Outline for general Chemistry (lD) 6A. Solution( Chapter 4) 1 class 61. Solute solvent. and solution 6.2. Solubility(S)and molarity(C) a). Solubil ity: grams of solute /100 g solvent; Molarity: moles of solute /1 L solution (b). Be able to convert between solubility and molarity of a given solution 6.3. Electrolyt (a). Strong electrolyte: fully dissociate into cations and anions in solution or melt (b). Weak electrolyte: partially dissociate(with a dissociation factor between 0-1), and majority remains as molecules 64. Acid base and salt Note that"insoluble salt" is still a strong electrolyte 6.5. Reaction/calculation between ions in solution (a). Water solubility of different acids, bases and salts (b). Find out the limiting reactants for calculation 6.6. Ionic equation 6B. Precipitate(Chapter 16.5--16.8) I class 6.7. Solubility product (a). Ksp=[cation]m x [anion]n,(where m, n are coefficients of ions in the precipitate's dissociation reaction) (b). Convert between solubility product(Ksp)and solubility(s) 6.8. Pred ict the solubility formation Compare the magnitude of ion product, [cation]m x [anion]n, with the Ksp (a). cation]m x [anion<Ksp> under saturated solution, No precipitate (b). [cation]m x [anion]n=Ksp> saturated solution, Start to precipitate (c). [cation]m x [anion]n>Ksp)Over saturated solution, Precipitate is formed 6.9. The common ion effect 6.10. Calculation of ion concentrations in solution When more than one precipitate can be formed, which one will precipitat When the 2nd precipitate starts to form, what is the remaining ion concentration for the 1st ion? 7. Oxidation-Reduction Reaction( Chapter Il) 2 class 7.1. Oxidation numbers(Oxidation state) 7.2. Rules for assigning the oxidation number Apply the 5 steps in orderOutline for General Chemistry (II) 6A．Solution (Chapter 4) 1 class 6.1．Solute, solvent, and solution 6.2．Solubility (S) and molarity (C) (a)．Solubility: # grams of solute / 100 g solvent; Molarity: # moles of solute / 1 L solution (b)．Be able to convert between solubility and molarity of a given solution 6.3．Electrolyte (a)．Strong electrolyte: fully dissociate into cations and anions in solution or melt (b)．Weak electrolyte: partially dissociate (with a dissociation factor between 0~1), and majority remains as molecules 6.4．Acid, base, and salt  Note that “insoluble salt” is still a strong electrolyte 6.5．Reaction/calculation between ions in solution (a)．Water solubility of different acids, bases and salts (b)．Find out the limiting reactants for calculation 6.6．Ionic equation 6B．Precipitate (Chapter 16.5—16.8) 1 class 6.7．Solubility product: (a)．Ksp = [cation]m × [anion]n , (where m, n are coefficients of ions in the precipitate’s dissociation reaction) (b)．Convert between solubility product (Ksp) and solubility (S) 6.8．Predict the solubility formation – Compare the magnitude of ion product, [cation]m × [anion]n , with the Ksp (a)．[cation]m × [anion]n < Ksp → under saturated solution, No precipitate (b)．[cation]m × [anion]n = Ksp → saturated solution, Start to precipitate (c)．[cation]m × [anion]n > Ksp → Over saturated solution, Precipitate is formed 6.9．The common ion effect 6.10．Calculation of ion concentrations in solution  When more than one precipitate can be formed, which one will precipitate first?  When the 2nd precipitate starts to form, what is the remaining ion concentration for the 1st ion? 7．Oxidation-Reduction Reaction (Chapter 11) 2 class 7.1．Oxidation numbers (Oxidation state) 7.2．Rules for assigning the oxidation number  Apply the 5 steps in order