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UA CH 102 - Solubility Products
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CH 102 1st Edition Lecture 17Outline of Current Lecture I. Blood ChemistryII. Blood pHIII. The Solubility ProductIV. The Solubility Product ConstantV. Solubility of Ferric Hydroxide in WaterVI. Common Ion EffectVII. Acid Rain Dissolving SculpturesCurrent LectureI. Blood Chemistrya. Blood is a complex fluidb. Contains blood cellsi. 4 to 6 million erythrocytes per microliterii. 4,000 to 11,00 leukocytes per microliteriii. 200,000 to 500,000 thrombocytes permicroliterc. Plasma ~55%i. 92% water, 8% blood plasma proteinsii. Traces of dissolved nutrients, glucose, amino acods, fatty acidsiii. Proteins include serum albumin, blood-clotting factors, immunoglobulins, lipoproteinThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.II. Blood pHa. The pH of blood is regulated to stay between 7.38 and 7.42b. The pH is largely controlled by the carbonate buffer systemc. When carbon dioxide dissolves in water, it form carbonic acid, a diprotic weak acidi. CO2 (g) D CO2 (aq)ii. H2O (l) + CO2 (aq) D H2CO3 (aq) iii. H2CO3 (aq) + H2O (l) D H3O+ (aq) + HCO3- (aq)iv. The apparent pKa1 = 6.3III. The Solubility Producta. AgBr (s) → Ag+ (aq) + Br- (aq)i. K_c=[〖Ag〗^+ ][〖Br〗 ^- ]/AgBrb. When the equilibrium expression contains a solid, the activity of the solid is onei. This means the concentration can be taken as oneIV. The Solubility Product Constanta. AgBr (s) → Ag+ (aq) + Br- (aq)i. K_c=[〖Ag〗^+ ][〖Br〗 ^- ]/1=[〖Ag〗^+ ][〖Br〗^- ]=K_spii. Ksp = [Ag+][Br-] = 5.35x10-13b. The solubility product constant, Ksp, is temperature dependent.c. Generally the solubility increases with increasing temperature.d. Values of Ksp are given for a temperature of 25 °C.V. Solubility of Ferric Hydroxide in Watera. Fe(OH)3 (s) → Fe3+ (aq) + 3 (OH)- (aq)b. Ksp = [Fe3+][OH-]3 = 2.79x10-39i. What is the molar solubility of iron hydroxide in water at 25 °C?ii. Have many grams will dissolve in a liter of water at 25 °C?iii. What is the pH of the solution?VI. Common Ion Effecta. For solubility equilibrium, adding a common ion to the solution decreases the solubility. b. What is the solubility of lead sulfate in a solution containing 0.100 M sodium sulfate?i. PbSO4 (s) → Pb2+ (aq) + SO42- (aq)ii. Ksp = [Pb2+][SO42-] = 1.82x10-8VII. Acid Rain Dissolving Sculpturesa. Marble is a metamorphic rock containing mostly calcium carbonateb. The solubility product constant for calcium carbonate isi. Ksp = [Ca2+][CO32-] = 4.96 x 10-9c. Eroding marble staturesd. What is the solubility of calcium carbonate in pure water?e. Acid rainf. Occasional pH readings in rain and fog water of well below 2.4 have been reported in industrialized


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UA CH 102 - Solubility Products

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