University:
Eastern Kentucky University
Course:
CHE 111 | General Chemistry
Academic year:

2020
Views:

437

Pages:

1
Author:

perlesdesfees9ovd

General Chemistry 9: Solutions Terminology Solubility Rules Solution: Homogenous mixture. Solvent particles surround solute particles via electrostatic interactions. Solvation or The process of dissolving a solute in solvent. Most Dissolution: dissolutions are endothermic, although dissolution of gas into liquid is exothermic. Solubility: Maximum amount of solute that can be dissolved in a solvent at a given temp. Soluble Na+, K+, NH4+ NO3Cl-, Br-, I-Except with Pb2+, Hg22+, Ag+ SO42- Except with Ca2+, Sr2+, Ba2+, Pb2+, Hg22+, Ag+ Molar Solubility: Molarity of the solute at saturation. Complex Ions: Cation bonded to at least one ligand which is the epair donor. It is held together with coordinate covalent bonds. Formation of complex ions #solubility. Solubility in Water: Polar molecules (with +/- charge) are attracted to water molecules and are hydrophilic. Nonpolar molecules are repelled by water and are hydrophobic. Polar = Hydrophilic Nonpolar = Hydrophobic Insoluble S2- Except with Na+, K+, NH4+, Mg2+, Ca2+, Sr2+, Ba2+ O2- Except with Na+, K+, Sr2+, Ba2+ OH- Except with Na+, K+, Ca2+, Sr2+, Ba2+ CrO42- Except with Na+, K+, Mg2+, NH4+ PO43- & CO32-Except with Na+, K+, NH4+ Concentration % by mass: -.""/"01234 -.""/"0123506 Mole Fraction: 𝑋< = Molarity: 𝑀= Molality: 𝐶- = Normality: 𝑁= × 100% -014"/"01234 303.1/-014" Colligative Properties -014"/"01234 1534>"/0?/"0123506 -014"/"01234 AB/0?/"01C463 #/0?/4F25C.1463" 1534>"/0?/"0123506 Can also just be a lowercase m For acids, the # of equivalents (n) is the # of H+ available from a formula unit. Dilutions: M1 V1 = M2 V2 Solutions Equilibria Saturated solutions are in equilibrium at that particular temperature. Solubility Product Equilibrium expression for something that dissolves. Constant: For substance AaBb, 𝐾"#= [A]( [B]* Ion Product: 𝐼𝑃= [A]( [B]* IP < Ksp unsaturated IP = Ksp saturated at equilibrium IP > Ksp supersaturated, precipitate Formation or Kf. The equilibrium constant for complex formation. Stability Constant: Usually much greater that Ksp. Common Ion ¯solubility of a compound in a solution that already Effect: contains one of the ions in the compound. The presence of that ion shifts the dissolution reaction to the left, decreasing its dissociation. Chelation: When a central cation is bonded to the same ligand in multiple places. Chelation therapy sequesters toxic metals. Colligative Properties: Physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity. Raoult’s Law: Vapor pressure depression. 𝑃< =/𝑋< 𝑃< ° The presence of other solutes ¯evaporation rate of solvent, thus ¯Pvap. Boiling Point Elevation: ∆𝑇I =𝑖/𝐾I /𝐶𝑖 =ionization/factor 𝐾I = boiling/point/depression/constant 𝐶- = molal/concentration Freezing Point Depression: ∆𝑇? =𝑖/𝐾? /𝐶𝐾? = freezing/point/depression/constant Osmolarity: The number of individual particles in solution. Example: NaCl dissociates completely in water, so 0"-01 1/M/NaCl= 2/ 1534> Osmotic Pressure: “Sucking” pressure generated by solutions in which water is drawn into solution. p =𝑖/𝑀/R/𝑇 𝑖 =vanb t/Hoff/factor 𝑀=molar/concentration/of/solute 𝑅 =gas/constant 𝑇=temperature