(Ci) Chapter 9: Solutions

Front 1

Solutions

Back 1

A homogeneous mixture of two or more substance that combine in the same phase. These are usually liquids.

Front 2

Can metals form solutions?

Back 2

Yes. Metal alloys are a combination of different metals to form a single type of metal.

Front 3

Name for a combination of gasses

Back 3

A combination of gasses is known as a mixture

Front 4

How do the particles of a solute interact with the solvent?

Back 4

The particles of a solute interact with the solvent through the dipole-dipole interactions and hydrogen bonding

Front 5

Solvation

Back 5

The electrostatic interaction between a solute and a solvent. This involves the breaking down of the solute bonds and the formation of bonds between the solute and the solvent

Front 6

What type of reaction is it when the solute-solvent bonds are stronger than the solute-solute bonds and the solvent-solvent bonds?

Back 6

When this occurs it is an exothermic reaction.

Front 7

What happens to a gas that is dissolved in a liquid as the temperature is raised?

Back 7

As the temperature is raised, the gas becomes less soluble in the liquid.

Front 8

What type of reaction is it when the solute-solvent bonds are weaker than the solute-solute bonds and the solvent-solvent bonds?

Back 8

This is an endothermic reaction since energy must be supplied in order to make the new, weaker bonds.

Front 9

For an ideal solution, what is the enthalpy?

Back 9

The enthalpy of an ideal solution is 0

Front 10

Is spontaneity dependent upon enthalpy change?

Back 10

No. Whether a reaction is spontaneous or not depends on the change in gibbs free energy

Front 11

Components of the Gibbs Free Energy and whether a reaction will be spontaneous

Back 11

You need to look at the value of the entropy and the enthalpy of the reaction to see whether or not it will be a spontaneous reaction.

Front 12

Solubility

Back 12

The extent to which a solute will dissolve in a solvent. If a solvent cannot dissolve any more solute then the solution is said to be saturated and the solute will precipitate to the bottom.

Front 13

What is solubility governed by?

Back 13

Solubility is governed by thermodynamics and specifically the gibbs free energy function. if at a given temp the solute and solvent have a negative gibbs function then the solute will dissolve spontaneously. If it has a positive gibbs function then it will not dissolve spontaneously

Front 14

Solubility

Back 14

(Make sure to look this up) A few rules that govern the solubility of different compounds in aqueous solutions.

Front 15

Sodium Salts and Nitrate Salts

Back 15

Both of these salts are completely soluble in aqueous solutions

Front 16

How do you distinguish between ions of the same element but with different charges?

Back 16

For the ions that has the lesser charge, you add the -ous suffix and for the ions that have a larger charge you add the -ic suffix

Front 17

Naming monoatomic anions

Back 17

Simply drop the end of the name and add the suffix -ide. For example, hydride.

Front 18

How do you distinguish between oxyanions that have more or less oxygens?

Back 18

For oxyanions that have less oxygen add the suffix -ite (as in light) and for oxyanions with more oxygen add the suffix -ate.

Front 19

Naming a series of oxyanions

Back 19

(from least oxygens to most) hypochlorite - chlorite - chlorate - hyperchlorate.

Front 20

Formula for bicarbonate

Back 20

HCO3 -

Front 21

Oxidation state of alkali metals, alkaline earth metals, and halogens

Back 21

+1, +2, -1

Front 22

Electrolytes

Back 22

When ions dissociate in water, the increase the electrical conductivity of the water (or any solution for that matter). The great the dissociation of the ion the greater the electrical conductivity.

Front 23

Molarity

Back 23

Moles per liter of a solution

Front 24

Molality

Back 24

Moles per kilogram of solvent

Front 25

Dilution Equation

Back 25

MV = MV. Where m is the moles and V is the volume

Front 26

Where will the unit for molality be used?

Back 26

When you are calculating the freezing point depression or boiling point elevation

Front 27

What is the change in free energy of a system at equilibrium?

Back 27

The change in free energy of a system at equilibrium is 0.

Front 28

Ksp - Solubility product constant

Back 28

This is the equilibrium constant which is similar to the Keq. It measures the equilibrium constant of an ion dissolved in a solution.

Front 29

What do you leave out of the solubility product constant?

Back 29

You always leave out the solids that you are dealing with.

Front 30

Value of the Ksp

Back 30

The larger the Ksp the greater the solute will be dissolved in the solvent while the lower the Ksp the lower a solute will be dissolved in a solvent.

Front 31

I.P.

Back 31

This is the same thing as Q for equilibrium. The IP tells you where the reaction is in terms of saturation. As in there is a point at which the solution becomes saturated and the IP tells you where that given point is when compared to the Ksp

Front 32

Qsp > Ksp

Back 32

The solution is saturated and precipitation will occur

Front 33

Qsp < Ksp

Back 33

The solution is not saturated and the solute will dissolve

Front 34

Qsp = Ksp

Back 34

The solution will be at equilibrium

Front 35

For Ksp, where do the exponents come from?

Back 35

The exponents come from the stoichiometric coefficients of the equation

Front 36

Slightly soluble salt of the formula MX3

Back 36

For every salt of this type the Ksp = 27x^4 where x is the molar solubility

Front 37

Slightly soluble salt of the formula MX2

Back 37

For every salt of this type the Ksp = 4x^3 where x is the molar solubility

Front 38

Slightly soluble salt of the formula MX

Back 38

For every salt of this type the Ksp = x^2.

Front 39

Common Ion Effect

Back 39

If you have an ion that is already dissolved in a solution, then more of that same ion will be less soluble given that there is already some of the ion already present.

Front 40

How do you find the concentration of a dissolved ion in a solution if you are given a Ksp?

Back 40

Simply look to see what kind of compound it is (is it an MX^3, MX, ect). Once you establish which one of these it is then you know which equation it will be equal to. Simply set the Ksp to the right equation (from above) and solve for x which will give you the moral solubility.