StudentAidUnit 9: Unit 9: Acid-Base Chemistry — Mcqs
11th Class Chemistry · Unit 9: Acid-Base Chemistry
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1.Given the following reaction: NH3(aq) + H2O(l) → NH4(aq) + OH(aq)
2.The pH of 10-3 mol dm-3 of an aqueous solution of H2SO4 is:
3.The solubility product of AgCl is 2.0 × 10-10 mol2 dm-6. The maximum concentration of Ag+ ions in the solution is:
4.Which indicator is typically used for titrations involving strong acids and strong bases?
5.Which of the following is the conjugate base of water?
6.Which of the following is a Lewis acid but not a Bronsted-Lowry acid?
7.In an acid-base titration, the equivalence point is reached when:
8.If the concentration of Cl- ion in a solution is increased, the solubility of silver chloride (AgCl) will:
9.Which of the following pairs of substances can act as a conjugate acid-base pair according to the Bronsted-Lowry theory?
10.If the pH of a solution is 11, what is the [OH-] concentration in the solution?
11.Which of the following pairs forms a buffer solution?
Bronsted lowery concept
12.An acid and base react to give a _____ acid and base.
13.The conjugate base of HClO4 is:
14.The definition of amphoteric is:
15.Which is amphoteric?
16.The Bronsted-Lowry definition identifies acids as:
17.In the reaction NH3 + H2O → NH4+ + OH-, H2O acts as a:
18.Which one is a monoprotic acid
19.The conjugate acid of NH3 is:
20.The conjugate base of H2CO3 is
21.Which of these is NOT a property of acids?
22.Litmus turns which color in a basic solution?
23.Which acid is present in vinegar?
24.Which of the following is a tribasic acid?
25.Which of the following is a diprotic acid?
26.Which species is both a Bronsted acid and base?
27.NaOH is not considered an Bronsted-Lowry acid because:
28.HCl + NH3 → NH4Cl shows:
Lewis concept
29.Which one is a Lewis acid?
30.Which one is a Lewis base?
Ionic product of H2O
31.Water's ion product Kw at 25°C is:
pH and pOH
32.Which has the highest pH?
35.A solution at pH < 7 has:
36.If [H+] = 1 × 10-5 M, then pH =
37.Which dialyzing solution has highest pH?
38.A 0.01 M solution of a strong acid has a pH of:
39.The pH scale ranges typically from:
40.The pH of distilled water at 25°C is:
41.pH of 10-9 M HCl is:
42.KOH is an example of a:
43.Which has the lowest pH?
44.The pH of a buffer doesn't change much when:
45.Acid rain is mainly due to:
46.Which is more acidic: pH 3 or pH 5?
47.The logarithmic nature of pH means:
48.pH of blood is around:
49.A solution with equal [H+] and [OH-] is:
50.Which of the following does not affect pH?
Ionization constant of acids
51.Strong acids completely dissociate in water because:
52.Which of the following is a weak base?
53.If Ka of acetic acid is 1.8 × 10-5, it is:
54.The strength of a base is measured by its:
55.A base that ionizes completely in aqueous solution is called:
56.An acid with low Ka value is:
57.Strong bases have:
58.Which is a weak acid?
59.The Ka of a weak acid is 10-5. Its pKa is:
Common Ion Effect
60.Which one of the following compound is added in purification of NaCl in common ion effect.
61.The suppression of ionization of a weak electrolyte by adding common ion is:
Buffer Solution
62.A buffer solution is:
63.The pKa value for HCOOH is?
Solubility Product
64.The solubility product of PbSO4 is:
65.Which one of the following is not the application of solubility products?
Salt Hydrolysis
66.A salt from strong acid + weak base gives:
67.CH3COONa is a salt of:
68.Strong acid + strong base neutralization gives:
69.A salt that hydrolyzes in water is from:
Acid-Base Indicators
70.A substance that changes color with pH is a:
71.Methyl orange in base turns:
72.In a titration, the equivalence point is when: