Name
Chemistry 12
PLO Set 4
J: ACIDS, BASES, AND SALTS (Properties and Definitions)
J1. J2. List general properties of acids and bases
J3. Write the balanced equation representing the neutralization of HCl by KOH in solution
J4. Define Arrhenius acids and bases
J5. Write names and formulae of some common acids and bases and outline some of their common
properties, uses, and commercial names
J6. Define Brönsted-Lowry acids and bases
J7. Identify the Brönsted-Lowry acids and bases in the equation
NH3 + H2O NH4+ + OH-
J8. Write balanced equations representing the reaction of water with
HCl
CO32J9. Explain the true nature of H+(aq) (i.e. the hydronium ion)
J10. Define conjugate acid-base pair
J11. Identify the conjugate of
HCN
CO32J12. Show that in any Brönsted-Lowry acid-base equation there are two conjugate pairs present.
K: ACIDS, BASES, AND SALTS (Strong and Weak Acids and Bases)
K1. How is electrical conductivity related to the strength of an acid or base?
K2. Will the conductivity of 1.0M HCN be greater or less than that of 1.0M H3PO4?
K3. Define a strong acid and a strong base
K4. Define a weak acid and a weak base
K5. Write equations to show
the ionization of HClO4 in water
the ionization of HF in water
the base ionization of NH2- in water
the ionization of NH3 in water
K6. compare the relative strengths, by using a table of relative acid strengths, of
HCN and HSO4CN- and HSK7. Explain why the strongest acid in aqueous solutions is H3O+ and the strongest base in aqueous
solutions is OH– (the leveling effect)
K8. Predict whether products or reactants are favoured by comparing the strength of the two acids :
NH4+ + CN- qe HCN + NH3
K9. Compare (qualitatively) the relative concentrations of H3O+ between HSO4- and CH3COOH using their
relative positions on an acid strength table
K10. Define amphiprotic
K11. Identify chemical species that are amphiprotic
(state some general rules that could be used as a guide to identifying amphiprotic species)
K12. Describe situations in which H2O would act as an acid or base
L: ACIDS, BASES, AND SALTS (Kw, pH, pOH)
L1. Write both forms (H3O+ and H+) of the equation representing the ionization of water:
L2. Write the equilibrium expression for the ion product constant of water, Kw
L3. For the equilibrium system 2H2O(l)qeH3O+(aq) + OH–(aq), predict the effect of the addition of
an acid
a base
L4. State the relative (qualitative) concentrations of H3O+ and OH– in acid, base, and neutral solutions
L5. State the value of Kw at 25°C:
L6. Describe the variation of the value of Kw with temperature
L7. Calculate [H3O+], using Kw, for an aqueous solution with [OH-] = 5.0 x 10-5M
L: ACIDS, BASES, AND SALTS (Kw, pH, pOH) (continued)
L8. Describe the pH scale (qualitatively) with reference to everyday substances such as lemon juice, battery
electrolyte, oven cleaner, distilled water, and soap:
L9. Define pH and pOH
L10. Define pKw , give its value at 25°C, and its relation to pH and pOH
L11. Calculate the pH of a 0.02M solution of NaOH
L12. Find [H+] in a solution whose pOH = 12.30
M: ACIDS, BASES, AND SALTS (Ka and Kb Problem Solving)
M1. write Ka and Kb equilibrium expressions for both acid ionization and base ionization of HCO3-
M2. Find the value of Ka or Kb for HCO3-, and state whether it is stronger as an acid or as a base, as
determined by the Ka and Kb values.
M3. For a 2.0M concentration of acetic acid, find:
- [H3O+]
- [OH–]
- pH
- pOH
M4. What is Kb for H2PO4-? Show calculations.
M5. calculate the value of Ka for a 0.50M weak acid solution with pH = 3.66
N: ACIDS, BASES, AND SALTS (Hydrolysis of Salts)
N1. Write a dissociation equation for a Na2CO3 in water
N2. Write the net ionic equation representing the hydrolysis of Na2CO3.
N3. Predict qualitatively whether a Na2CO3 solution would be acidic, basic, or neutral
N4. Determine whether HC2O4- will act as a base or an acid in solution.