L20_Solub1_115b08

L20_Solub1_115b08 - 15.43 Add 0.025 moles of HCl to 2.0 L...

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15.43. Add 0.025 moles of HCl to 2.0 L of 0.050 mol tris weak base p K b =5.92 . Calculate the pH. reactions: 1. Neutralization: tris + HCl -> trisH + Cl - -> trisH + + Cl - base acid salt Result: base + salt = buffer 2. Equilibrium of conj. acid trisH + in water: trisH + <-> tris + H + 0.025 0.025 0 Eq: 0.025-x 0.025+x x pK a = 14.0 -5.92 = 8.08 [ ] 0.025 log 8.08 log 8.08 [ ] 0.025 a acid pH pK base ≈− = = Note: You will do such neutralizations in lab (titration)
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L20: Ch. 16 Solubility and precipitation equilibria Cadmium, chromium (III), aluminum, and nickel (II) hydroxides Solubility and solubility product Effect of pH Common ion effect Complex ions and solubility
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What happens when solids are dissolved in water? Salt water
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Ionic salts (NaCl): NaCl(s) Na + + Cl - Na + (aq) + Cl - (aq) - + + - + -
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How much solute can we dissolve in 1 L of solvent? Characteristic of substance and solvent, called solubility . Solubilities of some salts in water at 25 C: 0.0018 1.3x10 -5 AgCl 5,570 27 AgClO 4 351 6 NaCl gram/L M/L Salt
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Solubility depends on temperature: Some salts are more soluble at higher temp and some less
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Salts of multi-valent ions are less soluble; Sulfates, carbonates, phosphates are insoluble.
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This note was uploaded on 07/22/2008 for the course CHEM 115b taught by Professor Reisler during the Spring '08 term at USC.

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L20_Solub1_115b08 - 15.43 Add 0.025 moles of HCl to 2.0 L...

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