Honors Chemistry Chapter 19

Organic

Acids that begin with H

properties of acids

Sour taste, reacts with bases (metal hydroxides), reacts with carbonates and bicarbonates, conducts electricity, react with indicators, pH of less than 7, form electrolytes in water

properties of bases

Feel slippery, react with indicators, taste bitter, form electrolytes in water, conducts with electricity pH greater than 7

Salt

ionic compound that does not have H or OH

Arrehnius Acid

When an acid is in water it will dissolve and release H+

Arrehnius Base

When a base is in water it will dissolve and release OH-

Bronsted-Lowry definition

acid is the one that gives H+ and the base is the acceptor

Proton

H+ is AKA

Lewis definition

Acid accepts electron pair, and the base donates electron pair

Strength

Refers to degree of ionization

Concentrated/dilute

indicate how much of an acid or base is dissolved in solution. Moles of acid/base in given volume

Kw for water

1x10^-14

hydronium ion

What is H3O+ called?

Ka

acid dissociation constant

Strong Acid

What does a Ka<1

Weak Acid

Ka>1

Kb

Base dissociation constant

14

pH+pOH=

Water

Self ionizes

-log[H+/OH-]

equation for pH/ pOH

inverselog (-pH/-pOH)

inverselog (-pH/-pOH)When given pH or pOH and you want [H+]/[OH-] what equation should you use?

Neutralization reaction

acid + base -> salt + water

titration

Used to find the concentration of acid or base

equivalence point

moles of acid equal to moles of base

endpoint

when the indicator changes color

indicator

A compound that changes color in the presence of an acid or a base

Titration equation

__ Ma x Va = ___Mb x Vb

Creates Salt

Neutralization of H+ and OH-

Salt of hydrolysis

salt that can react with water to produce acid or base

nuetral salt

Strong acid + Strong base =

basic salt

weak acid + strong base =

acidic salt

strong acid + weak base =

Buffer

compound that prevents sharp, sudden changes in pH

Buffer Capacity

amount that can be absorbed before a big change in pH

Composition of Buffers

Weak Acid and one of its salts OR Weak Base and one of its salts

monoprotic

An acid that can only donate 1 hydrogen ion per molecule (H)

diprotic

and acid that can only donate 2 hydrogen ions per molecule (H2)

triprotic

an acid that can only donate 3 hydrogen ions per molecule (H3)

Self ionization

reaction in which water molecules produce ions

Le Chatelier's Principle

if stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress

Stress in Le Chatelier Principle

change in concentration of reactants or products, changes in temperature, and changes in pressure.

=Kw

[H+] x [OH-]

Alkaline solutions

basic solution

Standard solution

a solution of known concentration

unknown concentration

unknown concentration