Weak Electrolyte Dissociation Quiz

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Questions and Answers

Which of the following is true about colligative properties?

The relative number of solute molecules and the nature of the solute and the solvent affect colligative properties

The relative number of solute molecules in the solution and nature of the solvent affect colligative properties (correct)

The relative number of solvent molecules affect colligative properties

The relative number of solute molecules is irrespective of the solute and the solvent nature

According to Raoult’s law, what does the relative lowering of saturated vapour pressure depend on for a dilute solution?

The relative lowering of saturated vapour pressure is equal to the mole fraction of the solute (correct)

The relative lowering of saturated vapour pressure is proportional to the amount of the solute in the solution

The lowering of saturated vapour pressure is equal to the mole fraction of the solute

The saturated vapour pressure of the solution is equal to the mole fraction of the solvent

What does the vapour pressure of the solvent above the solution depend on?

Molar concentration of the solvent

Mole fraction of the solute

Molar concentration of the solute

Mole fraction of the solvent (correct)

Which statement correctly describes the freezing point of the solution (Tf)?

Separation of the first crystal of the solvent takes place (D) Signup and view all the answers

Which of the following best describes the boiling point of a solution?

It is always higher than that of the pure solvent (D) Signup and view all the answers

What determines the osmotic pressure of a solution?

The number of particles in the solution (C) Signup and view all the answers

What is the characteristic of Kb (the molar boiling point elevation constant)?

Solvent (C) Signup and view all the answers

What happens to osmotic pressure when the temperature decreases?

Decreases (A) Signup and view all the answers

What type of solution has a lower osmotic pressure than a reference solution?

Hypotonic solution (D) Signup and view all the answers

Which solution has the higher osmotic pressure among the options?

1M NaCl (A) Signup and view all the answers

What is the osmotic pressure of a 0.1 M nonelectrolyte solution at 0°C?

2.24 atm (D) Signup and view all the answers

Which statement is correct for Vant Hoff’s law?

The osmotic pressure (π) of a solution is the pressure required to increase osmosis from pure solvent into the solution. (D) Signup and view all the answers

Which expressions are used for determination of molar concentration?

1,3,5 (D) Signup and view all the answers

What is correct for determination of a molar mass of a substance?

M = rac{ riangle Tf imes m_{solvent}}{m_{solute}} (A) Signup and view all the answers

What is the boiling point (Tb) of a 1M glucose solution?

100.520C (D) Signup and view all the answers

What is the freezing point (Tf) of a 1M glucose solution?

-1.860C (D) Signup and view all the answers

Which statement about ionic strength is correct?

Al(NO3)3 has the highest ionic strength among equimolar solutions. (D) Signup and view all the answers

Which species has the highest activity factor for K+ ions?

K3PO4 (C) Signup and view all the answers

According to Lewis concept, which statement is true about acids?

An acid is a substance that donates a lone pair of electrons. (A) Signup and view all the answers

Which statement regarding Ostwald's dilution law is correct?

The correct expression for Ostwald's dilution law is K = Cα2. (D) Signup and view all the answers

Among the given equimolar solutions, which one has the lowest ionic strength?

Na3PO4 (D) Signup and view all the answers

Which statement about the activity factor of NO3 - ions is correct?

The activity factor of NO3 - ions is lowest in Al(NO3)3. (B) Signup and view all the answers

Which compound has the highest ionic strength among ZnSO4, Na2SO4, and NaCl?

Fe2(SO4)3 (A) Signup and view all the answers

According to Bronsted-Lowry concept, what happens to the conjugate base as the acid gets stronger?

The conjugate base becomes stronger. (C) Signup and view all the answers

Which solvents have a leveling effect on acids?

Solvents with lower affinity towards protons. (D) Signup and view all the answers

Which equation is used to determine the ionic strength for strong electrolytes?

I = 1/2 Σcz2 (D) Signup and view all the answers

Which type of system does not allow transfer of matter but allows transfer of energy to and from surroundings?

Closed system (D) Signup and view all the answers

Which of the following is an example of a state function?

Entropy (B) Signup and view all the answers

What is the equation for entropy change (ΔS) in terms of the entropy change of the system (ΔSsys) and the entropy change of the surroundings (ΔSsurr)?

ΔS = ΔSsys + ΔSsurr (C) Signup and view all the answers

What is the criteria for spontaneity of a reaction?

ΔG < 0 (C) Signup and view all the answers

Which thermodynamic potential measures the maximum reversible work that can be done by a system at constant temperature and pressure?

Gibbs free energy (G) (B) Signup and view all the answers

What is the equation for Gibbs free energy change (ΔG) for a reaction?

ΔG = ΔH - TΔS (B) Signup and view all the answers

For which type of reaction does the heat released have a negative value?

Exothermic reaction (C) Signup and view all the answers

What type of reaction absorbs energy from its surroundings?

Endothermic reaction (D) Signup and view all the answers

Which law deals with the relationship between heat changes that occur during a series of reactions?

Hess's law (D) Signup and view all the answers

What does the change in Gibbs free energy (ΔG) for a reaction represent?

The maximum reversible work that can be done by the reaction at constant temperature and pressure (A) Signup and view all the answers

What quantity is independent of the path taken to reach that state?

State functions (B) Signup and view all the answers

What potential measures the disorder or randomness of a system?

Entropy (S) (C) Signup and view all the answers

Which of the following factors does NOT affect the dissociation constant (K) of a weak electrolyte?

The osmotic pressure of the solution (A) Signup and view all the answers

Which of the following statements about the dissociation degree of a weak electrolyte (α) is correct?

“α” increases by dilution of water solution (B) Signup and view all the answers

When NH4Cl is added to a solution of NH4OH, what happens to the concentration of OH–?

Concentration of OH– decreases (D) Signup and view all the answers

Which factor does NOT practically affect the dissociation degree of acetic acid in an aqueous solution?

Raising the temperature (B) Signup and view all the answers

Which equation is correct for polyprotic acids?

Ka total=K1+K2+K3 (A) Signup and view all the answers

Which expressions are correct for the relationship between Ka, Kb, and Kw?

pKa · pKb = 14 (D) Signup and view all the answers

Which expressions are correct for Kw, [H+], and [OH–]?

-lgKw = (–lg[H+] ) – (–lg[OH–] ) (C) Signup and view all the answers

If Ka for an acid is 10–5, what is the pKb value of its conjugate base?

9 (B) Signup and view all the answers

If pKa values of four acids at 25°C are given below, what is the pKa of the strongest acid?

2 (D) Signup and view all the answers

[OH–] ion concentration in a solution is 10^–4, what is the pH of the solution?

12 (D) Signup and view all the answers

If the pH of a solution is 4 and it increases up to 5, what should be the change in the H+ ion concentration?

Halved (C) Signup and view all the answers

What is the equation for calculating pH of a weak acid solution?

pH = 14 − 1/2 (pKa + lgCa) (A) Signup and view all the answers

What type of system allows transfer of neither matter nor energy to and from its surroundings?

None of the above (D) Signup and view all the answers

Which of the following is an example of a closed system?

Some amount of water present in equilibrium with its vapor in a closed and insulated beaker (D) Signup and view all the answers

Which type of system is the human body an example of?

An open system (B) Signup and view all the answers

Which of the following are state functions?

1, 3, 4 (C) Signup and view all the answers

What is a thermodynamic state function?

A quantity the value of which is independent on the path (D) Signup and view all the answers

Which of the following is not a state function?

q + w (B) Signup and view all the answers

According to Hess's law, the thermal effects of a reaction depend on...

initial and final conditions of the reacting substances (B) Signup and view all the answers

Enthalpy changes of a reaction depend on...

2, 3, 4 (B) Signup and view all the answers

The enthalpy change of a reaction does not depend on the...

the number of intermediate steps for converting reactants into products (B) Signup and view all the answers

The enthalpies of the elements in their standard states are...

zero at 298 K (B) Signup and view all the answers

The enthalpy of formation of a compound from the elements ...

is either positive or negative (A) Signup and view all the answers

The heat of neutralization is constant when dilute solution of...

strong acid and strong base react (D) Signup and view all the answers

Which of the following neutralization reactions have the highest neutralization heat?

NH4OH and HCl (B) Signup and view all the answers

Which of the following is NOT correct?

The free energy of a system in any spontaneous process tends to decrease (D) Signup and view all the answers

When ice melts into water, entropy…

increases (C) Signup and view all the answers

Which of the following expressions is correct?

$1/2 P P nRTln ΔS=$ (B) Signup and view all the answers

What happens to the concentration of OH– when NH4Cl is added to a solution of NH4OH?

Decreases (B) Signup and view all the answers

Study Notes

A closed system is a system where transfer of matter is not possible, but transfer of energy to and from surroundings ispossible.
Examples of closed systems: some amount of hot water enclosed in a closed container.
Human body is an example of an open system, as it exchanges matter with the environment.
State functions are thermodynamic potentials that only depend on the current state of a system and not on the path taken to reach that state.
Examples of state functions: internal energy (ΔE), entropy (S), and enthalpy (H).
A thermodynamic state function is a quantity whose value is independent of the path taken to reach that state.
Heat of compound formation is the heat absorbed or released when one mole of a compound is formed from its elements in their standard states.
Enthalpy changes of a reaction depend on the conditions of the reaction, initial and final concentration, and the physical state of reactants and products.
For an exothermic reaction, the heat released is a negative value.
Entropy is a measure of disorder and increases when a system undergoes a spontaneous change.
The Gibbs free energy (G) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
An endothermic reaction is a reaction that absorbs energy from its surroundings, and for it to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
The criteria for spontaneity of a reaction: ΔG < 0.
Gibbs free energy, enthalpy, and entropy are related through the legacy of Gibbs, specifically through the equation G = H - TS.
Gibbs free energy is the maximum reversible work that can be done by a system at constant temperature and pressure.
For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
Internal energy (ΔE) is a state function that measures the maximum reversible work that can be done by a system at constant temperature and volume.
Enthalpy (H) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
Entropy (S) is a thermodynamic potential that measures the disorder or randomness of a system.
Hess's law deals with the relationship between heat changes that occur during a series of reactions.
The thermal effects of a reaction depend on the initial and final conditions of the reacting substances.
Enthalpy changes of a reaction are independent of the number of intermediate steps involved in the reaction.
Heat of compound formation is the heat absorbed or released when one mole of a compound is formed from its elements in their standard states.
The enthalpy change of a reaction is the difference in enthalpy between the reactants and the products.
The heat of neutralization is the heat absorbed or released when an acid and a base react to form a salt and water.
The heat of neutralization is constant for dilute solutions of strong acids and strong bases.
When ice melts, the entropy increases due to the increase in the number of translationally disordered water molecules.
The equation for entropy change (ΔS) in terms of the entropy change of the system (ΔSsys) and the entropy change of the surroundings (ΔSsurr) is: ΔS = ΔSsys + ΔSsurr > 0.
The Gibbs free energy change (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
For a spontaneous reaction, ΔG is negative, which means that the enthalpy change is less than the product of the temperature (T) and entropy change (ΔS) of the reaction.
The criteria for spontaneity of a reaction are: ΔG < 0.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The change in Gibbs free energy (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
For a reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
The change in Gibbs free energy (ΔG) for a reaction is the difference between the enthalpy change (ΔH) and the product of the temperature (T) and entropy change (ΔS) of the reaction.
For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
The Gibbs free energy change (ΔG) for a reaction is given by the equation: ΔG = ΔH - TΔS.
For an endothermic reaction to proceed spontaneously, the entropy change (ΔS) must be positive and greater than the enthalpy change (ΔH).
The change in Gibbs free energy (ΔG) for a reaction is the difference between the enthalpy change (ΔH) and the product of the temperature (T) and entropy change (ΔS) of the reaction.
The Gibbs free energy change (ΔG) is a thermodynamic potential that measures the maximum reversible work that can be done by a system at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work that can be done by the reaction at constant temperature and pressure.
The Gibbs free energy change (ΔG) for a reaction is a measure of the maximum reversible work

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Test your knowledge of weak electrolyte dissociation with this quiz. Answer questions about factors affecting dissociation constant (K) and the dissociation degree (α) of weak electrolytes.