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Gen Chem (5)
| Question | Answer |
|---|---|
| What is the difference between solute and solvent? | Solute = minor component dissolved in the solution; Solvent = major component that does the dissolving |
| What is the difference between unsaturated, saturated, and supersaturated solutions? | Unsaturated = less than maximum solute dissolved; Saturated = maximum solute dissolved (rate of dissolution = rate of precipitation); Supersaturated = more dissolved solute than normally possible at a given temperature/pressure |
| Always soluble | Group 1 metal cations, NO3⁻, ClO4⁻, C2H3O2⁻, NH4⁺ |
| Always insoluble | Ag⁺, Pb²⁺, Hg2²⁺, OH⁻, S²⁻, CO3²⁻, PO4³⁻ the soluble component trumps the insoluble (e.g., NH4OH is soluble because NH4⁺ is soluble) |
| What are the three categories of electrolytes? | Strong electrolytes = fully dissociate (soluble ionic compounds, strong acids, strong bases); Weak electrolytes = partially dissociate (weak acids like HF, HCN; weak bases like NH3); Non-electrolytes = do not dissociate (e.g., glucose C6H12O6) |
| What are the strong acids? | HCl, HBr, HI, HClO4, HClO3, H2SO4, HNO3 |
| What are the strong bases? | Group 1 metal hydroxides, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| What are the phase solubility rules? | Solids are more soluble at higher temperatures; Gases are more soluble at lower temperatures; Gases are more soluble at higher pressures |
| What is Beer's Law? | Beer's Law states that light absorption is directly proportional to path length and concentration of the solution. |
| What is the "like dissolves like" principle? | Polar solvents dissolve polar solutes; Non-polar solvents dissolve non-polar solutes; Polar and non-polar substances do NOT dissolve in each other |
| What are the three intermolecular forces in order of strength? | Weakest to strongest: (1) London Dispersion Forces — (2) Dipole-Dipole (3) Hydrogen Bonding — H bonded to N, O, or F interacting with an electronegative atom on another molecule |
| What are the two main classifications of matter? | Pure substances — broken into elements (one type of atom) and compounds (two or more elements, broken apart by chemical reactions); Mixtures (two or more substances non-chemically combined) — broken into heterogeneous and homogeneous (uniform) |
| What is the difference between heterogeneous and homogeneous mixtures? | Heterogeneous = non-uniform distribution, visually distinguishable components, can be physically separated (e.g., salad, oil + water); Homogeneous = uniform distribution, components cannot be identified individually (e.g., air, wine, solutions) |
| What is molarity and its formula? | Molarity (M) = moles of solute per liter of solution. Formula: M = moles of solute / liters of solution |
| What is molality and its formula? | Molality (m) = moles of solute per kilogram of solvent. Formula: m = moles of solute / kilograms of solvent |
| Why is molality preferred over molarity when temperature is involved? | Molality uses mass (unaffected by temperature), while molarity uses volume (which changes with temperature due to expansion/contraction) |
| Colligative | depend only on the concentration (number) of solute particles, not their identity (e.g., boiling point elevation, freezing point depression, vapor pressure depression, osmotic pressure) |
| Non-colligative | depend on the identity of the substance (e.g., surface tension, viscosity, solubility, volatility, color, density) |
| What is vapor-pressure depression | Adding a solute lowers the vapor pressure of the solvent because solute molecules occupy surface space, reducing evaporation. |
| What is the relationship between vapor pressure and boiling point? | Inverse relationship — as vapor pressure increases, boiling point decreases, and vice versa. Boiling point = the temperature at which vapor pressure equals atmospheric pressure |
| What is boiling point elevation? | Adding a non-volatile solute raises the boiling point because solute lowers vapor pressure, requiring more energy to boil. |
| What is the van't Hoff factor (i)? | The number of particles a solute dissociates into. Examples: NaCl → i = 2 (Na⁺ + Cl⁻); MgCl2 → i = 3 (Mg²⁺ + 2Cl⁻); glucose → i = 1 (does not dissociate) |
| What is freezing point depression? | Adding a solute lowers the freezing point because solute molecules interfere with solvent molecule arrangement during solidification. |
| What is osmotic pressure? | Osmotic pressure (Π) = pressure needed to stop osmosis (net movement of water across a semipermeable membrane from low to high solute concentration). |
| What is the difference between a molecular equation, ionic equation, and net ionic equation? | Molecular = all compounds written as intact molecules; Ionic = ionic compounds written as separate ions; Net ionic = only the ions/compounds directly involved in the reaction (spectator ions removed) |
| What are spectator ions? | Ions that do not participate in the reaction — they appear unchanged on both sides of the ionic equation and are removed when writing the net ionic equation |
Created by:
smurtab