2.  As temperature increases, the molecules velocity increases, increasing the pressure on the container.

4. StateShapeVolumeCompressible?Flows?SolidDefiniteDefiniteNoNo LiquidIndefiniteDefiniteNoYes GasIndefiniteIndefiniteYesYes

9.  Critical Point – above this temperature, no amount of pressure can liquefy it.  Triple Point – all three phases are in equilibrium

11.  Homogeneous mixtures  Solvent – the substance there is more of; it does the dissolving.  Solute – the substance there is less of; it is being dissolved.  Solute is dissolved in solvent

12.  Are all things soluble? ◦ No  Polar solvents dissolve polar solutes. ◦ Ex: water (polar)  Non polar solvents dissolve non polar solutes. ◦ Ex: oil (non polar)  “Like Dissolves Like”

13.  Intermolecular Forces  Temperature  Pressure ◦ For gases  What states of matter are required to form solutions? ◦ Any: solid, liquid or gas

14.  Heating  Stirring  Crushing  One exception: gases dissolve better in colder temperatures.

15.  Solubility of gas increases with pressure

16.  Solubility – the amount of solute that will dissolve in a given amount of solvent at a given temperature.  Saturated Solution – solution that contains all the solute it can at a given temperature.  Unsaturated Solution – solution that contains less than the saturated amount of solute.  Supersaturated Solution – solution that contains more solute than it could normally hold.

17.  Every compound has its own solubility curve.  Typically, when heated, solubility will increase

18.  Acids produce hydrogen ions  HCl  H + + Cl -  Bases produce hydroxide ions  NaOH  Na + + OH - H+H+ OH -

19.  Acids donate protons (+)  Bases accept protons (+)  Conjugate acid – particle formed when a base gains a hydrogen ion  Conjugate bases – particle that remains when an acid has donated a hydrogen ion  Conjugate acid-base pair – 2 substances that are related by the loss or gain of a single hydrogen ion ◦ Ex: NH 3 and NH 4 +

20. HCl (g) + H 2 O (l)  Cl - (aq) + H 3 O + (aq) AcidConj. AcidConj. Base Base Acid + Base  Conj. Base + Conj. Acid NH 3(g) + H 2 O (l)  NH 4 + (aq) + OH - (aq) Acid BaseConj. BaseConj. Acid

21.  Taste sour  pH from 0-6.99  Has H + at the beginning of the formula  Produce H 2(g) when reacting with most metals  Neutralize bases  Conducts electricity (because they contain electrolytes)  Turns litmus paper red

22.  HClhydrochloric acid  HBrhydrobromic acid  HIhydroiodic acid  HNO 3 nitric acid  H 2 SO 4 sulfuric acid  HClO 4 perchloric acid The stronger an acid, the weaker its conjugate base and vice versa.

23.  Taste bitter  pH between 7.01-14  Have OH - ions  Feels slippery  Neutralize acids  Turns litmus paper blue

24.  LiOHlithium hydroxide  NaOHsodium hydroxide  KOHpotassium hydroxide  RbOHrubidium hydroxide  CsOHcesium hydroxide  Ca(OH) 2 calcium hydroxide  Sr(OH) 2 strontium hydroxide  Ba(OH) 2 barium hydroxide  Mg(OH) 2 magnesium hydroxide ◦ Milk of magnesia, it is not completely soluble, but what does dissolve is a strong base.

25. AnionAcid NameExample -idehydro—icHCl hydrochloric acid -ite--ous HNO 2 nitrous acid -ate--icHNO 3 nitric acid **only binary acids use “hydro”

26.  H 2 SO 4  HF  H 3 PO 4  H 2 SO 3  H 2 CO 3  HNO 3 Sulfuric Acid Hydrofluoric Acid Phosphoric Acid Sulfurous Acid Carbonic Acid Nitric Acid

27.  Monoprotic – has 1 hydrogen ◦ HCl  Diprotic – has 2 hydrogens ◦ H 2 SO 4  Triprotic – has 3 hydrogens ◦ H 3 PO 4

28.  Always form a salt and water  Salt – a crystalline compound formed form an acids anion and a bases cation. HCl (aq) + NaOH (aq)  NaCl (s) + H 2 O (l)

29.  Can act as either an acid or a base  Water is amphoteric

30. [H+]pHpOH[OH-]

31. Once you have 1 item, you can get any other one.

33.  An unknown concentration of acid or base can be determined by measuring the amount of known acid or base that will neutralize the unknown.  An indicator changes color when the “end point” or neutralization occurs

34.  Standard solution ◦ Solution in which the concentration is known  End point ◦ The point at which equivalent amounts of reactants are present

35.  For one to one ratios  For non one to one ratios ◦ Need to calculate a mole ratio.

36.  If 15.0 mL of 0.500M NaOH is used to neutralize 25 mL of HCl, what is the concentration of the acid?  NaOH + HCl  H 2 O + NaCl  Since the ratio is 1:1, use M a V a =M b V b  (0.500M)(15.0mL)=M b (25.0mL)  M b =0.300M HCl

37. x = 0.0075 mol NaOH 0.0075 mol HCl 0.300M HCl

38.  A 25 mL solution of H 2 SO 4 is completely neutralized by 18 mL of 1.0M NaOH. What is the concentration of the acid?  NaOH + H 2 SO 4  H 2 O + Na 2 SO 4 2 1 1 2 x = 0.018mol NaOH

39. 0.0090mol H 2 SO 4 0.36M H 2 SO 4

40.  Can absorb moderate amounts of acid or base without a significant change in pH  Consists of a weak acid and its salt or a weak base and its salt.  Example ◦ Acetic acid: HC 2 H 3 O 2 ◦ Sodium acetate: NaC 2 H 3 O 2

41. HAH + + A - HA H + + A - Strong Acid Weak Acid Lots of H +, very little HA Lots of HA, very little H +