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Chapter 11
General Chemistry 2 Spring Semester 2026
| Question | Answer |
|---|---|
| What is miscibility? | The ability to mix without separating into two liquids |
| What is miscibility's rule of thumb? What does this mean? | Like dissolves like Polar substances dissolve in polar solvents Non-polar substances dissolve in non-polar solvents |
| What does it mean when two liquids can't mix without sperating? | Immiscibility |
| What is a solution? | A homogeneous mixture of two or more substances |
| What is the majority component of a solution called? | Solvent |
| What is the minority component of a solution called? | Solute |
| What are solute-solute interactions? | Attractive forces between the solute particles |
| What are solute-solvent ineractions? | Attractive forces between the solute particles and solvent particles |
| What happens when the solute and solvent attractions are strong enough? | The solute will dissolve, or mix with solvent particles |
| Dissolve definition | Mix with solvent particles |
| What is a strong electrolyte (definition)? | When a solute completely dissociates into ions in water |
| What are examples of strong electrolytes? | Ionic compounds and strong acids Strong bases KBr, NaCl H2SO4 (only the first H is strong, second is weak) |
| What is a weak electrolyte (definition)? | When a solute partially dissociates into ions in water |
| What are examples of weak electrolytes? | Weak acids CH3COOH, HF |
| What is a non-electrolyte (definition)? | When a solute stays intact as a molecule when dissolved in water |
| What are examples of non-electrolytes? | Most compounds of carbon Organic compounds C12H22O11, H2O CH3OH, C2H5OH |
| Define solublity | Describes the maximum concentration that can dissolve (at a temp) |
| Define saturated | A solution that is at the maximum concentration |
| Define unsaturated | Below max concentration |
| Define supersaturated | Above max concentration, dissolved |
| Define saturated solution. What does this mean? | the dissolved solute is in dynamic equilibrium with the excess undissolved solute Additional solute will not dissolve |
| Define unsaturated solution. What does this mean? | A solution containing less than. the equilibrium amount of solute More solute will dissolve |
| What is the solubility of a solute in a solvent? | The maximum amount that can dissolve in a given set of conditions |
| What happens to an equilibrium when there is a temperature change? | The equilibrium shifts; solubility in water increases with increasing temperature Low temp= less dissolves; high temp= more dissolves |
| Gas solubility | Gases generally have lower solubility in water than ionic or polar covalent solids because most are non-polar molecules |
| What affects gas solubility? | Temperature and pressure |
| How does temperature affect gas solubility? | Solubility of the gas in water decreases with rising temepratures |
| How does pressure affect gas solubility? | The higher the partial pressure of a gas above a liquid, the more soluble the gas is in the liquid |
| What is solubility of a substance? | The amount of the substance that will dissolve in a given amount of solvent |
| How does temperature affect solubility of solids? How does pressure? | Usually increases with increasing temperature No effect when pressure increases |
| How does temperature affect solubility of gases? How does pressure? | Decreases with increasing temperature Increases with increasing pressure |
| What are the three ways to express the relative amount of a solute in a solution? | Molarity Molality Mole Fraction |
| Molarity equation (M) | moles of solution/liters of solution |
| Molality equation (m) | moles of solute/kg of solvent |
| Mole fraction (X) | moles of solute/moles total moles of solute/(mole of solute+moles of solvent) |
| What do you assume when calculating the relative amount of solute in a solution | That the denominator is 1 until more information is found/given |
| What are colligative properties? | Properties that depend on the number of particles dissolved in solution, not on the type of particle |
| What are the three types of colligative properties? | Vapor pressure lowering Freezing point depression Boiling point elevation |
| What do colligative properties depend on? What is treated differently because of this? | The number of dissolved particles Electrolytes and non-electrolytes are treated differently |
| What is a non-electrolyte? | A compound that does not dissociate into ions when dissolved in water |
| What is an electrolyte? | A substance that dissociates into ions to conduct electricity when dissolved in water |
| What is the Van't Hoff Factor? What splits? | Van't Hoff Factor is when ionic compounds dissociate Everything splits apart except for polyatomic ions |
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