Chem 130 Test 1

List the group 1A strong bases

LiOH, NaOH, KOH, RbOH, CsOH

Chloric acid

HClO3

Monoprotic

acids that contain one hydrogen molecule

Sulfuric Acid

H2SO4

Henry's Law

Sg=kPg

log(a^b)=

b(loga)

The presence of ions in a solution allows it to...

conduct electricity

If system gains entropy the value of ΔS will be...

positive

Give the Greek meaning for the word Metathesis.

"to transpose" or "to change partners"

mass percent=

(mass of solute/total mass) x 100

ppm=

(mass of solute/total mass) x 100 mg/kg or L

Determine the oxidation number of sulfur in SCl2

+2

Determine the oxidation number of sulfur in Na2SO3

+4

Determine the oxidation number of sulfur in H2S

-2

Rule #3 of oxidation numbers

-Oxygen has an oxidation number of -2 except for peroxide (-1) -Hydrogen is -1 when bonded to metal and +1 when bonded to nonmetal -Fluorine is always -1 -Other halogens have -1

Rule #4 of oxidation numbers

-The sum of the oxidation numbers in a neutral compound is 0 -The sum of the oxidation numbers in a polyatomic ion is the charge on the ion

Determine the oxidation number of sulfur in S8

0

Calculate the molarity of a solution made by dissolving 23.4g of Na2SO4 in enough water to form 125 mL of solution.

1.32 M

How many mL of 3.0 M H2SO4 are needed to make 450 mL of 0.10 M H2SO4?

15 mL H2SO4

How many grams of Na2SO4 are required to make 0.350 L of 0.500 M Na2SO4?

24.9 g Na2SO4

Rule #1 of activity series

Any metal may be oxidized by ions of a metal salt below it on the table

List the heavy group 2A strong bases

Ca(OH)2, Sr(OH)2, Ba(OH)2

Rule #1 of oxidation numbers

Elements in their elemental form have an oxidation number of zero.

Acids increase the ___ concentration when dissolved in water.

H+

Hydrobromic Acid

HBr

Hydrochloric Acid

HCl

Perchloric Acid

HClO4

Hydroiodic Acid

HI

Nitric Acid

HNO3

What dissolved species are present in a solution of KCN

K+ (aq) and CN- (aq)

What dissolved species are present in a solution of NaClO4

Na+ (aq) and ClO4- (aq)

Bases increase the ___ concentration when dissolved in water.

OH-

Rule #2 of activity series

Only the metals above hydrogen in the activity series may react with acids

OIL RIG

Oxidation is loss (of electrons) Reduction is gain (of electrons)

What Swedish physicist/chemist defined acids as substances that increase the concentration of H+ when dissolved in water?

S. A. Arrhenius

Rule #2 of oxidation numbers

The oxidation number of a monatomic ion is the same as its charge

What is formed when ions are mixed to create new insoluble compounds?

a precipitate

Redox Reaction

a reaction in which certain atoms undergo changes in oxidation states

Nonelectrolyte

a substance that may dissolve in water, but does form ions when it does

Electrolyte

a substance that readily forms ions when dissolved in water

Tripotic

acids that contain three hydrogen molecules

Diprotic

acids that contain two hydrogen molecules

Other than ___ and ___, molecular compounds tend to be...

acids, bases, nonelectrolytes

Which ionic compounds are strong electrolytes?

all ionic compounds are strong electrolytes

Which antacids produce gaseous products?

any containing CaCO3

Soluble ionic compounds tend to be...

electrolytes

Solution

homogeneous mixture of two or more pure substances

Solubility of gases ___ with increasing mass.

increase

Classify lead sulfate (PbSO4) as soluble or insoluble.

insoluble

What is Henry's Law constant?

k=3.4x10^-2 mol/L-atm

If 10^x=50, then...

log50 = x

log(axb)=

loga + logb

log(a/b)=

loga - logb

mole fraction=

moles of component/total moles

molality (m)=

moles of solute/kg solvent

molarity (M)=

moles of solute/liters solution

If system loses entropy the value of ΔS will be...

negative

Any molecular compound that is not an acid or base is a ___ electrolyte.

non

Classify C2H5OH as strong, weak, or nonelectrolytic and explain your reasoning.

nonelectrolyte b/c it is a molecular compound

Dissociation

occurs when the solvent pulls the individual ions from the crystal and solvates them

The species that increases in oxidation states is...

oxidized

Bronsted and Lowry defined bases as...

proton acceptors

Bronsted and Lowry defined acids as...

proton donors

Oxidation-Reduction reactions are also called...

redox reactions

The species that decreases in oxidation states is...

reduced

Generally, when solutions of an acid and a base are combined, the products are ___ and ___.

salt and water

Classify sodium carbonate (Na2SO4) as soluble or insoluble.

soluble

Aqueous Solution

solution in which the solvent is water

Acids and bases that COMPLETELY ionize in the solution are...

strong

Strong acids and bases tend to be ___ electrolytes.

strong

Classify CaCl2 as strong, weak, or nonelectrolytic and explain your reasoning.

strong electrolyte b/c it is a soluble ionic compound

Classify KOH as strong, weak, or nonelectrolytic and explain your reasoning.

strong electrolyte b/c it is a strong base

Classify HNO3 as strong, weak, or nonelectrolytic and explain your reasoning.

strong electrolyte b/c it is one of the seven strong acids

Solute

substance dissolved into solvent

Solvent

substance having the greatest abundance in a solution

What is the most familiar redox reactions?

the corrosion of metal

Enthalpy (ΔH)

the measure of energy in a system

Spectator Ions

the species that didn't change in the reaction (and where deleted from a net ionic equation)

Entropy (ΔS)

the thermodynamic measure of disorder or randomness in a system

Acids and bases that PARTIALLY ionize in the solution are...

weak

Weak acids and bases tend to be ___ electrolytes.

weak

Classify HCOOH as strong, weak, or nonelectrolytic and explain your reasoning.

weak electrolyte b/c it is a weak acid