Solutions, Electrolytes, and Chemical Properties

Flashcards related to solutions, electrolytes and chemical properties.

Electrolytic solution

A solution that conducts electricity.

Electrolyte

A substance that, when added to water, conducts electricity.

Strong Electrolyte

100% ions present in a solution.

Weak Electrolyte

Some ions present in a solution.

Non-electrolyte

No ions present in a solution.

Ionic Compounds

Ionic compounds, metals, and nonmetals attraction.

Ionic Bond

Positive and negative ions don't share, they transfer.

Solvable

Ionic compound that is solvable.

Insolvable

Ionic compound that is not solvable.

Electrolytic Nature

Ionic compounds are strong or weak electrolytes depending on if they are soluble or not.

Arrhenius Acid

A substance that produces H3O+ (hydronium ion) when added to water.

Strong Acids (6)

HCI, HBr, HI, HClO4, HNO3, H2SO4

Arrhenius Base

A substance that produces /OH (hydroxide ions) when added to water.

Weak Bases

All molecular bases.

Strong Base

Solvable ionic compounds where hydroxide ion is strong.

Dissolution

The process of ionic compounds dissolving in water.

Metal Ions

Metal ions lose electrons to make a +Gp# charge.

Nonmetal Ions

Make a negative (8-Gp#) charge.

Polyatomic Ions

Need to memorize formula and charge.

Ionic Compound Charge Balance

Total amount of +ions = total amount of –ions.

Electrolytic Nature of Ionic Compounds

Strong Electrolytes (→) or Weak electrolytes (⇌) depending on if soluble or not (physical properties).

Soluble Ionic Compounds Rule 1

All sodium (Na+), potassium (K+), and ammonium (NH4 +) salts are soluble.

Soluble Ionic Compounds Rule 2

All nitrate (NO3 -), acetate (CH3CO2 -), chlorate (ClO3 -), and perchlorate (ClO4 -) salts are soluble.

Soluble Ionic Compounds Rule 3

All chloride (Cl-), bromide (Br-), and iodide (I-) salts are soluble — EXCEPT those containing: lead, silver, or mercury (I) (Pb2+, Ag+, Hg2 2+) which are NOT soluble.

Soluble Ionic Compounds Rule 4

All sulfate (SO4 2-) salts are soluble — EXCEPT those containing: calcium, silver, mercury (I), strontium, barium, or lead (Ca2+, Ag+, Hg2 2+, Sr2+, Ba2+, Pb2+) which are NOT soluble.

Not Soluble Ionic Compounds Rule 5

Hydroxide (OH-) and oxide (O2-) compounds are NOT soluble — EXCEPT those containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble.

Not Soluble Ionic Compounds Rule 6

Sulfide (S2-) salts are NOT soluble — EXCEPT those containing: sodium, potassium, ammonium, or barium (Na+, K+, NH4 +, Ba2+) which are soluble.

Not Soluble Ionic Compounds Rule 7

Carbonate (CO3 2-) and phosphate (PO4 3-) salts are NOT soluble — EXCEPT those containing: sodium, potassium, or ammonium (Na+, K+, NH4 +) which are soluble.

Electrolytes

Creates a solution that conducts electricity when added to water.

Strong electrolytes

Solutions strongly conduct electricity—solutes have 100% been converted into ions.

Weak electrolytes

Solutions weakly conduct electricity—a small fraction of solute particles have been converted into ions.

Nonelectrolytes

Solutions don’t conduct electricity—solutes produce no ions in water.

Molarity

Moles of solute per Liter of solution.

Molality

Moles of solute per kg of solvent.

Mole Fraction

Mole of component interested in per total number of moles present (solute + solvent).

Mass (weight) percent or percent by weight

Mass fraction x 100%.

Solution

A homogeneous mixture, solvent vs solute, amounts can vary because it is a mixture.

Concentration

How close together the solute particles are in a solution, reflects amount of solute per some characteristic of the solution.

Given (GUESS C method)

Assign variables to numbers given, identify roles, identify balanced chemical equation.

Unknown (GUESS C method)

What are you looking for?

Equation (GUESS C method)

Do you have an equation linking givens and unknown?

Setup (GUESS C method)

Write down! Convince yourself of steps.

Solve (GUESS C method)

Now get calculator.

Check (GUESS C method)

Is answer reasonable? Units? Significant digits?

Hydrogen bonding

The attraction between a N, O or F to a H that is bonded to a N, O or F.

Dipole-dipole forces

The attraction between polar molecules.

London dispersion forces

The attraction between temporary/induced dipoles, strength increases with increasing mass (number and polarizability of electrons).

"Like dissolves like"

Substances with similar strength of IMF’s will be able to mix together, or, polar solvents dissolve polar solutes, nonpolar solvents dissolve nonpolar solutes.

Intramolecular Force

Strong force within a molecule.

Intermolecular Force

Force between molecules.