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Equilibrium between Solid Calcium Carbonate and Solvated Ions

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Equilibrium between Solid Calcium Carbonate and Solvated Ions

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Questions and Answers

What does the equilibrium equation between solid calcium carbonate and its solvated ions describe?

The concentration of calcium ions in a saturated solution

The ratio of solid calcium carbonate to its ions in solution

The establishment of equilibrium in an aqueous solution with calcium and carbonate ions (correct)

The precipitation of calcium carbonate

What happens if the reaction quotient, Qsp, is less than the solubility product, Ksp?

No precipitation will occur (correct)

Equilibrium is established

Precipitation will occur

The solution becomes unsaturated

In which direction does the reaction proceed if Qsp is greater than Ksp?

Reverse direction (precipitation will occur) (correct)

The solution becomes unsaturated

Equilibrium is established

Forward direction (no precipitation occurs)

What is the significance of comparing Qsp to Ksp when predicting precipitation?

It allows for prediction of the direction of the reaction Signup and view all the answers

What happens if the ion concentrations yield a reaction quotient equal to the solubility product?

Equilibrium is established Signup and view all the answers

Why is it necessary for Qsp to exceed Ksp for precipitation to occur?

To ensure supersaturation and drive the reaction towards precipitation Signup and view all the answers

How does the comparison of Qsp to Ksp help predict whether precipitation will occur?

By evaluating if ion concentrations surpass the level for precipitation Signup and view all the answers

What happens if Qsp is less than Ksp in a solubility equilibrium?

No precipitate forms as the saturation level is not exceeded Signup and view all the answers

Equilibrium between Solid Calcium Carbonate and Solvated Ions

Choose a study mode

Podcast

Questions and Answers

What does the equilibrium equation between solid calcium carbonate and its solvated ions describe?

What happens if the reaction quotient, Qsp, is less than the solubility product, Ksp?

In which direction does the reaction proceed if Qsp is greater than Ksp?

What is the significance of comparing Qsp to Ksp when predicting precipitation?

What happens if the ion concentrations yield a reaction quotient equal to the solubility product?

Why is it necessary for Qsp to exceed Ksp for precipitation to occur?

How does the comparison of Qsp to Ksp help predict whether precipitation will occur?

What happens if Qsp is less than Ksp in a solubility equilibrium?

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