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Acids, Bases, pH and pOH

Acids, Bases, pH and pOH. Pg 547 # 1-11. Acid concentration  pH. [H 3 O + ]  pH 1.0 x 10 -4 mol/L = pH 4 3.16 x 10 - 3 mol/L = -log [ H 3 O + ] = 3.16 x 10 - 3 log+/- = pH 2.50 #7. pH  Acid concentration. pH 3  1.0 x 10 - 3 mol/L

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Acids, Bases, pH and pOH

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  1. Acids, Bases, pH and pOH Pg 547 # 1-11

  2. Acid concentration  pH • [H3O+]  pH • 1.0 x 10-4mol/L = pH 4 • 3.16 x 10-3mol/L= -log [H3O+] = • 3.16 x 10-3log+/- • = pH 2.50 • #7

  3. pH  Acid concentration • pH 3 1.0 x 10-3mol/L • pH 2.9  1.O x 10-2.9mol/L • = .001258 or • = 1.3 x 10-3 M or • = 1.3 x 10-3 mol/L • #8

  4. pH to pOH • pH + pOH = 14 • pH = 14 – pOH • pOH = 14 - pH

  5. Concentration of Base  pOH • [OH-]  pOH • 3.2 x 10-11M = 3.2 x 10-11log+/- • pOH 10.5 • pH = 14 – pOH = 14 – 10.5 = pH 3.5 • #10

  6. #7. The hydronium ion concentration in a solution is 3.16 x 10-3mol/L. What is the [OH-] • Find pH. • Find pOH • Find concentration of [OH-]

  7. #9. If 5.3 g of the strong base NaOH is dissolved in water to form 1500 mL of solution, what are the pH, [H3O+], and [OH-]

  8. Answers Pg 547 # 7-11

  9. Clues for Answering Questions • If pH is less than 7 = Acid = red • If the concentration of [H30+] in the solution has a exponent less than -7 = Acid • If the pOH is high then the pH is low • If pH is more than 7 = Base = blue • If the concentration of the [OH-] in the solution has an exponent less than -7 = Base • If the pOH is low, the pH is high

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