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pH

C h a p t e r 2 0

Water forms ions

H

2

O ----> H + + OH -

Water splits apart into hydrogen ions (H+) and hydroxide ions (OH-).

This process is called self-ionization.

pH

 pH stands for potential hydrogen.

It is a measure of the hydrogen ion (H+) concentration in a solution.

Acids

An acid is a substance that increases the Hydrogen ion (H+) concentration in a solution.

Acids taste sour.

Common acids include:

Battery acid

Stomach acid

Lemon juice, tomatoes

Vinegar

Beer, wine, soda, coffee

Rain

Milk

Urine

Acids used in Chemistry

HCl Hydrochloric acid

HNO

3

Nitric acid

H

2

SO

4

H

3

PO

4

Sulfuric acid

Phosphoric acid

CH

3

COOH Ethanoic acid

H

2

CO

3

Carbonic acid

Bases

A base is a substance that reduces the the H+ concentration in a solution. It has a lot of OH- ions.

Bases taste bitter and feel slippery.

Common bases include:

Blood

Seawater

Pepto Bismal, Tums, etc.

Soap

Ammonia

Bleach

Oven Cleaner

Bases used in Chemistry

KOH Potassium hydroxide

NaOH Sodium hydroxide

Ca(OH)

2

Mg(OH)

2

Calcium hydroxide

Magnesium hydroxide

Neutral pH

If the concentration of hydrogen ions and hydroxide ions is equal, a solution is said to have a neutral pH.

Pure water (distilled water) has a neutral pH

pH Scale

The pH scale ranges from 0-14.

Acids are less than 7, Bases are greater than 7.

Determining pH from H+ concentration

The numbers on the scale come from the H+ ion concentration, for example:

[H + ] = 10 -7  pH = 7

[H + ] = 10 -4  pH = 4

[H + ] = 10 -12  pH = 12 pH values are equal to the absolute value of the exponent of the H+ ion concentration.

Determining pH from OH- concentration

The pH is the absolute value of 14 minus the absolute value of the [OH ] concentration

[OH ] = 10 -10  pH= 4

[OH ] = 10 -3  pH= 11

[OH ] = 10 -2  pH= 12

pH scale

Most biological fluids have pH 6 – 8

 pH values in human stomach can reach 2

Each pH unit represents a 10-fold difference in H + &

OH concentrations.

 small change in pH actually indicates a substantial change in [H + ] & [OH ]

Buffers

Buffers are substances that minimize changes in the concentrations of H+ and OH- in solution.

Buffers in your blood keep your pH close to 7.4 by accepting or donating H+ ions as needed.

Determining pH

Titration: you add an indicator and watch for a color change pH meter: electronic, very sensitive pH paper (Litmus paper): color change scale

Cabbage Juice: natural pH indicator, color change

pH Lab

Use the garbage cans!! Do the front side BEFORE you start your lab.

You will be testing 10 substances:

1. isopropyl alcohol

2. vinegar

3. baking soda solution

4. 7-up soda

5. hydrogen peroxide

6. alka seltzer solution

7. pineapple juice

8. bottled water

9. tap water (get some from the faucet)

10. your spit

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