ACIDS, BASES, SALTS
ACIDS, BASES, SALTS
Total Questions: 70
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1. Salts of weak acid + strong base hydrolyse to give _ solution
Basic
2. According to Brønsted–Lowry, acids lose proton to become...
Conjugate base
3. According to Brønsted–Lowry, base accept proton to become...
Conjugate acid
4. Arrhenius defined acids as substances which dissociate in water to give...
H+ ions
5. The conjugate acid of H2PO4– is _
H3PO4
6. All Amphoteric substances are Amphiprotic.
False
7. According to G.N. Lewis, acids are substances that can...
Accept paired electrons
8. Lewis acid + Lewis base =
Adduct
9. Corrosive action of acids is related to...
Anion of the acid
10. Solutions that can conduct electric current are known as...
Electrolyte
11. One of these dissociates completely in water
HBr
12. Acids react with Bisulphites to liberate which of these gases?
SO2
13. Acids react with carbonates to liberate which of these gases?
CO2
14. Which of these is a yellowish compound, used as a bleaching agent in chemistry?
CaOCl2
15. One of these acids is a strong dehydrating agent
H2SO4
16. The number of hydrogen atoms that can be replaced in an acid is termed...
Basicity
17. One of these is a dibasic acid
H2SO4
18. Ionisation of strong acids in water is an equilibrium reaction
False
19. Ionisation of weak acids in water is an equilibrium reaction
True
20. One of these acids is used to produce ammonium nitrate fertilisers
HNO3
21. One of these acids is used for etching of glass
HF
22. The acid that is present in vinegar is...
Acetic acid
23. _ causes sour taste in milk
Lactic acid
24. The acid found in lime and lemon is...
Citric acid
25. The concentrated form of one of these bases is corrosive
KOH
26. Soaps are produced by saponification reaction between bases and...
Fatty acids
27. One of these bases is a major component in an antacid called Milk of Magnesia
Mg(OH)2
28. Salts are _
Ionic compounds
29. The activity of any pure substance in its standard state tends to...
1
30. _ have the ability to resist pH changes when small amount of strong acids or bases are added to the solution
Buffers
31. What is pH when pOH is 2.90
11.1
32. What is [H+] when pH is 3.84?
0.00014
33. What is the pH of pure water?
7
34. Which of these acids is injected when an ant stings?
Formic acid
35. What is the pH of 0.2 M H2SO4 solution
0.4
36. What is the pH of 0.1 M KOH?
13
37. What is the pOH of 0.004 M HNO3?
11.6
38. Pb(OH)NO3 is a _ salt?
Basic salt
39. The hydrogen ion concentration of a solution is 3.6 × 10–5 M. What is the pOH of the solution?
9.56
40. A 15.00 mL sample of 0.100 M sodium hydroxide required 22.37 mL of hydrochloric acid, HCl, for neutralisation. What is the concentration of HCl?
0.067
41. Which of the following salts forms aqueous solutions with pH = 7?
NaNO3
42. Aqueous solutions of _ are basic
NaF
43. What is the pH of 0.10 M solution of weak acid, given its pKb = 4.13
5.44
44. Phosphoric acid is a _ acid
Triprotic
45. Which of the following is the conjugate acid of the hydrogen phosphate ion, HPO42–?
H2PO4–
46. Which one of the following is not a conjugate acid–base pair?
H3O and OH–
47. The stronger the acid, ...
The weaker its conjugate base
48. Which of the following compounds cannot be a Brønsted–Lowry base?
NH4+
49. Basic salts arise when?
Less than stochiometric amount of acids react with polyhydroxy bases
50. Which of the following is a Monoprotic acid?
CH3COOH
51. At 25°C, the value of kw for pure water is 1.0 × 10–14. What is the value of pKw?
14
52. Arrhenius concept of acids and bases did not recognise one of the following ions.
H3O+
53. A buffer solution contains 0.5 M NH3 and 0.8 M NH4Cl. Calculate the pH of the solution (kb for NH3 = 1.8 × 10–5)
9.06
54. The ka of propionic acid is 1.34 × 10–5. What is the pH of a solution containing 0.50 M propionic acid, and 0.5 M sodium propionate?
4.87
55. The pH of 0.20 M NaOH solution is...
13.3
56. A solution at 25°C contains 0.1 M sodium acetate and 0.03 M acetic acid. What is its pH (pKa for CH3COOH = 4.57)
5.09
57. The pH of a 0.02 M Mg(OH)2 solution is...
12.7
58. The pH of a 0.0001 M of HNO3?
4
59. Calculate the pH of a buffer solution that is 0.25 M in Formic acid and 0.1 M in sodium formate (ka for formic acid is 1.8 × 10–4)
3.35
60. The strength or degree of dissociation of 0.001 M propanoic acid is... (ka for propanoic acid is 1.5 × 10–5)
1.22 × 10–4
61. Which of the following is a Diprotic acid?
H2SO4
62. The relationship between pH, pKa, and log (salt / acid) is known as...
Henderson–Hasselbalch equation
63. The pH value of two equimolar solutions of two Monoprotic acids A and B are 2 and 4 respectively. Which is more acidic?
A
64. The concentration of H+ in a solution is 1.5 × 10–6. Find the concentration of OH– and state if the solution is acidic or basic.
6.67 × 10–9 / acidic
65. _ substances are molecules or ions that can behave as Brønsted acid and base
Amphiprotic
66. Calculate the dissociation constant of a base, given that ka = 6.8 × 10–4
1.5 × 10–11
67. A solution which maintains its pH fairly constant even upon the addition of small amount of acid or base is...
A buffer solution
68. Which of the following pair is not a Brønsted–Lowry acid/base
MgO / SO2
69. Alkali metals replace hydrogen in organic acids forming salts such as _ and _
CH3COONa and C6H5COOK
70. Carbon dioxide is _
An acidic oxide
