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
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) - + + - + -
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
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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