Ksp Mastery Quiz(Unit 6)

What is solubility?

The measurement of how much solute can mix in solvent( in grams solute per 100 mL of water)

Unsaturated solution can hold _____ solute in solution before solids settle in beaker

more solute(can continue adding)

Saturated solution _____ _____ more solute in solution(solids immediately settle in beaker)

CANNOT hold more

Molar solubility

(x when solving ICE table) represents the maximum concentration of ions a solution can have and still remain in aqueous phase (otherwise, solid will begin to form)

on the graph of molar solubility, below the line represents

unsaturated solution(has not reached capacity yet, line is capacity for amount of solute that can be added)

On the graph of molar solubility, above the line represents

saturated solution(no more solute can be added as it will form precipitate)

What is used to measure solubility?

Ksp

Ksp > > 1 indicates

substance has high solubility

KSp < < 1 indicates

substance has low solubility

Even “insoluble” ionic compounds _____ a tiny amount

dissociate

Ksp = (equation)

[products]/[reactants]; excludes solids and pure liquids

How do you separate mixtures?

Due to different Ksp values, adding a solution to a beaker containing two types of ions will result in one ion(the one with the higher Ksp value) creating solid precipitate first, and the other beginning to do so once a different volume of solution has been added. This allows one to separate some solid form of one ion from a solution containing two types of ions

Fractional precipitation

formation of precipitation at different rates in a solution

What do you do to the concentration of an ion in an ice table when the solution added to the compound contains the ion as well(given molarity of solution)?

Add the molarity to the x expression of the ion as there is already some of the ion present in the solution before the reaction takes place