Untitled

sour

acid taste

bitter

base taste

slippery

base feel

pH less than 7

acid pH

pH greater than 7

base pH

releases H+ ions in aqueous solution

acid releases …

releases OH- ions in aqueous solution

base releases …

corrosive

acid

non-corrosive

base

turns litmus paper pink

acid litmus paper

turns litmus paper blue

base litmus paper

produces OH- ions

Arrhenius base

produces H+ ions

Arrhenius acid

Arrehnius acid formula

HA→ (H+) (A-)

arrehnius base formula

MOH → (M+) (OH-)

bronsted Lowery Base

proton acceptor (takes a H+)

Bronsted Lowery Acid

proton donor (gives an H+)

conjugate acid-base pair

differ by 1 proton

amphoteric

a substance that can act as an acid and a base by gaining or losing a proton

metal + acid

Salt +H+ gas

acid + carbonate/hydrogen carbonate

salt + water + carbon dioxide

metal + water

base + hydrogen

nonmetal oxide + water

acid

Neutralization: acid + base

salt + water

metaloxide + water

base

strong acids

HCl, H2SO4 (only first H+), HNO3, HI, HBr, HCLO4

strong bases

Ba(OH2) or Li→ Fr

Pressure Units

1 atm=101.3 KPa=760 mmHg or torr

Volume

Liters 22.7@STP=1 mol

Temperature

k=C+273

Boyle’s Law

P up V down P1V1=P2V2

Charles’ Law

V up T up V1/T1 = V2/T2

Avogadro’s Law

n (mols) up V up n1/v1 = n2/V2

Ideal Gas Law

PV=nRT

R for atm

0\.0821

R for KPa

8\.314

Combination

PV/T = PV/T

pH +pOH

14

Molarity equation

M= mol/L

Know Stoicheometry

for dilution, gas laws, and molarity

H → pH

\-log\[H+\]

pOH → OH

10^-pOH

OH → pOH

\-log\[OH-\]

H+ → OH-

Kw=\[H+\]\[OH-\]

pH →H

10^-pH

Kw

1 x 10^14