8 Questions
What does the equilibrium equation between solid calcium carbonate and its solvated ions describe?
The establishment of equilibrium in an aqueous solution with calcium and carbonate ions
What happens if the reaction quotient, Qsp, is less than the solubility product, Ksp?
No precipitation will occur
In which direction does the reaction proceed if Qsp is greater than Ksp?
Reverse direction (precipitation will occur)
What is the significance of comparing Qsp to Ksp when predicting precipitation?
It allows for prediction of the direction of the reaction
What happens if the ion concentrations yield a reaction quotient equal to the solubility product?
Equilibrium is established
Why is it necessary for Qsp to exceed Ksp for precipitation to occur?
To ensure supersaturation and drive the reaction towards precipitation
How does the comparison of Qsp to Ksp help predict whether precipitation will occur?
By evaluating if ion concentrations surpass the level for precipitation
What happens if Qsp is less than Ksp in a solubility equilibrium?
No precipitate forms as the saturation level is not exceeded
Learn about the equilibrium relationship between solid calcium carbonate and its solvated ions in aqueous solutions. Explore how the equilibrium constant Ksp is calculated and its significance in predicting precipitation outcomes. Test your understanding with a quiz on this topic.
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