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Acid-Base Equilibrium

Acid-Base Equilibrium. pH and pOH. Hydrogen Ion Concentration and pH. pH scale developed by a Danish chemist Sören S ö renson Numerical value without units, that communicates the hydrogen ion concentration of a solution

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Acid-Base Equilibrium

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  1. Acid-Base Equilibrium pH and pOH

  2. Hydrogen Ion Concentration and pH • pH scale developed by a Danish chemist SörenSörenson • Numerical value without units, that communicates the hydrogen ion concentration of a solution • The pH of a solution is the negative of the logarithm to the base ten of the hydrogen ion concentration pH = -log[H+(aq)]

  3. pH = -log[H+(aq)] • The number of significant digits following the decimal point in the pH value is equal to the number of significant digits in the hydrogen ion concentration Example Calculate the pH of a solution with a hydrogen ion concentration of 4.57 x 10-11 mol/L. Answer 4.57 x 10-11mol/L has three significant digits, therefore pH = 10.340 has three decimal places

  4. At SATP, • an acidic solution is one in which the [H+(aq)] is GREATER than 10-7 mol/L • a basic solution is one where the [H+(aq)] is LESSthan 10-7mol/L • A neutral solution is one where the [H+(aq)] is EQUAL to 10-7 mol/L

  5. pH Scale • Neutral solution pH = 7.00 • Acidic solution pH < 7.00 • Basic solution pH > 7.00 • NOTE that the hydrogen ion concentration changes by a multiple of 10 for every increase or decrease in one pH unit.

  6. Converting pH to [H+(aq)] • Sometimes converting from pH to the molar concentration of hydrogen may be necessary • Conversion based on the mathematical concept that a base ten logarithm represents an exponent [H+(aq)] = 10-pH Example Convert a pH of 11.36 to a hydrogen ion concentration. Answer pH = 11.36 has two decimal places, therefore the hydrogen ion concentration is 4.4 x 10-12 mol/L with two significant digits.

  7. pOH and [OH-(aq)] • It is convenient to describe hydroxide ion concentrations in a similar way as is done for H+(aq) concentrations, by calculating pOH pOH= -log[OH-(aq)] • A solution’s pOH may be used to calculate the hydroxide ion concentration: [OH-(aq)] = 10-pOH

  8. pKw pKw = -logKw • Since we know Kw = 1.0 x 10-14 at SATP the –logKw = 14.00 = pKw • Using logarithm rules and equilibrium law expression for the autoionization of water we can say pH + pOH = pKw pH + pOH = 14.00 (at SATP)

  9. Learning Checkpoint p. 546 Practice UC # 12, 13, 14, 15(a)(b)(c) p. 549 Practice UC # 17, 18, 19 p. 549 Section 8.1 Questions UC # 4

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