added
If a strong acid is added to a buffer solution the concentration of the weak acid decreases
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The correct expression for the acid dissociation constant, Ka, for the dissociation of benzoic acid, C6H5COOH is
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Which of the following statements is correct?
As temperature increases, the pH value of pure water decreases
As temperature decreases, the pH value of pure water decreases
The pH of water is unaffected by temperature
Pure water is not neutral
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Which of the following is the pH of 0.08 mol dm-3 Ba(OH)2?
(Kw = 1.00 x 10-14 mol2 dm-6 at 25 ℃)
14.80
13
13.20
12.90
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What is the pH of ethanoic acid with a concentration of 0.75 mol dm-3 at 25 oC?
(Ka of ethanoic acid at 25 ℃ = 1.78 x 10-5 mol dm-3)
4.62
0.12
9.72
2.44
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The pH range of four different indicators are:
Indicator | pH range for colour change |
Methyl orange | 3.2 - 4.4 |
Phenolphthalein | 8.2 - 10.0 |
Thymol blue | 1.2 - 2.8 |
Bromothymol blue | 6.0 - 7.6 |
Which indicator would be suitable for a titration involving hydrochloric acid and ammonia?
Methyl orange
Phenolphthalein
Thymol blue
Bromothymol blue
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What is the pH of a buffer solution containing 0.0413 moles of ethanoic acid and 0.0398 moles of sodium ethanoate in 500 cm3 at 25 oC?
(Ka of ethanoic acid at 25 ℃ = 1.78 x 10-5 mol dm-3)
1.08
4.73
2.91
4.77
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Which statement is correct for the following equation?
NH4+ + OH– ⇌ H2O + NH3
NH4+ is the base
H2O is the conjugate acid
NH3 is the conjugate acid
OH– is the acid
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25.00 cm3 of 0.25 mol dm−3 nitric acid is added to 12.50 cm3 of 0.10 mol dm−3 sodium hydroxide.
What is the pH of the resulting mixture?
0.88
0.60
2.30
13.00
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A buffer solution is prepared by mixing 200 cm3 of 2.00 mol dm–3 propanoic acid, CH3CH2COOH, with 600 cm3 of 1.00 mol dm–3 sodium propanoate, CH3CH2COONa.
Ka for CH3CH2COOH = 1.32 × 10–5 mol dm–3
What is the pH of the buffer solution?
4.58
4.70
5.06
4.87
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Which of the following statements is/are correct?
1, 2 and 3
Only 1 and 2
Only 2 and 3
Only 1
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X g of potassium ethanoate was added to ethanoic acid to form a buffer solution with a final volume of 250 cm3 and a pH of 4.70. The final concentration of ethanoic acid was 0.40 mol dm-3. Ka for ethanoic acid is 1.8 x 10-5 mol dm-3.
What was the mass of potassium ethanoate added?
68.0 g
5.41 g
41.6 g
8.85 g
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A student has 0.72 mol dm-3 of potassium hydroxide solution, a solution of sodium hydroxide with a pH of 13.4 and a solution of hydrogen cyanide with a pH of 4.20 and a Ka of 6.2 x 10-10 mol dm-3.
Kw = 1.00 x 10-14 mol2 dm-6.
What is the pH of potassium hydroxide, the concentration of sodium hydroxide (mol dm-3) and the concentration of hydrogen cyanide (mol dm-3) respectively?
13.90, 0.60, 6.42
13.80, 0.25, 4.05
13.90, 0.25, 6.42
14.70, 0.60, 4.05
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What is the pH of a buffer solution formed when 2.5 g of NaOH is added to 1.0 dm3 of 0.15 mol dm-3 solution of ethanoic acid? Ka for ethanoic acid is 1.74 x 10-5 mol dm-3.
4.61
4.19
5.96
5.58
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