Unit 3 Modules:6-8

Nitric acid

HNO3

Sulfuric acid

H2SO4

Hydrochloric acid

HCl

Hydrobromic acid

HBr

Hydroiodic acid

HI

Perchloric acid

HClO4

Hydrofluoric acid

HF

Phosphoric acid

H3PO4

Carbonic acid

H2CO3

Sulfurous acid

H2SO3

nitrous acid

HNO2

hydrogen sulfide

H2S

Another name for H2S

hydrosulfuric acid

hydrogen cyanide

HCN

another name for HCN

hydrocyanic acid

Organic acids

RCOOH

formic acid

HCOOH

acetic acid

CH3COOH

Lithium hydroxide

LiOH

Sodium hydroxide

NaOH

Potassium hydroxide

KOH

rubidium hydroxide

RbOH

cesium hydroxide

CsOH

Calcium hydroxide

Ca(OH)2

Strontium hydroxide

Sr(OH)2

Barium hydroxide

Ba(OH)2

Ammonia

NH3

Acid strength of HNO3

strong acid

Acid strength of H2SO4

strong acid

Acid strength of HCl

strong acid

Acid strength of HBr

Strong acid

Acid strength of HI

Strong acid

Acid strength of HClO4

strong acid

acid strength of HF

weak acid

acid strength of H3PO4

weak acid

acid strength of H2CO3

weak acid

acid strength of H2SO3

weak acid

acid strength of HNO2

weak acid

acid strength of H2S

weak acid

acid strength of HCN

weak acid

acid strength of RCOOH

weak acid

acid strength of HCOOH

weak acid

acid strength of CH3COOH

weak acid

acid strength of LiOH

strong base

acid strength of NaOH

strong base

acid strength of KOH

strong base

acid strength of RbOH

strong base

acid strength of CsOH

strong base

acid strength of Ca(OH)2

strong base

acid strength of Sr(OH)2

strong base

acid strength of Ba(OH)2

strong base

acid strength of NH3

weak base

acid strength of organic amines

weak base

acid

substance with H in formula that dissociates in H2) to yield H30+

base

substance with OH in formula that dissociates in H2O to yield OH-

oxyacids

acid where the central atom is attached to nothing but oxygen

Bronsted Lowry Acid

an acid is an H+ donor

Bronsted Lowry Base

a base is an H+ acceptor

what is Kb

base ionization constant; a base that doesn't associate

Acid base buffer

solutions that don't exhibit large changes in pH upon addition of acid or base are known as buffers

common ion effect

the shift in ionic equilibrium caused by the addition of a solution that provides an ion that takes part in the equilibrium.

Henderson Hasselbalch Equation

pH = pKa + log(base/acid)

When is the Henderson-Hasselbalch equation used?

buffers only

buffer capacity

the ability to withstand additions of acid or base without significant pH change

2 Factors that capacity is controlled by

1. Concentration of buffer components

2. The ratio of [A-] to [HA]

buffer range

the pH range over which the buffer acts effectively

pKa +/- 1

Solubility product constant (Ksp)

An equilibrium constant for a slightly soluble ionic compound dissolving in water.

System

part of universe we wish to study, a particular reaction

surroundings

all others parts of universe, including reaction vessel

Entropy (S)

disorder, randomness. Refers to the state of order of a system

1st law of thermodynamics

energy cannot be created or destroyed

2nd law of thermodynamics

the entropy of the universe increases in a spontaneous process and remains unchanged if the system is at equilibrium

standard entropy (S°)

the entropy of the standard state of the substance at 25°C

3rd law of thermodynamics

the entropy of a perfect crystalline substance is a zero at absolute 0

spontaneous change

a change that occurs under specified conditions without a continuous input of energy from an outside system

nonspontaneous change

a change that only occurs if the surroundings continuously supply the system with an input of energy