Chapter 18

Chapter 18 - [H 3 O + ] = 0.050 M [OH-] = 2.0 x 10-13-If...

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Chapter 18 Strong Electrolytes -equilibria of weak acids and bases -distinguish weak acids and bases from strong electrolytes -Strong Water Soluble Acids -list of strong acids (Chapter 4) -Strong Water Soluble Bases -list of strong bases -Most Water Soluble Salts Example 18-1 : Calculate the concentrations of ions in 0.050 M nitric acid, HNO 3 HNO 3 → H + (aq) + NO - 3(aq) 0.050 M 0.050 M 0.050M Example 18-2 : Calculate the concentrations of ions in 0.020 M strontium hydroxide, Sr(OH) 2 , solution [Sr 2 ] = 0.020 M [OH - ] = 0.040 M The Autoionization of Water H 2 O (l) + H 2 O (l) ↔ H 3 O + (aq) + OH - (aq) K c = [H 3 O + ][OH - ] K w = 1.0 x 10 -14 Example 18-3 : Calculate the concentrations of H 3 O + and OH - in 0.050 M HCl
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Unformatted text preview: [H 3 O + ] = 0.050 M [OH-] = 2.0 x 10-13-If either the [H 3 O = ] or [OH-] is known, the pH and pOH can be calculated Example 18-4: Calculate the pH of a solution in which the [H 3 O + ] = 0.030M pH = 1.50, [OH-] = 3.3 x 10-13 , pOH =12.50 (pH + pOH = 14) Example 18-5 : The pH of a solution is 4.597. What is the concentration of H 3 O + ? [H 3 O + ] = 2.5 x 10-5 [OH-] = 3.45 x 10-10 pOH = 9.403 ****slide 23 [H 3 O + ][OH-] = Example 18-6 : [H 3 O + ] = 0.020 M [OH-] = 5.0 x 10-13 M pH = 1.70 pOH = 12.30 Ionization Constants for Weak Monoprotic Acids and Bases-=***slide 32 ***slide 34 3,2,1,4,5...
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