Solubility Equilibria

Question 1

Solute + Salt =

Answer 1

process of dissolution

Question 2

hydration

Answer 2

When an ion is surrounded and stabilized by a shell of solvent (ie: water)

Question 3

precipitation

Answer 3

when ions come together to form a solid, solid falls out of solution and forming ion crystals

Question 4

electro static interactions

Question 5

what needs to happen in order for precipitation to form

Answer 5

electrostatic interactions of ionic crystal must be stronger than the forces of hydration

Question 6

spectator ions

Answer 6

when ions do not take part in a reaction and are not directly involved

Question 7

solubility equilibria

Answer 7

when the rate of dissolution = the rate of precipitation, therefore the reactants and products are constant, amount of solid is constant, forms a saturated solution

Question 8

Ksp

Answer 8

equilibrium constant, indicates how much salt will dissolve

Question 9

what happens when Ksp (equilibrium constant) is less than one

Answer 9

indicates salt is NOT very soluble

Question 10

what happens when Ksp (equilibrium constant) is more than one

Answer 10

indicates salt is soluble and dissolves easily in water

Question 11

solubility of a substance refers to

Answer 11

amount of solid that dissolves to form a saturated solution

Question 12

Units for solubility

Answer 12

g/L

Question 13

molar solubility

Answer 13

refers to the # of moles that dissolve to form 1L of saturated solution

M = mol/L

Question 14

in order to compare Ksp values what needs to happen

Answer 14

reaction needs to produce the same number of ions

Question 15

common ion effect

Answer 15

when the solubility of less soluble salt is decreased by the presence of a common ion

Question 16

pH and solubility

Answer 16

decreasing pH and increasing solubility of a slightly soluble salt happens whenever the slightly soluble salt contains a basic anion

Question 17

what happens to molar solubility when pH decreases

Answer 17

increases making solid more soluble to balance equilibrium and reduce stress

Question 18

What happens to Ksp when pH decreases

Answer 18

stays the same

Question 19

CASH-N-GIA

Answer 19

a mneumonic for solubility rules

usually when these are a part of a reaction they are more soluble

chlorates
acetates
sulfates
halides (not F-)
nitrates
group 1 metals
ammonium

Question 20

exception to group 1 metals that are not as soluble

Answer 20

Pb2+, Hg2+, Ag+, when attached to soluble compounds reduces solubility (HAPpy)

Question 21

exception to solubility rules

Answer 21

calcium (Ca2+), barium (Ba2+), Strontium (Sr2+) group 2 metals REDUCE solubility

Question 22

what happens when you add more of a product to a saturated solution

Answer 22

causes a precipitate to form

Question 23

how to find molar solubility given the Ksp

Answer 23

divide the exponent by the # of ions to give you a rough idea of the magnitude of the negative exponent (ie: Y(OH)3 has 4 ions Y + 3OH and the Ksp = 1.0 x 10^-22 - so you would divide -22/4 which is ~ 5.5, the lower an exponent the lower molar solubility

IF EXPONENTS ARE CLOSE TO # of IONS FULL MATH SHOULD BE USED (ie: ICE table)