Chem Chapters 5 & 6
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40 terms
Terms | Definitions |
|---|---|
 solute | what is being dissolved |
| solvent | thing dissolving the solute (ie- water) |
| solution | homogeneous mixture of solvent and solute |
| concentration | amount of solute relative to solvent solution |
| saturated solution | solution that contains maximum amount of solute |
| solubility | amount of solute required to give a saturated solution |
| precipitant | solid that forms in solution |
| precipitation reaction | reaction that produces precipitant |
| electrolytes | substance that dissolves in water to produce ions and therefore conduct electricity |
| ionic compounds and few molecular compounds are... | electrolytes |
| non-electrolyte | opposite of electrolyte (substance that does NOT dissolve in water to produce ions and DOES NOT conduct electricity) |
| examples of non-electrolytes | molecular compounds (except HCl, HBr, etc) |
| strong electrolyte | substance dissociates in water to LARGE extent |
| weak electrolyte | substance dissociates in water to a LIMITED extent (ex- HF, CH3CO2H) |
| Steps to writing a net ionic equation | 1. determine the products, 2. balance equation, 3. determine if you have a precipitant |
| Acids (according to Arrhenius) | dissociates in water to produce H+ reacts with water to produce H3O+ (hydronium ion) |
| Base (according to Arrhenius) | dissociates in water to produce OH- |
| strong acids and strong bases | have strong electrolytes |
| examples of strong acids | H2SO4, HCl, HBr, HNO3 |
| examples of strong bases | NaOH, COH, Ca(OH)2 |
| examples of weak acids | H3PO4, HF, CH3CO2H |
| examples of weak bases | NH3 |
| naming for binary acids | hydrogen + element |
| example of binary acid nomenclature: HCl | hydro chloric acid |
| naming for exoacids | hydrogen, oxygen, and element (name based on polyatomic ion) |
| formula for Molarity (M) | M = (moles of solute in moles) / (volume of solution in L) |
| dilution of solutions formula | McVc = MolVol |
| solubility rules for soluble compounds #1 | all compounds of group 1A are soluble |
| solubility rules for soluble compounds #2 | all salts containing NH4+, NO3 -, ClO4 -, ClO3 - , and C2H3O2 - are SOLUBLE |
| solubility rules for soluble compounds #3 | all salts containing Cl-, Br-, and I- are soluble EXCEPT when combined with Pb^ 2+, Hg2^ 2+, and Ag + |
| solubility rules for soluble compounds #4 | all salts containing SO4^ 2- are soluble except those containing Pb^ 2+, Ca^ 2+, Sr^ 2+, Hg2^ 2+, and Ba^ 2+ |
| solubility rules for insoluble compounds #1 | all metal hydroxides and all metal oxides are insoluble except those of group 1A and those of Ca^ 2+, Sr^ 2+, and Ba^ 2+ |
| solubility rules for insoluble compounds #2 | all salts containing PO4^ 3-, CO3^ 2-, SO3^ 2-, and S^ 2- are INSOLUBLE exxcept those of group 1A and NH4 + |
| Chapter 6 | Oxidation-reaction Reactions (Redox) |
| oxidation | loss of electrons |
| reduction | gain of electrons |
| redox reaction | involves both oxidation and reduction and transfer of electrons |
| oxidizing agent | species that gets reduced |
| reducing agent | species that gets added to (opposite of oxidizing agent) |
| oxidizing number | way of indicating whether an atom is electron rich, poor, or neutral |
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