Calculating Ksp

According to Le Chatelier’s Principle, what happens to the position of the equilibrium if magnesium sulfate is added?

• The position of the equilibrium will shift to the left with the addition of magnesium sulfate.
• The position of the equilibrium will shift to the right with the addition of magnesium sulfate.

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SPQ-5.A

With the shift in the position of the equilibrium from question 1, will the solubility of calcium sulfate increase or decrease?

• Addition of magnesium sulfate (a strong electrolyte) shifts the equilibrium, increasing the solubility of the calcium sulfate.
• Addition of magnesium sulfate (a strong electrolyte) shifts the equilibrium, decreasing the solubility of the calcium sulfate.

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SPQ-5.A

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+

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SPQ-5.A

4.) What is the concentration of the silver ion if Ag₂CrO₄(s) is dissolved in 1.00 M Na₂CrO₄?

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SPQ-5.A

(read additional information on Mrs. Zaepfel's slide)

If Q < Ksp,

• the reaction will proceed in the forward direction, creating more dissolved ions.
• the reaction will proceed in the reverse direction, creating more precipitated solid.
• the reaction is at equilibrium.

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SPQ-5.A

If Q > Ksp,

• the reaction will proceed in the forward direction, creating more dissolved ions.
• the reaction will proceed in the reverse direction, creating more precipitated solid.
• the reaction is at equilibrium.

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SPQ-5.A

If Q = Ksp,

• the reaction will proceed in the forward direction, creating more dissolved ions.
• the reaction will proceed in the reverse direction, creating more precipitated solid.
• the reaction is at equilibrium.

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SPQ-5.A

Write the solubility product constant expression for:

AgCl

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SPQ-5.A

Write the solubility product constant expression for:

PbI₂

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SPQ-5.A

Write the solubility product constant expression for:

BaSO₄

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SPQ-5.A