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The solubility product constant (Ksp) is defined as:
a) The product of the concentrations of the ions
b) The sum of the concentrations of the ions
c) The difference between the concentrations of the ions
d) The ratio of the concentrations of the ions
Which of the following is true for a slightly soluble salt at equilibrium?
a) The ionic product is greater than Ksp
b) The ionic product is less than Ksp
c) The ionic product is equal to Ksp
d) The ionic product is zero
For a salt AB, the Ksp expression is:
a) [A⁺][B⁻]²
b) [A⁺]²[B⁻]
c) [A⁺][B⁻]
d) [A⁻][B⁺]
If the concentration of one ion in a saturated solution of a slightly soluble salt is doubled, the concentration of the other ion will:
a) Double
b) Halve
c) Quadruple
d) Remain unchanged
Which of the following salts has the highest solubility product (Ksp)?
a) AgCl
b) PbSO₄
c) CaF₂
d) BaSO₄
The solubility of a salt increases if:
a) A common ion is added
b) Temperature is increased
c) pH is decreased
d) pH is increased
The presence of a common ion will:
a) Increase the solubility of a salt
b) Decrease the solubility of a salt
c) Have no effect on the solubility of a salt
d) Increase the Ksp value
For the salt PbCl₂, the Ksp expression is:
a) [Pb²⁺]²[Cl⁻]
b) [Pb²⁺][Cl⁻]²
c) [Pb⁺][Cl⁻]²
d) [Pb²⁺][Cl⁻]
The solubility of calcium phosphate (Ca₃(PO₄)₂) in water can be determined using:
a) The pH of the solution
b) The Ksp value
c) The concentration of PO₄³⁻ ions
d) The concentration of Ca²⁺ ions
If Qsp < Ksp for a slightly soluble salt, the solution is:
a) Saturated
b) Unsaturated
c) Supersaturated
d) Precipitating
The solubility product of BaSO₄ is affected by:
a) Pressure
b) Volume
c) Temperature
d) Presence of a common ion
In a solution containing a common ion, the solubility of a salt is:
a) Higher
b) Lower
c) Unchanged
d) Variable
The addition of NaCl to a solution of AgCl will:
a) Increase the solubility of AgCl
b) Decrease the solubility of AgCl
c) Not affect the solubility of AgCl
d) Precipitate NaCl
For the salt Ag₂CO₃, the Ksp expression is:
a) [Ag⁺][CO₃²⁻]
b) [Ag⁺]²[CO₃²⁻]
c) [Ag⁺][CO₃⁻]
d) [Ag⁺]²[CO₃⁻]
When the ionic product exceeds Ksp, the solution is:
a) Saturated
b) Unsaturated
c) Supersaturated
d) At equilibrium
The addition of NH₄Cl to a solution containing NH₄OH and Mg²⁺ will:
a) Increase the solubility of Mg(OH)₂
b) Decrease the solubility of Mg(OH)₂
c) Precipitate MgCl₂
d) Have no effect on Mg(OH)₂ solubility
Which of the following is a common ion effect?
a) Increase in solubility due to a decrease in pH
b) Decrease in solubility due to the presence of a common ion
c) Increase in solubility due to the addition of a complexing agent
d) Decrease in solubility due to an increase in temperature
For the salt CaF₂, the Ksp expression is:
a) [Ca²⁺][F⁻]²
b) [Ca⁺][F⁻]²
c) [Ca²⁺]²[F⁻]
d) [Ca²⁺][F⁻]
The solubility of PbSO₄ in water will decrease if:
a) Na₂SO₄ is added
b) HCl is added
c) Temperature is increased
d) Pressure is increased
If a solution is supersaturated with respect to a slightly soluble salt, then:
a) Precipitation will occur
b) No precipitation will occur
c) The solution is at equilibrium
d) The solution is unsaturated
The addition of a common ion will shift the equilibrium:
a) To the left, decreasing solubility
b) To the right, increasing solubility
c) To the right, decreasing solubility
d) To the left, increasing solubility
The Ksp of Ag₂CrO₄ is:
a) [Ag⁺][CrO₄²⁻]
b) [Ag⁺]²[CrO₄²⁻]
c) [Ag⁺][CrO₄⁻]
d) [Ag⁺]²[CrO₄⁻]
If a slightly soluble salt is dissolved in a solution containing a common ion, the Ksp:
a) Remains constant
b) Increases
c) Decreases
d) Depends on the concentration of the common ion
The Ksp of a salt at a particular temperature is:
a) Constant
b) Variable
c) Dependent on the concentration of ions
d) Dependent on pressure
Which of the following factors does NOT affect the value of Ksp?
a) Temperature
b) Concentration of ions
c) Common ion effect
d) Presence of a complexing agent
The Ksp of Mg(OH)₂ is:
a) [Mg²⁺][OH⁻]
b) [Mg⁺][OH⁻]
c) [Mg²⁺][OH⁻]²
d) [Mg²⁺]²[OH⁻]
When the solubility of a salt decreases due to the addition of a common ion, this is known as:
a) Common ion effect
b) Le Chatelier’s principle
c) Ion pairing
d) Complex formation
Which of the following salts has the lowest Ksp value?
a) AgCl
b) CaF₂
c) BaSO₄
d) PbSO₄
The solubility of Ca(OH)₂ decreases when:
a) NaOH is added
b) Temperature is increased
c) Pressure is decreased
d) CaCl₂ is added
The product of the ion concentrations raised to the power of their coefficients in the balanced equation is called:
a) Ksp
b) Ionic product
c) Solubility
d) Molarity
If the concentration of one ion is known, the concentration of the other ion in a saturated solution can be determined using:
a) Molarity
b) pH
c) Ksp
d) Pressure
In a saturated solution of Ag₂SO₄, if the concentration of Ag⁺ ions is doubled, the concentration of SO₄²⁻ will:
a) Double
b) Halve
c) Quadruple
d) Remain unchanged
The presence of a complexing agent will:
a) Increase the solubility of a salt
b) Decrease the solubility of a salt
c) Have no effect on the solubility of a salt
d) Increase the Ksp value
The solubility product constant (Ksp) for AgI is:
a) [Ag⁺][I⁻]²
b) [Ag⁺]²[I⁻]
c) [Ag⁺][I⁻]
d) [Ag⁺]²[I⁻]²
The Ksp value is typically given in:
a) Molarity (M)
b) Mol/L
c) L/mol
d) Unitless
When a salt has a low Ksp value, it indicates:
a) High solubility
b) Low solubility
c) No solubility
d) Supersaturation
The addition of a strong acid to a solution containing a slightly soluble salt will:
a) Increase the solubility if the anion is a weak base
b) Decrease the solubility if the anion is a weak base
c) Not affect the solubility
d) Increase the Ksp value
If the ionic product of a salt is less than its Ksp, the solution is:
a) Saturated
b) Unsaturated
c) Supersaturated
d) Precipitating
The solubility of Ag₂SO₄ in water will increase if:
a) H₂SO₄ is added
b) AgNO₃ is added
c) NH₄OH is added
d) Temperature is decreased
In a saturated solution of a slightly soluble salt, if the concentration of one ion is decreased, the concentration of the other ion will:
a) Increase
b) Decrease
c) Remain the same
d) Be halved
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