Solubility

Question 1

What is a solution?

Answer 1

A homogeneous mixture of two or more substances.

Question 2

True or False: A solute is the substance that is dissolved in a solution.

Answer 2

false

A solute is the substance that is dissolved in a solvent to create a solution

Question 3

Fill in the blank: The substance that does the dissolving in a solution is called the __________.

Answer 3

solvent

Question 4

What is the process of a solute dissolving in a solvent called?

Answer 4

Dissolution

Question 5

Which of the following is an example of a solid solute: a) Salt b) Water c) Air?

Answer 5

a) Salt

Question 6

What type of solution has the maximum amount of solute dissolved at a given temperature?

Answer 6

Saturated solution

Question 7

Multiple choice: Which factor does NOT affect the rate of dissolution? a) Temperature b) Surface area c) Color of the solute

Answer 7

c) Color of the solute

Question 8

What is the term for a solution that contains less solute than it can hold at a given temperature?

Answer 8

Unsaturated solution

Question 9

True or False: All solutes can dissolve in any solvent.

Answer 9

False

Question 10

What is the term for a solution with more solute than can be dissolved at a given temperature?

Answer 10

Supersaturated solution

Question 11

Fill in the blank: The ability of a solute to dissolve in a solvent is called __________.

Answer 11

solubility

Question 12

What is the main factor that determines the solubility of a substance?

Answer 12

The nature of the solute and solvent.

Question 13

Multiple choice: Which type of solute generally dissolves well in polar solvents? a) Non-polar solutes b) Ionic compounds c) Metals

Answer 13

b) Ionic compounds

Question 14

What happens to the solubility of most solids as temperature increases?

Answer 14

It generally increases.

Question 15

True or False: Gases are usually more soluble in liquids at higher temperatures.

Answer 15

False

Question 16

What is the term for the measure of how much solute can dissolve in a solvent at a specific temperature?

Answer 16

Solubility

Question 17

Fill in the blank: A __________ solution contains dissolved solute in a concentration that is below its saturation point.

Answer 17

dilute

Question 18

What is the process called when a solid solute forms crystals as it comes out of a saturated solution?

Answer 18

Crystallization

Question 19

Multiple choice: Which of the following increases the solubility of a gas in a liquid? a) Increasing temperature b) Decreasing pressure c) Increasing pressure

Answer 19

c) Increasing pressure

Question 20

True or false: a rxn is exothermic when the new solvent/solute interaction is weaker than the solvent/solute molecules on their own

Answer 20

false

True or false: a rxn is exothermic when the new solvent/solute interaction is stronger than the solvent/solute molecules on their own endothermic. the rxn is

Question 21

solubility

Answer 21

the max amount of solute that can be dissolved at a specific temp

Question 22

True or false: nitrate, acetate, sulfite, and alkali metals are all water soluble

Answer 22

false

nitrate, acetate, ammonium, and alkali metals are all water soluble

Question 23

What is the definition of solubility product (Ksp)?

Answer 23

The solubility product (Ksp) is the equilibrium constant for a saturated solution of a sparingly soluble ionic compound.

Question 24

True or False: The solubility product constant is temperature dependent.

Answer 24

True

Question 25

Fill in the blank: The solubility product expression for AgCl is _____.

Answer 25

Ksp = [Ag+][Cl-]

Question 26

What does a higher Ksp value indicate about a compound's solubility?

Answer 26

A higher Ksp value indicates greater solubility of the compound.

Question 27

Which of the following compounds has the highest Ksp? a) AgCl b) BaSO4 c) CaF2

Answer 27

c) CaF2

Question 28

What happens to the solubility of a salt when a common ion is added?

Answer 28

The solubility of the salt decreases due to the common ion effect.

Question 29

True or False: Ksp can be used to predict whether a precipitate will form in a solution.

Answer 29

True

Question 30

Short answer: What is the relationship between Ksp and the concentrations of ions in solution?

Answer 30

Ksp is equal to the product of the concentrations of the ions, each raised to the power of their coefficients in the balanced equation.

Question 31

Fill in the blank: The Ksp for calcium fluoride (CaF2) is expressed as Ksp = _____.

Answer 31

Ksp = [Ca2+][F-]^2

Question 32

What is the unit of Ksp?

Answer 32

Ksp has no units; it is a dimensionless quantity.

Question 33

Multiple choice: Which of the following factors does NOT affect Ksp? a) Temperature b) Pressure c) Concentration of ions

Answer 33

c) Concentration of ions

Question 34

True or False: Ksp values can be used to compare the solubility of different salts.

Answer 34

True

Question 35

What is the impact of increasing temperature on the Ksp of an endothermic dissolution process?

Answer 35

Increasing temperature typically increases the Ksp for an endothermic dissolution process.

Question 36

Short answer: Describe the common ion effect.

Answer 36

The common ion effect is the decrease in solubility of a salt when a common ion is added to the solution.

Question 37

Fill in the blank: If the Ksp of a salt is 1.0 x 10^-10, its solubility in mol/L is likely to be _____.

Answer 37

approximately 1.0 x 10^-5

Question 38

True or False: The solubility product can be determined experimentally.

Answer 38

True

Question 39

Multiple choice: Which of the following is a correct expression for Ksp? a) Ksp = [A]^a[B]^b c) Ksp = [C]^c[D]^d b) Ksp = [A]^x[B]^y

Answer 39

b) Ksp = [A]^x[B]^y

Question 40

True or false: if Qsp is < Ksp, the solution is supersaturated

Answer 40

false ## Footnote if Qsp is < Ksp, the solution is unsaturated

Question 41

if Qsp is > Ksp, the solution is A.) unsaturated, B.) supersaturated, C.) normally saturated, D.) at equilibrium

Answer 41

B.) supersaturated

Question 42

What is a complex ion?

Answer 42

A complex ion is a charged species consisting of a central metal atom or ion bonded to one or more molecules or ions, known as ligands.

Question 43

True or False: Complex ions can only form with transition metals.

Answer 43

False: While complex ions are commonly formed with transition metals, they can also form with main group metals.

Question 44

Fill in the blank: A ligand that donates two pairs of electrons to a metal ion is called a __________ ligand.

Answer 44

bidentate

Question 45

What is the coordination number in complex ion formation?

Answer 45

the number of ligand donor atoms that are bonded to the central metal ion in a complex.

Question 46

Which of the following is an example of a monodentate ligand? (a) Ethylenediamine (b) Ammonia (c) Oxalate

Answer 46

b) Ammonia

Question 47

What type of bond is primarily formed between the central metal ion and the ligands in a complex ion?

Answer 47

Coordinate covalent bond

Question 48

Short Answer: Name one factor that affects the stability of a complex ion.

Answer 48

The nature of the metal ion, the type of ligands, or the overall charge of the complex.

Question 49

True or False: Chelate complexes are generally more stable than non-chelate complexes.

Answer 49

True

Question 50

What is the role of ligands in complex ion formation?

Answer 50

Ligands act as electron pair donors that coordinate to the central metal ion, influencing the properties and stability of the complex.

Question 51

Multiple Choice: Which of the following ligands is capable of forming a chelate complex? (a) Water (b) Ethylenediamine (c) Chloride

Answer 51

b) Ethylenediamine