[GENERAL CHEMISTRY] Solution Equilibria

Proverbs 16:3

a. Acid

[ACIDS AND BASES]

Sour taste.

a. Acid

b. Base

b. Base

[ACIDS AND BASES]
Bitter taste

a. Acid

b. Base

a. Acid

[ACIDS AND BASES]
Turn red in litmus paper.

a. Acid

b. Base

b. Base

[ACIDS AND BASES]

Turn blue in litmus paper.

a. Acid

b. Base

a. Acid

[ACIDS AND BASES]
Produce H2 gas with metals which corrode metals.

a. Acid

b. Base

a. Acid

[ACIDS AND BASES]
Produce CO2 gas or effervescence with carbonate/bicarbonates.

a. Acid

b. Base

b. Base

[ACIDS AND BASES]
When added to fat, it produce soap which is slippery.

a. Acid

b. Base

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

[ACIDS AND BASES]

Used in manufacturing of soap.

a. Acid and fat

b. Acid and bicarbonates

c. Base and fat

d. Base and carbonates

a. NaOH

[ACIDS AND BASES]

Specifically used for manufacturing of hard soap.

a. NaOH

b. KOH

c. ClO-

d. H2SO4

b. KOH

[ACIDS AND BASES]
Specifically used for manufacturing of soft soap.

a. NaOH

b. KOH

c. ClO-

d. H2SO4

a. Arrhenius theory

[THEORIES]

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

a. Arrhenius theory

b. Bronsted-Lowry theory

c. Lewis theory

b. Bronsted-Lowry theory

[THEORIES]

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

a. Arrhenius theory

b. Bronsted-Lowry theory

c. Lewis theory

c. Lewis theory

[THEORIES]
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

a. Liberate H+

[THEORIES]
Arrhenius acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

c. Proton donor

[THEORIES]
Bronsted-Lowry acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

f. Electron acceptor

[THEORIES]
Lewis acid.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

b. Liberate OH-

[THEORIES]
Arrhenius base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

d. Proton acceptor

[THEORIES]

Bronsted-Lowry base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

e. Electron donor

[THEORIES]

Lewis base.

a. Liberate H+

b. Liberate OH-

c. Proton donor

d. Proton acceptor

e. Electron donor

f. Electron acceptor

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 THEORY]
Lewis acid except:

a. Nucleophile

b. Electron (e-) loving

c. Positive (+) ions

d. Electron poor species

e. Metals

f. None

a. I, II, III, IV

[LEWIS THEORY]

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. Ni

[LEWIS THEORY]

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

a. Ni

b. Co

c. Both

d. None

b. Co

[LEWIS THEORY]

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

a. Ni

b. Co

c. Both

d. None

b. SnCl4

[LEWIS THEORY]
Which is the Lewis acid (+) in the reaction: Cl- + SnCl4

a. Cl-

b. SnCl4

c. Both

d. None

a. Cl-

[LEWIS THEORY]

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

a. Cl-

b. SnCl4

c. Both

d. None

a. Pearson

[ACIDS AND BASES]

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

a. Pearson

b. Le Chatelier

c. Henry

d. Van slyke

d. a and b

[ACIDS AND BASES]

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

a. Ionic complexes

[ACIDS AND BASES]

Hard acid + hard base will form:

a. Ionic complexes

b. Covalent complexes

c. Both

d. None

b. Covalent complexes

[ACIDS AND BASES]
Soft acid + soft base will form:

a. Ionic complexes

b. Covalent complexes

c. Both

d. None

e. b and c

[ACIDS AND BASES]

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. I, II, IV

Hard acids and bases properties:

I) Small ionic radius

II) High oxidation states

*III) Low polarizability

IV) High electronegativity

[ACIDS AND BASES]
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

d. I, III, IV

Soft acids and bases properties:

I) Large ionic radius

*II) Low oxidation states

III) High polarizability

IV) Low electronegativity

[ACIDS AND BASES]
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. a and b

Example of hard acids and bases:

a) Ions of alkali earth metals

b) Ions of alkaline earth metals

[ACIDS AND BASES]
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

c. Heavy metals

[ACIDS AND BASES]
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

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

[ACIDS AND BASES]

Example of hard acids and bases except:

a. H+

b. NH4

c. Ti4+

d. Cr3+

e. Cd2+

f. None

f. None

[ACIDS AND BASES]
Example of hard acids and bases except:

a. OH-

b. F-

c. Cl-

d. CO3^2-

e. CH3COO-

f. None

f. None

[ACIDS AND BASES]
Example of soft acids and bases except:

a. Ag+

b. Au+

c. Hg2^2+

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]

Example of soft acids and bases except:

a. H+

b. I-

c. SCN-

d. Hg2+

e. Cd2+

f. None

b. False

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

[ACIDS AND 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

e. None

[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

[ACIDS AND BASES]
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

a. True

[ACIDS AND BASES]

pka is constant while pH varies.

a. True

b. False

a. True

[ACIDS AND BASES]

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

a. True

b. False

a. HA and A-

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

[ACIDS AND BASES]

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-

b. H20 and H30

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

[ACIDS AND BASES]
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-

a. True

[ACIDS AND BASES]

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

a. True

b. False

e. a and c

*b) Solid and liquid is NOT included.

[ACIDS AND BASES]

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

f. All

[ACIDS AND BASES]
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

c. Common Ion Effect

This is the addition of a compound having an ion in common with the dissolved substance will result to:

• Equilibrium shift

• Suppressed ionization of the dissolved substance (WA or WB)

• pH change

a. Le Chatelier's Principle

b. Buffer Capacity

c. Common Ion Effect

d. Solubility Product

a. True

[ACIDS AND BASES]
All inorganic and organic salts are strong electrolytes which has 100% dissociation.

a. True

b. False

b. CH3COO-

[ACIDS AND BASES]

Common ion of CH3COONa with CH3COOOH.

a. CH3COO+

b. CH3COO-

c. H+

d. CH3-

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

[ACIDS AND BASES]

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

e. b and c

Buffer solution is composed of:

b) Weak acid and its conjugate base

c) Weak base and its conjugate acid

[ACIDS AND BASES]

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

c. Both

[ACIDS AND BASES]
Which is an example of buffer solution among the following :

a. HAc + Ac-

b. NH3 + NH4

c. Both

d. None

a. True

[ACIDS AND BASES]

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

a. True

b. False

b. Henderson-Hasselbalch

[ACIDS AND BASES]
Buffer pair equation is by:

a. Noyes Whitney

b. Henderson-Hasselbalch

c. Pearson

d. Van Slyke

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

[ACIDS AND BASES]
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)

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

[ACIDS AND BASES]
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)

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

[ACIDS AND BASES]

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

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)

[ACIDS AND BASES]

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

b. Buffer solution

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

a. Neutralization reaction

b. Buffer solution

c. Salt hydrolysis

d. Amphoteric substance

d. Van Slyke

[ACIDS AND BASES]

Buffer capacity equation is by:

a. Noyes Whitney

b. Henderson-Hasselbalch

c. Pearson

d. Van Slyke

e. All

[ACIDS AND BASES]
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

a. True

[ACIDS AND BASES]

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

a. True

b. False

a. Solubility

[ACIDS AND BASES]
Number of grams of solute dissolved in in 1L of saturated solution.

a. Solubility

b. Molar solubility

c. Molality

d. Normality

b. Molar solubility

[ACIDS AND BASES]

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

a. Solubility

b. Molar solubility

c. Normality

d. Molality

d. g/L

[ACIDS AND BASES]

Standard unit of solubility:

a. mg/100mL

b. g/mL

c. g/100mL

d. g/L

d. mol/L

[ACIDS AND BASES]

Standard unit of molar solubility:

a. mol/100mL

b. mol/mL

c. mol/100mL

d. mol/L

f. All

[ACIDS AND BASES]
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

a. True

[ACIDS AND BASES]
In computing for Ksp, equilibrium constant is used while in computing for Q, unionized or initial concentration is used.

a. True

b. False

c. Supersaturated

[ACIDS AND BASES]
Q > Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

b. Saturated

[ACIDS AND BASES]
Q = Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

a. Unsaturated

[ACIDS AND BASES]

Q < Ksp

a. Unsaturated

b. Saturated

c. Supersaturated

a. Noyes Whitney Equation

[ACIDS AND BASES]

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

d. None

[ACIDS AND BASES]

Dissolution rate increases with the increase of the following except:

a. Surface area

b. Solute concentration at boundary layer

c. Diffusion coefficient

d. None