Chem Acid and Base

Monoprotic

acids that donate one H+

Diprotic

acids that donate two H+

Triprotic

acids that donate three H+

[ ] → pH

-log

pH → [ ]

10^-pH

polyprotic

more than one H+

Name all strong acids

HCl, HBr, HI, H_2SO_4, HNO_3, HClO_4

Strong acids are ____

Strong electrolytes

In strong acids, the H is bonded to a

a highly electronegative ion

Why is H+ referred to as a proton

The electronegative ion takes the electron, and the H+ does not have any neutrons (as it is not a heavy isotope of hydrogen)

Covalently bonded atoms that give off an H+

molecular weak acid

Negative ions that have a hydrogen that leaves

anions containing ionizable H atoms/ weak acid

What are the amount of H_2O that are gained for +1,2,3 cations

2H_20, 4H_2O, 6H_2O (double the ligands)

Cations except ______ become hydrated

group I and SrBaCa

Why do bases dissociate instead of ionize

the base compounds are ionic

acids ____ protons and bases _____ them

donate, accept

What does a bigger k generally mean

the more k has done “its thing”

Ka=

[H+][CB]/ [Acid]

Kb=

[CA][OH-]/ [base]

5% Rule Test Formula

[H+] or [OH-]/ intial conc x 100% < 5%

How do you Sucessive Approximation

1. Go through normally

2. Plug in the “[.100-x]”

3. Cycle until x stays the same

Neutral Anions

Cl-, Br-, I-, NO_3-, ClO_4-

Neutral Cations

Li+, Na+, K+, Rb,+, Cs+, Ca+2, Ba+2, Sr+2

Basic Cations

none

Basic Anions

HCO_3^-, HS^-, F^-, CO_3^-2, S^-2, PO_4^-3, CN^-, NO_2^-2, HPO_4^-2, SO_4^-2, C_2H_3O_2^-

Acidic Cations

Mg+2, Al+3, NH_4+, transtions

Defintion of a Salt

cation + anion (can be acidic, basic, or neutral)

“Is a Salt basic, acidic, or neutral problem”

1. Determine if the cation and the anion are acidic, basic, or neutral

2. The one that overpowers and has a bigger K value wins (making the salt basic or acidic)

3. Show work by stating the ionization (acid) and dissociation (base)

4. Remember the H_2O in weak acids and double the ligands

H_2PO_4 system

H_2PO_4^-, HPO_4^-2, PO_4^-3

When taking log

add one sig fig

When taking inverse log

drop one sig fig