Chapter 09: Acid Base Chemistry
Interactive MCQs & Virtual Chemistry Lab
Multiple Choice Questions
Q.1 Given the following reaction: NH 3(g) + H2O,)NH (ag) + OH (ag)
pH and pOH
Q.2 The pH of 10-3 mol dm of an aqueous solution of H2SO4 is:
Solubility Product
Q.3 The solubility product of AgCl is 2.0 × 10-1° mol? dm. The maximum concentration of Ag+ ions in the solution is:
Q.4
Which indicator is typically used for titrations involving strong acids and strong bases?
Concepts of Acids and Bases
Q.5
Which of the following is the conjugate base of water?
Lewis Concept
Q.6
Which of the following is a Lewis acid but not a Bronsted-Lowry acid?
Q.7
In an acid-base titration, the equivalence point is reached when:
Q.8
If the concentration of Cl ion in a solution is increased, the solubility of silver chloride (AgCl) will:
Q.9
Which of the following pairs of substances can act as a conjugate acid-base pair according to the Bronsted-Lowry theory?
Q.10
If the pH of a solution is 11, what is the [OH] concentration in the solution?
Buffer Solutions
Q.11
Which of the following pairs forms a buffer solution?
Q.12
An acid and base react to give a acid and base.
Q.13 The conjugate base of HCO4 is:
Q.14 The definition of amphoteric is:
Q.15
Which is amphoteric?
Q.16
The Bronsted-Lowry definition identifies acids as:
Q.17 In the reaction NH3 + H2O → NH4* + OH, H2O acts as a:
Q.18 Which one is a monoprotic acid
Q.19
The conjugate acid of NH: is:
Q.20 The conjugate base of H2CO3 is
Q.21
Which of these is NOT a property of acids?
Q.22
Litmus turns which color in a basic solution?
Q.23
Which acid is present in vinegar?
Q.24
Which of the following is a tribasic acid?
Q.25
Which of the following is a diprotic acid?
Q.26
Which species is both a Bronsted acid and base?
Q.27
NaOH is not considered an Bronsted- Lowry acid because:
Q.28 Hcl + NH3 → NH4Cl shows:
Q.29
Which one is a Lewis acid?
Q.30
Which one is a Lewis base?
Ionic Product of Water
Q.31
Water's ion product Kw at 25 °C is:
Q.32
Which has the highest pH?
Q.33
pH of 1x10* M HCl is:
Q.34 The pOH of 1x103 M HCl is:
Q.35
A solution at pH < 7 has:
Q.36 If [H*] = 1x10-s M, then pH =
Q.37
Which dialyzing solution has highest pH?
Q.38
A 0.01 M solution of a strong acid has a pH of:
Q.39 The pH scale ranges typically from:
Q.40
The pH of distilled water at 25 °C is:
Q.41
pH of 10-9 M HCl is:
Q.42 KOH is an example of a:
Q.43
Which has the lowest pH?
Q.44
The pH of a buffer doesn't change much when:
Q.45 Acid rain is mainly due to:
Q.46
Which is more acidic: pH 3 or pH 5?
Q.47 The logarithmic nature of pH means:
Q.48
pH of blood is around:
Q.49
A solution with equal [Ht] and [OH] is:
Q.50
Which of the following does not affect pH?
Q.51
Strong acids completely dissociate in water because:
Q.52
Which of the following is a weak base?
Q.53
If Ka of acetic acid is 1.8 × 10s, it is:
Q.54 The strength of a base is measured by its:
Q.55
A base that ionizes completely in aqueous solution is called:
Q.56 An acid with low Ka Value is:
Q.57 Strong bases have:
Q.58
Which is a weak acid?
Q.59
The Ka of a weak acid is 105. Its pKa is:
Common Ion Effect
Q.60
Which one of the following compound is added in purification of NaCl in common ion effect.
Q.61
The suppression of ionization of a weak electrolyte by adding common ion is:
Q.62 A buffer solution is:
Q.63
The pK. value for HCOOH is?
Q.64 The solubility product of PbSO4 is:
Q.65
Which one of the following is not the application of solubility products?
Q.66 A salt from strong acid + weak base gives:
Q.67 CH COONa is a salt of:
Q.68 Strong neutralization gives:
Q.69 A salt that hydrolyzes in water is from:
Q.70 A substance that changes color with pH is a:
Q.71 Methyl orange in base turns:
Q.72
In a titration, the equivalence point is when:
pH Titration Lab Simulator
Drop NaOH into HCl solution and monitor pH changes.
Volume Added: 0 mL
Color Indicator: Methyl Red