Unit 9- Solution Chemistry



Unit 9- Solution ChemistrySolution Chemistry: Study of Chemical reactions that occur in solution9.1 – Solutions and SolubilityDefine in your own words and give an example: (p.193)Solution –Solvent – Solute – Soluble- Saturated - Unsaturated –Solubility - Assignments: Hebden p.194 #1-4 Explain: Why is Solution Chemistry so convenient? 9.2Conductivity : Chemistry that Kills-316865198755452120-5715+ = _____OR:Ye-olde Hair Dryer Ye-olde Bath-tub2307590146685-9080539370+ = ___ Any solution with a sufficient amount of ions will conduct electricity.So, in order to conduct electricity - solutions must have ______● ___ ions, ___ conductivity___ ions, ___ conductivity -320675103505The ion is actually a new concept, and the idea of it revolutionized solution chemistry. In fact, __________________________, the chemist who discovered them, won the _______________ in 1903. "in recognition of the extraordinary services he has rendered to the advancement of chemistry by his electrolytic theory of dissociation”.Solutions that will conduct - ______________________ dissolved in water● metal + non-metal- _______________________● start with H+, end with COOH● end with OH-* organic acids → conductex: CH3COOH, acetic acid/ vinegarSolutions that will not conduct________________non-metal + non–metalcompounds who’s formulae start with __________ (organic)exception: acetic acidIonic compound → solid8890339725How to decide if a substance is ______________ or _____________Assignment: Hebden pg 196 #5bcd, 6-8 (a,c,e,g,i)9.3Molecular PolarityIntermolecular forces - forces _____________ molecules (aka Vander Waals forces)3 kinds: ___________________________________________________________London Forces -weak attractive forces that arise because of _____________- London forces are always present/possible- the larger _________________, stronger the forces- due to a temporary ______________Definiton – Dipole: ___________________________________________________Dipole-Dipole Forces- due to a ______________________ dipole- one side of the molecule is _________________ positive and one side is ______________ negative-for this to happen, the bond must be between two atoms with different _________________________Ex. HCl NH3 H2OHydrogen Bondingspecial kind of ________________________________ forcebetween H and ____, H and _____ or H and ______3577590-331470Hydrogen bonds are ________________ than dipole-dipole forces because Hydrogen has a ____________________________The information above was only for specific BONDS. Now lets see how this applies to entire MOLECULES (which often have more than one bond)Some definitions:Polar - a molecule that has a _______________ bond- __________________(bond dipoles don’t cancel each other out)- someone will win the tug of warNon-polar- has a _______________ bond - ________________(bond dipoles cancel each other out)- no one will win the tug of warExamples:HCl CH3Cl BH3 BeF2What kinds of forces are involved with the following molecules?O H HO – O H – Cl - ________ - London - London - __________ - dipole – dipole - ______________Assignment: Polar Covalent Worksheet and pg. 199-203 #9-10, 14**** Remember: we are looking at dipoles in COVALENT molecules. Ionic compounds have permanent charges so this doesn’t apply to them****9.4Polar and Non Polar SolventsWhat is a solvent again?What does polar mean?Some examples of Polar and Non-Polar SolventsHow do we know what dissolves in what? There is a general rule:“ ________ dissolves __________.”__________ (ionic) solvents dissolves ____________ (ionic)________________ solvents dissolves ________________But why?Dissolving process involves _______ different attractions:the attraction of a ___________ molecule to other solvent moleculesthe attration of a ____________ molecule to _________ particlesthe attraction of ____________ particles to solute particlesIf ____________ is needed to _________ a bond, this must mean energy must be ______________ when a bond is _________. If there are ___________ bonds formed between solvent and solute particles, there is enough energy to allow solute particles to _______ their bonds. The ________________ of the solvent molecules to each other allows the broken bonds of the solute to be dispersed and dissolving occurs.In-Class Assignment:Dissolving Proof:Based on the kind of reasoning above, in partners of 2, have one person explain in written word the process of non-polar solvents dissolving non-polar solutes and why polar solutes do not dissolve. Have the other person explain the polar dissolving process and why non-polar solutes do not dissolve in them. Share your work together in pairs, and summarize your findings and proofs.This must be written on a separate piece of paper, and each person must complete a copy of their own. Your logic is important here as you are proving the statement “Like dissolves like”Solubility of Polar and Ionic Solutes:Solubility of Non Polar SolutesAssignment: Hebden pg 207 #17-22Nature of solution of ionsThe process of dissolving is quite complicated. If sugar or salt dissolves in solution, then macroscopically it looks like it is “disappearing”. But as chemists we know better.In order for a solution to form, a solute must be able to ___________ in a solvent. This interaction between a solute and solvent is called ____________________.Ionic solid- solid made of _______ in the form of a ______________ (the orderly arrangement of particles within a crystal)1459865151130Na+ =Cl- =Molecular solid- solid made from ________________________1944370105410C = H =From the previous section, the nature of solvation determines the extent to which a solute dissolves.There are several ways a solute can dissolve into ions:Dissociation - separating previously existing _______ in ionic solidNaCl(s) → Na+(aq) + Cl –(aq)-16637010160ORIonization – separating ______________ molecules into ions. *There are no ions before the solute is able to react with the solvent.CH3COOH(l) → CH3COO-(aq) + H+(aq)Examples:Write an equation to show the dissociation of CaCl2(s) in water.Write an equation to show the ionization of HCN in water.Calculating concentration of ions in solutionsEnding the Solution Chemistry Unit, we will practice some ion concentration calculations based on our knowledge of ion dissociation.Ex.What is the [F-] in 0.20M AlF3?Ex. What is the [ ] of the all the ions when 25.0mL of 0.25M BF3 is mixed with 75.0mL of 0.50M MgF2? Ex. What is the [OH-] formed when 15.0 g of Fe(OH)3 is dissolved in 0.500 L?Assigned Work: Hebden pg.210 #28-35 ................
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