Let’s take a look at water  2H 2 O  H 3 O + + OH -  [H 3 O + ][OH - ]= 1x10 -14 M 2  [H 3 O + ]= 1x10 -7 M  [OH - ]= 1x10 -7 M  K w = 1x10 -14 M.

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Presentation transcript:

Let’s take a look at water  2H 2 O  H 3 O + + OH -  [H 3 O + ][OH - ]= 1x M 2  [H 3 O + ]= 1x10 -7 M  [OH - ]= 1x10 -7 M  K w = 1x M 2

Example 1  An acid is added to water and gives a hydroxide ion concentration [OH - ] of 1.0x M. What is the hydrogen ion concentration [H + ] ?

What is pH?  Pouvoir hydrogene: “hydrogen power”  pH = measure of [H 3 O + ] Acidity  [H 3 O + ] expressed in powers of 10  Ex to 10 -1

pH Scale  Range from  NEUTRAL, pH=7. (pure water)  BASE, pH > 7. (ocean water, milk of magnesia, baking soda)  ACID, pH < 7. (stomach acid/HCl, vinegar, soft drinks)

pH Scale

How do we measure the pH of a solution?  Acid-base indicators (ex. litmus paper)  pH meter

Equations  pH = -log[H + ]  pOH = -log[OH - ]  pH + pOH = 14  [H + ][OH - ] = 1x M 2

 Example 2: What is the pH of a solution with a hydrogen ion concentration of 1x10 -4 M ? Is this solution acidic or basic ?

 Example 3: What is the hydrogen ion concentration of a solution with a pH of 11 ? Is this solution acidic or basic ?

 Example 4: Calculate the [H + ] and [OH - ] of a vinegar solution with a pH of 2.5.

Now, you try……  1) [H 3 O + ] = 1.5x10 -6 M. Find the pH.  2) A solution’s pH is What are the [H 3 O + ] and [OH - ] concentrations in the solution?

Thought Question  When an acid is added to a beaker of water, what happens to the [H 3 O + ] and [OH - ] in the solution? Why? What happens to the pH? Why?