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better solutions
| Question | Answer |
|---|---|
| What is a solution? | A homogeneous mixture of a solute dissolved in a solvent |
| What is a solute? | The substance being dissolved; usually the lesser amount |
| What is a solvent? | The substance doing the dissolving; usually the greater amount |
| What is a common solvent in chemistry? | Water |
| What type of mixture is a solution? | Homogeneous mixture |
| Do solute particles settle out in a solution? | No |
| Can solute and solvent pass through a filter? | Yes |
| Are solutions clear or cloudy? | Clear |
| Do solutions scatter light? | No |
| What rule predicts whether substances dissolve in each other? | Like dissolves like |
| What kind of molecule is water? | Polar |
| What dissolves well in water? | Polar molecules and ionic compounds |
| Do nonpolar substances dissolve well in water? | No |
| What dissolves nonpolar substances? | Nonpolar solvents |
| What attracts positive ions in water? | The partially negative oxygen atoms |
| What attracts negative ions in water? | The partially positive hydrogen atoms |
| What is solubility? | The amount of solute that can dissolve in a solvent |
| What factors affect solubility? | Temperature, pressure, and chemical nature of substances |
| How does increasing temperature affect the solubility of most solids in water? | It increases |
| How does increasing temperature affect the solubility of gases in water? | It decreases |
| How does pressure affect the solubility of solids in liquids? | Little to no effect |
| How does increasing pressure affect gas solubility in liquids? | It increases |
| Under what conditions are gases most soluble in water? | Low temperature and high pressure |
| What is a saturated solution? | Contains the maximum amount of dissolved solute |
| What happens if more solute is added to a saturated solution? | It will not dissolve |
| Where is a saturated solution located on a solubility curve? | On the curve |
| What is an unsaturated solution? | Contains less than the maximum amount of dissolved solute |
| Can more solute dissolve in an unsaturated solution? | Yes |
| Where is an unsaturated solution located on a solubility curve? | Below the curve |
| What is a supersaturated solution? | Contains more dissolved solute than normally possible |
| What happens if a crystal is added to a supersaturated solution? | Excess solute rapidly crystallizes out |
| Where is a supersaturated solution located on a solubility curve? | Above the curve |
| What is a precipitate? | An insoluble solid formed in a reaction |
| What is a complete ionic equation? | An equation showing all dissolved ions separately |
| What are spectator ions? | Ions that appear unchanged on both sides of an equation |
| How do you identify spectator ions? | They are identical on both sides of the ionic equation |
| What is a net ionic equation? | The equation after spectator ions are removed |
| What is heat of solution? | The heat absorbed or released when 1 mole dissolves |
| What sign does an exothermic heat of solution have? | Negative |
| What sign does an endothermic heat of solution have? | Positive |
| If a solution feels cool while dissolving, is the process endothermic or exothermic? | Endothermic |
| If a solution feels warm while dissolving, is the process endothermic or exothermic? | Exothermic |
| In an endothermic process, does temperature increase or decrease? | Decrease |
| In an exothermic process, does temperature increase or decrease? | Increase |
| If dissolving is endothermic, what is crystallization? | Exothermic |
| If dissolving is exothermic, what is crystallization? | Endothermic |
| What is concentration? | The amount of solute in a given amount of solution |
| What does concentrated mean? | Relatively high concentration |
| What does dilute mean? | Relatively low concentration |
| Which is more concentrated: 1 M NaCl or 2 M NaCl? | 2 M NaCl |
| Which is more dilute: 0.5 M HCl or 3 M HCl? | 0.5 M HCl |
| What is molarity? | Moles of solute per liter of solution |
| What is the symbol for molarity? | M |
| What are the units of molarity? | mol/L |
| What is the molarity formula? | M = mol/L |
| How do you find moles from molarity? | mol = M × L |
| How do you find volume from molarity? | L = mol/M |
| Must volume be in liters for molarity calculations? | Yes |
| What equation is used for dilution problems? | M1V1 = M2V2 |
| What remains constant during dilution? | Moles of solute |
| What happens to molarity when water is added? | It decreases |
| What happens to molarity when water evaporates? | It increases |
| What glassware is used to prepare an accurate solution? | Volumetric flask |
| When making a solution, do you add water to the desired volume or add solute to the desired volume? | Add water until the final solution reaches the desired volume |
| What is percent by mass? | (mass of solute ÷ mass of solution) × 100 |
| What is mass of solution? | Mass of solute + mass of solvent |
| What is percent by volume? | (volume of solute ÷ volume of solution) × 100 |
| When is percent by volume commonly used? | Liquid-liquid solutions |
| What does ppm stand for? | Parts per million |
| When is ppm commonly used? | Very dilute concentrations |
| What is the ppm formula? | (mass of solute ÷ mass of solution) × 1,000,000 |
| What are colligative properties? | Properties that depend on the number of dissolved particles |
| What happens to boiling point when a nonvolatile solute is added? | It increases |
| What happens to freezing point when a nonvolatile solute is added? | It decreases |
| What is boiling point elevation? | An increase in boiling point due to dissolved particles |
| What is freezing point depression? | A decrease in freezing point due to dissolved particles |
| Why is salt spread on icy roads? | It lowers water's freezing point |
| How does concentration affect boiling point elevation? | Higher concentration causes a higher boiling point |
| How does concentration affect freezing point depression? | Higher concentration causes a lower freezing point |
| Which solution has the higher boiling point: 2 M NaCl or 3 M NaCl? | 3 M NaCl |
| Which solution has the lower freezing point: 2 M NaCl or 3 M NaCl? | 3 M NaCl |
| What is an electrolyte? | A substance that forms ions in water and conducts electricity |
| Which types of substances are electrolytes? | Ionic compounds, acids, and bases |
| What is a non-electrolyte? | A substance that does not form ions in water |
| Which types of substances are non-electrolytes? | Most covalent compounds |
| Which has a greater colligative effect at the same concentration: an electrolyte or non-electrolyte? | Electrolyte |
| Why do electrolytes have a greater colligative effect? | They produce more particles in solution |
| How many ions form when NaCl dissolves? | 2 ions |
| How many ions form when CaCl2 dissolves? | 3 ions |
| Which has the higher boiling point at equal concentration: NaCl or CaCl2? | CaCl2 |
| Which has the lower freezing point at equal concentration: NaCl or CaCl2? | CaCl2 |
| Which has the lower freezing point at equal concentration: NaCl or C12H22O11? | NaCl |
| Which solution has the lower boiling point: 1 M NaCl or 2 M NaCl? | 1 M NaCl |
| Which solution has the highest freezing point: 1 M NaCl, 2 M NaCl, 1 M C12H22O11, or 2 M C12H22O11? | 1 M C12H22O11 |
| What is the first step when comparing boiling points? | Determine whether boiling point increases or decreases with concentration |
| What is the first step when comparing freezing points? | Determine whether freezing point increases or decreases with concentration |
| What must be considered when comparing colligative properties? | Concentration and number of dissolved particles |
Created by:
markoii