Part 11 - Solution Equilibria

Sour taste.

a. Acid

b. Base

a. Acid

Bitter taste

a. Acid

b. Base

b. Base

Turn red in litmus paper.

a. Acid

b. Base

a. Acid

Turn blue in litmus paper.

a. Acid

b. Base

b. Base

Produce H2 gas with metals which corrode metals.

a. Acid

b. Base

a. Acid

Produce CO2 gas or effervescence with carbonate/bicarbonates.

a. Acid

b. Base

a. Acid

When added to fat, it produce soap which is slippery.

a. Acid

b. Base

b. Base

Used in manufacturing of soap.

a. Acid and fat

b. Acid and bicarbonates

c. Base and fat

d. Base and carbonates

c. Base and fat - manufacturing of soap is also known as the saponification.

Specifically used for manufacturing of hard soap.

a. NaOH

b. KOH

c. ClO-

d. H2SO4

a. NaOH

Specifically used for manufacturing of soft soap.

a. NaOH

b. KOH

c. ClO-

d. H2SO4

b. KOH

State that acid liberates H+ and base liberates OH-.

a. Arrhenius theory

b. Bronsted-Lowry theory

c. Lewis theory

a. Arrhenius theory

State that acid donates p+ and base accepts p+.

a. Arrhenius theory

b. Bronsted-Lowry theory

c. Lewis theory

b. Bronsted-Lowry theory

State that acid is an e- pair acceptor and base is an e- pair donor.

a. Arrhenius theory

b. Bronsted-Lowry theory

c. Lewis theory

c. Lewis theory

Arrhenius acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

a. Liberate H+

Bronsted-Lowry acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

c. Proton donor

Lewis acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

f. Electron acceptor

Arrhenius base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

b. Liberate OH-

Bronsted-Lowry base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

d. Proton acceptor

Lewis base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

e. Electron donor

Lewis acid except:

a. Nucleophile

b. Electron (e-) loving

c. Positive (+) ions

d. Electron poor species

e. Metals

f. None

a. Nucleophile

Lewis acid:

*a) Electrophile

b) Electron (e-) loving

c) Positive (+) ions

d) Electron poor species - thus they love electron because it’s something that they don’t have

e) Metals

Lewis base:

I. Nucleophile

II. Negative (-) ion

III. Nonmetals

IV. Electron (e-) rich species

a. I, II, III, IV

b. I, II, III

c. II, III, IV

d. I, III, IV

e. II, IV

a. I, II, III, IV

Which is the Lewis acid (+) in the reaction: Ni + CO

a. Ni

b. Co

c. Both

d. None

a. Ni

Which is the Lewis base (-) in the reaction: Ni + CO

a. Ni

b. Co

c. Both

d. None

b. Co

Which is the Lewis acid (+) in the reaction: Cl- + SnCl4

a. Cl-

b. SnCl4

c. Both

d. None

b. SnCl4

Which is the Lewis base (-) in the reaction: Cl- + SnCl4

a. Cl-

b. SnCl4

c. Both

d. None

a. Cl-

Hard and Soft Acid and Base (HSAB) theory is by:

a. Pearson

b. Le Chatelier

c. Henry

d. Van slyke

a. Pearson

Combination of acid and base that will lead to thermodynamically stronger interaction.

a. Hard-Hard

b. Soft-Soft

c. Hard-Soft

d. a and b

e. b and c

f. All

d. a and b

Hard acid + hard base will form:

a. Ionic complexes

b. Covalent complexes

c. Both

d. None

a. Ionic complexes

Soft acid + soft base will form:

a. Ionic complexes

b. Covalent complexes

c. Both

d. None

b. Covalent complexes

Combination of acid and base that will lead to thermodynamically weaker interaction.

a. Hard-Hard

b. Soft-Hard

c. Hard-Soft

d. a and b

e. b and c

f. All

e. b and c

Hard acids and bases properties:

I. Small ionic radius

II. High oxidation states

III. High polarizability

IV. High electronegativity

a. I, II, III, IV

b. I, II, III

c. II, III, IV

d. I, III, IV

e. I, II, IV

e. I, II, IV

Hard acids and bases properties:

I) Small ionic radius

II) High oxidation states

*III) Low polarizability

IV) High electronegativity

Soft acids and bases properties:

I. Large ionic radius

II. High oxidation states

III. High polarizability

IV. Low electronegativity

a. I, II, III, IV

b. I, II, III

c. II, III, IV

d. I, III, IV

e. I, II, IV

d. I, III, IV

Soft acids and bases properties:

I) Large ionic radius

*II) Low oxidation states

III) High polarizability

IV) Low electronegativity

Example of hard acids and bases:

a. Ions of alkali earth metals

b. Ions of alkaline earth metals

c. Heavy metals

d. a and b

e. b and c

f. All

d. a and b

Example of hard acids and bases:

a) Ions of alkali earth metals

b) Ions of alkaline earth metals

Example of soft acids and bases:

a. Ions of alkali earth metals

b. Ions of alkaline earth metals

c. Heavy metals

d. a and b

e. b and c

f. All

c. Heavy metals

Example of hard acids and bases except:

a. H+

b. NH4

c. Ti4+

d. Cr3+

e. Cd2+

f. None

e. Cd2+ - this is one of heavy metals which are soft acid or bases.

Example of hard acids and bases except:

a. OH-

b. F-

c. Cl-

d. CO3^2-

e. CH3COO-

f. None

f. None

Example of soft acids and bases except:

a. Ag+

b. Au+

c. Hg2^2+

d. Hg2+

e. Cd2+

f. None

f. None

Example of soft acids and bases except:

a. H+

b. I-

c. SCN-

d. Hg2+

e. Cd2+

f. None

a. H+ - this is under hard. H- or hydride is what’s under soft acids or bases.

Acids and bases general formulas are for weak acids and base while ionic equilibria is for strong acids and base.

a. True

b. False

b. False

Acids and bases general formulas are for STRONG acids and base while ionic equilibria is for WEAK acids and bases.

Acid and bases general formulas except:

a. pH = -log[H+]

b. pOH = -log[OH-]

c. pH + pOH = 14

d. Kw = [H+][OH-] = 1x10^-14

e. None

e. None

Ionic equilibria formulas except:

a. pKa = -log[ka]

b. pKb = -log[kb]

c. pKa + pKb = 14

d. Kw = Ka x Kb = 1x10-1

e. None

e. None

pka is constant while pH varies.

a. True

b. False

a. True

In measurement of acid and bases, concentration is expressed as [ ] which denotes automatically that concentration is in Molar (M).

a. True

b. False

a. True

Identify the acid and its conjugate base in the following reaction:

HA (aq) + H2O (l) <—> H30 (aq) + A- (aq)

a. HA and H30

b. H20 and H30

c. HA and H2O

d. H3O and A-

a. HA and A-

Conjugate base is minus 1 H+ from the substance in question thus HA (acid) and A- (conjugate base)

Identify the base and its conjugate acid in the following reaction:

HA (aq) + H2O (l) <—> H30 (aq) + A- (aq)

a. HA and H30

b. H20 and H30

c. HA and H2O

d. H3O and A-

b. H20 and H30

Conjugate acid is plus 1 H+ to the substance in question thus H20 (base) and H3O (conjugate acid).

Ka = [H+][A-]/[HA]

a. True

b. False

a. True

In writing Equilibrium constants:

a. Aqueous and gaseous reacting species are included

b. Solid and liquid forms are included

c. Unit should be in Molar (M)

d. a and b

e. a and c

f. All

e. a and c

*b) Solid and liquid is NOT included.

In common ion effect addition of compound having an ion in common with the dissolved substance will result to:

a. Equilibrium shift (either to the left or right)

b. Suppressed ionization of the dissolved substance (weak acid or weak base)

c. pH change

d. a and b

e. b and c

f. All

f. All

All inorganic and organic salts are strong electrolytes which has 100% dissociation.

a. True

b. False

a. True

Common ion of CH3COONa with CH3COOOH.

a. CH3COO+

b. CH3COO-

c. H+

d. CH3-

b. CH3COO-

Mixing CH3COONa with CH3COOOH will result to:

a. Increase CH3COO-

b. Increase pH

c. Suppressed ionization of CH3COOH

d. Equilibrium shift to the left

e. None

f. All

f. All

Mixing CH3COONa with CH3COOOH will result to:

a. Increase (CH3COO-) - as their common ion

b. Increase pH - since CH3COO- is basic

c. Suppressed ionization of CH3COOH

d. Equilibrium shift to the left - to balance the increased CH3COO- in the product side

Buffer solution is composed of:

a. Strong acid and conjugate base

b. Weak acid and its conjugate base

c. Weak base and its conjugate acid

d. a and b

e. b and c

f. All

e. b and c

Buffer solution is composed of:

b) Weak acid and its conjugate base

c) Weak base and its conjugate acid

Which is an example of buffer solution among the following :

a. HAc + Ac-

b. NH3 + NH4

c. Both

d. None

c. Both

Conjugate acid and base doesn't exists in ionized form but in its salt form only.

a. True

b. False

a. True

Buffer pair equation is by:

a. Noyes Whitney

b. Henderson-Hasselbalch

c. Pearson

d. Van Slyke

b. Henderson-Hasselbalch

ph of buffer solution of weak acid:

a. pH = pka + log (salt/acid)

b. pH = pka + log (acid/salt)

c. pH = pkb + log (base/salt)

d. pH = pkb + log (salt/base)

a. pH = pka + log (salt/acid)

ph of buffer solution of weak base:

a. pH = pka + log (salt/acid)

b. pH = pka + log (acid/salt)

c. pH = pkb + log (base/salt)

d. pH = pkb + log (salt/base)

c. pH = pkb + log (base/salt)

pH = pka at

a. Half neutralization point

b. Equimolar mixture

c. Neutral medium

d. a and b

e. b and c

f. All

d. a and b

Most of the buffer system is in equimolar mixture:

• pH = pka + log (2M/2M)

• pH = pka + log (1)

• pH = pka + 0

• pH = pka

Buffer solution:

a. Has the ability to resist changes in pH upon addition of large amounts of either acid or base

b. Weak acid and its CB (salt of WA)

c. Weak base and its CA (salt of WB)

d. a and b

e. b and c

f. All

d. a and b

Buffer solution:

*a) Has the ability to resist changes in pH upon addition of SMALL amounts of either acid or base

b) Weak acid and its CB (salt of WA)

c) Weak base and its CA (salt of WB)

Buffer capacity equation is by:

a. Noyes Whitney

b. Henderson-Hasselbalch

c. Pearson

d. Van Slyke

d. Van Slyke

Degree or magnitude of capability to resist change in pH of the buffer.

a. Buffer capacity

b. Buffer index

c. Buffer value

d. Buffer efficiency

e. All

e. All

The higher the solubility product constant (Ksp), the higher the solibility.

a. True

b. False

a. True

Number of grams of solute dissolved in in 1L of saturated solution.

a. Solubility

b. Molar solubility

c. Molality

d. Normality

a. Solubility

Number of moles of solute dissolved in 1L of saturated solution

a. Solubility

b. Molar solubility

c. Normality

d. Molality

b. Molar solubility

Standard unit of solubility:

a. mg/100mL

b. g/mL

c. g/100mL

d. g/L

d. g/L

Standard unit of molar solubility:

a. mol/100mL

b. mol/mL

c. mol/100mL

d. mol/L

d. mol/L

Ion product constant:

a. Denoted as Q

b. Computed based on initial concentration

c. Used in predicting formation of precipitate formation

d. a and b

e. b and c

f. All

f. All

In computing for Ksp, equilibrium constant is used while in computing for Q, unionized or initial concentration is used.

a. True

b. False

a. True

Q > Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

c. Supersaturated

Q = Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

b. Saturated

Q < Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

a. Unsaturated

Dissolution rate is directly proportional to the solute surface area, solute concentration at boundary layer, and diffusion coefficient.

a. Noyes Whitney Equation

b. Henderson-Hasselbalch Equation

c. Pearson's Theory

d. Van Slyke Equation

a. Noyes Whitney Equation

Dissolution rate increases with the increase of the following except:

a. Surface area

b. Solute concentration at boundary layer

c. Diffusion coefficient

d. None

d. None