Acids, Bases, Buffers, and pH

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Battery Acid

Lemon Juice

Vinegar, Cola

Tomato Juice

Black Coffee

Rainwater, Urine

Saliva, Human Blood + Tears

Seawater, Small Intestine

Milk of Magnesia

Household ammonia

Household bleach

1M NaOH

Acid

Any substances that increases the H+ concentration of a solution

Base

Any substance that reduces the H+ concentration of a solution

pH defined by neg. logarithm of H+ concentration

Neutral = [H+] = 10^(-7)

pH = -(-7) = 7

Every change in pH is a difference of 10

One substance has a pH of 4, another a pH of 8.

Substance 1 would have a H+ concentration 10,000 times that of substance 2.

Buffer - substances that minimize changes in concentration of H+ and OH-

Weak Acids

Reversibly release and accept back H+

Ocean Acidification

when C02 dissolves in seawater, it reacts with H2O, creating carbonic acid

Increases the ocean's pH by 0.1