WorksheetsCalculating Ksp
Total questions: 20
Worksheet time: 39mins
According to Le Chatelier’s Principle, what happens to the position of the equilibrium if magnesium sulfate is added?
With the shift in the position of the equilibrium from question 1, will the solubility of calcium sulfate increase or decrease?
What is the concentration of the silver ion if Ag₂CrO₄(s) is dissolved in water?
(read additional information on Mrs. Zaepfel's slide)
Type in using the E. For example, 1.23 x 104 M Ag+ would look like:
1.23E4 M Ag+
(a)
4.) What is the concentration of the silver ion if Ag₂CrO₄(s) is dissolved in 1.00 M Na₂CrO₄?
(a)
(read additional information on Mrs. Zaepfel's slide)
If Q < Ksp,
If Q > Ksp,
If Q = Ksp,
Write the solubility product constant expression for:
AgCl
(a)
Write the solubility product constant expression for:
PbI₂
(a)
Write the solubility product constant expression for:
BaSO₄
(a)
Write the solubility product constant expression for:
ZnCO₃
(a)
Which salt is most soluble?
Which salt is least soluble?
What is the solubility in moles/liter of AgBr if the Ksp = 5.0 x 10⁻¹³?
(a)
If the solubility of Li₂CO₃ = 0.15 moles/liter, what is its Ksp at this temperature?
(a)
What is the solubility in moles/liter, of PbI₂ if the Ksp = 8.5 x 10⁻⁹?
(a)
If the solubility of Ag₂CrO₄ = 7.2 x 10⁻⁵ moles / L, what is the Ksp?
(a)
How many moles of AgCl will dissolve in 500. mL of water if the Ksp = 1.7 x 10⁻¹⁰?
(a)
Calculate [Ag¹⁺] in this saturated solution.
(a)
What mass of Na₂SO₄ must be added to 0.500 L of the solution to decrease [Ag¹⁺] to 4.0 x 10⁻³ M?
(This is connected to the previous question)
(a)
