PH Read pp. 301-303.

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Presentation transcript:

pH Read pp. 301-303

What is pH and pOH? pH A measure of how acidic a solution is, or more specifically, how much H+ ions are present Key Idea: The more H+ ions present, the more acidic the solution pOH A measure of how basic a solution is (how much OH- ions are present) Key Idea: The more OH- ions present, the more basic the solution

[H+] (mol/L)

Each step on the scale is either 10 times stronger or weaker. (eg Each step on the scale is either 10 times stronger or weaker. (eg. 3 steps on the scale = 10x10x10 = 1000 times stronger or weaker) As you get closer to pH=0, it is more acidic. If it gets closer to pH=14, it is more basic. Neutral is when the pH=7.

pH Strength and Weakness How many times stronger is a solution that is pH=2 compared to a solution that is pH=6? How many times weaker is a solution that is pH=9 compared to a solution that is pH=3?

Calculations pH = - log[H+] [H+] = 10-pH To find pH (or pOH): To find [H+] (or [OH-]) pH = - log[H+] [H+] = 10-pH pOH = - log[OH-] [OH-] = 10-pOH Note: pH + pOH = 14

What is the pH if… [H+] = 0.052 mol/L? [OH-] = 0.00065 mol/L?

What is the pOH if… [OH-] = 0.25 mol/L? [H+] = 0.00010 mol/L?

Calculate [H+] if… pH = 3.4 pOH = 8.1

Calculate [OH-] if… pOH = 11.4 pH = 4.5