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power of hydrogen

power of hydrogen. pH scale. Logarithmic scale expressing H +1 concentration, [H +1 ] If pH changes by factor of 1, [H +1 ] changes by factor of 10 pH = -log[H +1 ]. Molarity to pH. To determine pH: express [H +1 ] in scientific notation

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power of hydrogen

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  1. power of hydrogen

  2. pH scale • Logarithmic scale • expressing H+1 concentration, [H+1] • If pH changes by factor of 1, [H+1] changes by factor of 10 • pH = -log[H+1]

  3. Molarity to pH To determine pH: • express [H+1] in scientific notation • remember, [ ] means concentration of whatever is inside brackets • log is the power of 10

  4. Molarity to pH for Pure water tiny bit of ionization in pure water: H2O  H+1 + OH-1 • [H+1] = [OH-1] = 1 X 10-7M • pH =-log[H+1]= -(-7) = 7

  5. [H+1] 1 M or 1X100 M 0.1 M or 1 X 10-1M 0.01 M or 1 X 10-2M .001 M or 1 X 10-3M pH 0 1 2 3 pH

  6. pH to Molarity pH = -log[H+1], solve for [H+1] • -pH = log[H+1] • antilog(-pH) = [H+1] • say pH = 5, then –pH = -5 • antilog(-5) = 10-5 • the –pH becomes the power of 10!

  7. pOH • by analogy: pOH is defined as –log[OH-1] • express [OH-1] in scientific notation • if [OH-1] = 1.0 X 10-3 M • then pOH = -log(10-3) = -(-3) = 3

  8. pOH = 14 10 7 4 0

  9. pH range • 0 to 14 (7 is neutral) • pH = 0, strongly acidic • pH = 14, strongly basic

  10. ACID or BASE? • acids: [H+1]  [OH-1] • bases: [OH-1]  [H+1]

  11. Relationships of: pH, pOH, [H+1] and [OH-1] productof [H+1] and [OH-1] is always 1x10-1M add exponents when multiple in scientific notation sum of pH and pOH is always 14

  12. 11 4 5 13 pH + pOH = 14 • pH = 3, pOH = • pH = 7, pOH = • pH = 10, pOH = • pH = 9, pOH = • pH = 1, pOH = 7

  13. 1 x 10-4 M 10 1x10-10 M if pH = 4 • [H+1] = ? • pOH = ? • [OH-1] = ?

  14. 14 – 3 = 11 1x10-11 M if the [OH-1] = 1 X 10-3 pOH = -log[OH-1] = -log(10-3) = -(-3) = 3 • pOH = ? • pH = ? • [H+1] = ?

  15. 5 14 – 5 = 9 1x10-9M if the [H+1] = 1 x 10-5M • pH = ? • pOH = ? • [OH-] = ?

  16. [H+] (M) pH [OH-] (M) pOH Acidic or Basic 3 1x10-3 1x10-11 11 A 1x10-5 5 1x10-9 9 B 1x10-2 A 1x10-12 12 2 6 B 1x10-6 8 1x10-8

  17. How to safely test pH • instruments – use a pH meter • indicators – use a series of indicators • see if substance reacts with a metal other than Cu, Ag, or Au • NEVER “taste”

  18. pH meters

  19. Indicator • substance that changes color over narrow pH range • use several indicators to narrow down pH range of substance • See Table M

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