Unit 3- Solubility Flashcards
Define the Solubility Product
The equilibrium constant for the equilibrium between a slightly soluble ionic solute and a solution of its ion is called the solubility product (Kip) of the solid.
Do solids appear in the Ksp Expression?
NO; it follows the same rules as the Kc. (Only solute and gaseous species are included)
What does the value of Ksp represent?
How soluble a compound is; the more close it is to one and the higher it is than 1, the more soluble it is than a value that is less than 1.
Define Molar Solubility
The measure as moles of dissolved solute per liters of solution.
Define Gram Solubility
Solubility can be expressed in terms of mass per unit volume. For example, grams per liter.
In problem that involve solving for the prediction of precipitation, what must be done?
It is the same procedure used in unit 1 (predicting the direction of the forward and reverse reaction). COMPARE THE VALUE OF Q to KSP
Given the KSP for two different substances, how do you know which one will precipitate first?
The value with the LOWER KSP will form; the lower the value of KSP, the less soluble the substance is.
In terms of the value of Q and Ksp, when does the precipitate form?
The precipitate forms when the value of Q=KSP
What is the relationship between Q and Ksp for an unsaturated solution?
Q<Ksp
What is the relationship between Q and Ksp for a saturated solution?
Q= Ksp (ionic product is equal to the solubility product)
How do you determine what type of substance will be more soluble in acidic solution compared to pure water?
The compounds in which anions come from WEAK ACIDS would be more soluble in acidic solution rather than in pure water; hence, any of the anions coming from the strong acids (HI, HBr,HCl, HSO4, HNO3, HCLO4) would be LESS SOLUBLE in an acidic solution.
What is the difference between a saturated solution and an unsaturated solution?
A saturated solution is a solution that contains the maximum amount of solute and is capable of dissolving; an unsaturated solution is a solution that contains less than the maximum capacity of the solute and is capable of being dissolved.
