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Exam 1*
Things good to know
| Question | Answer |
|---|---|
| 7 strong acids | HCl, HBr, HI, HNO3 (nitric acid), H2SO4 sulfuric acid, HClO3 chloric acid, HClO4 perchloric acid |
| Group IA metal cations or NH4+ | SOLUBLE. No exceptions. |
| NO3− (nitrate), ClO4− (perchlorate), ClO3- (chlorate), C2H3O2- (acetate) or HCO3- (bicarbonate) anions | SOLUBLE. No exceptions. |
| Cl− (chloride), Br− (bromide), CN- (cyanide), and I− (iodide) anions | SOLUBLE except when combined with Ag+, Hg22+, and Pb+2 cations. |
| SO42- (sulfate) and SO32- (sulfite) anions | SOLUBLE except when combined with Ag+, Hg22+, Pb+2, Ca+2, Ba+2 or Sr+2 cations. (Sulfur loves heavier group 2A metals) |
| Most Ionic compounds that contain PO43- (phosphate), CO32- (carbonate), OH- (hydroxide), S2- (sulfide), O2- (oxide), CrO42- (chromate) and F- (fluoride) anions | INSOLUBLE (except when combined with Group IA or NH4+ cations) |
| Exception - Ca(OH)2, Ba(OH)2, and Sr(OH)2 are considered soluble. Group IA and heavier Group IIA oxides react with water, to form the corresponding hydroxide which is soluble. Na2O(s) + H2O → 2 NaOH(aq) CaO(s) + H2O → Ca(OH)2(aq) | |
| Boiling point/Freezing point Elevation/depression | ∆T= i(K_b)(molality_solute) |
| Weight % | Wt %= (Kg solute)/ (Kg solution, which also includes the solute, or Kg total) |
| Osmotic pressure | π= iMRT i= disassociation M= Molality T= K˚ R= constant |
| To turn 25˚ C into K˚ | Just add 273.15 |
| Vapor pressure | P= iX(P_0) i= disassociation X= mole fraction of what you want P_0= pure vapor pressure of substance |
| Mole Fraction | X= #mole solute/ (total moles or moles solution, which also means total) |
| Formula for acetate | CH3COO, there is an extra H when it is acidic |
| Solubility of Gas in relation to pressure | C(concentration in terms of Molarity)= (K_H)(P_partial pressure) - note that partial pressure is related to mole fraction |
| Relation ship of solution temp, solubility, & ∆H of dissolving a solid** solute | Watch the equilibrium |
| What happens to the solubility of a gas as temp goes up? | It decreases. Can this also be explained by ∆H and the equilibrium? It should be explained by it. Remember there must be ∆H in the equilibrium because the gas goes from no interaction, as a gas, to interacting with liquid, as a liquid. |
Created by:
hlatif
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