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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, or the substance present in a lesser amount. |
| What is a solvent? | The medium in which the solute is dissolved, or the substance present in a greater amount. |
| What is the most common solvent in chemistry? | Water. |
| What are four examples of solutions formed by different phase combinations? | Solid in liquid (salt water), gas in liquid (soda), gas in gas (air), and liquid in liquid (rubbing alcohol). |
| What are four distinct properties of aqueous solutions? | Solute particles do not settle, solute and solvent pass through a filter, they are always clear (even if colored), and they do not disperse light because the particles are too small. |
| What is the rule of thumb for solubility based on chemical nature? | "Like dissolves like" (polar/ionic substances dissolve in polar solvents like water; non-polar substances dissolve in non-polar solvents like benzene or carbon tetrachloride). |
| What is molecule-ion attraction? | The intermolecular attraction where water molecules surround broken-apart ions; positive ions attract to partial negative oxygen atoms, and negative ions attract to partial positive hydrogen atoms. |
| How does temperature affect the solubility of solids vs. gases in water? | As temperature increases, the solubility of solids generally increases, whereas the solubility of gases decreases. |
| How does pressure affect the solubility of solids vs. gases in a liquid? | Changes in pressure do not affect solid solubility, but an increase in pressure directly increases gas solubility. |
| Under what conditions of temperature and pressure is a gas most soluble in a liquid? | Low temperature and high pressure (Think about a cold, sealed can of soda!). |
| What is a saturated solution and how does it look on a solubility curve (Table G)? | A solution containing the maximum amount of solute allowed under given conditions; one more crystal will not dissolve, and it sits "on the curve". |
| What is an unsaturated solution and how does it look on a solubility curve (Table G)? | A solution containing less than the maximum amount of allowed solute; one more crystal will dissolve, and it sits "below the curve". |
| What is a supersaturated solution and how does it look on a solubility curve (Table G)? | A highly unstable solution containing more than the maximum amount of allowed solute; one more crystal causes other solute particles to rapidly precipitate out, and it sits "above the curve". |
| What are spectator ions? | Ions that do not participate in a chemical reaction and appear identical on both sides of a complete ionic equation. |
| What is a net ionic equation? | A balanced chemical equation that isolates the actual chemical reaction by removing all spectator ions. |
| What is the definition of heat of solution? | The amount of heat absorbed or released when dissolving one mole of a substance (kJ/mol). |
| How do you differentiate between an exothermic and endothermic heat of solution by touch? | Exothermic feels warm because it releases heat (temperature increases, negative sign); endothermic feels cool because it absorbs heat from your hand (temperature decreases, positive sign). |
| What is the relationship between the heat of dissolving and the heat of solidifying? | They are exact opposites; if dissolving a substance is endothermic, recrystallizing/solidifying it is exothermic. |
| What is the main definition of concentration? | The mathematical way to describe the exact amount of solute in a particular solution. |
| What do the relative terms "concentrated" and "dilute" mean? | "Concentrated" means a solution has a relatively large value of concentration; "dilute" means it has a relatively small value of concentration. |
| What is the primary formula for Molarity? | molarity = moles of solute / liters of solution |
| What are the rearranged formulas to find moles of solute or liters of solution using molarity? | moles of solute = molarity x liters of solution AND liters of solution = moles of solute / molarity |
| What laboratory tool is specifically used to prepare a solution correctly to an exact volume? | A volumetric flask. |
| What is the formula used for solution dilution and evaporation problems? | M1V1 = M2V2 |
| What is the formula for Percent Solution by Mass? | % solution by mass = (mass of solute / mass of solution) x 100 |
| How do you find the total mass of a solution if it isn't given directly? | mass of solution = mass of solute + mass of solvent |
| What is the formula for Percent Solution by Volume? | % solution by volume = (volume of solute / volume of solution) x 100 |
| What is the formula for Parts Per Million (ppm)? | parts per million = (grams of solute / grams of solution) x 1000000 |
| What are colligative properties? | Physical property changes that occur when a non-volatile solute is added to water, specifically causing the boiling point to increase and the freezing point to decrease. |
| Why do we add salt to roads and sidewalks during a winter storm? | The added salt lowers the freezing point of water, which helps melt existing snow/ice and prevents new water from freezing. |
| How does solution concentration relate to boiling and freezing point changes? | The more concentrated a solution is, the greater the effect: a higher concentration leads to a higher boiling point and an even lower freezing point. |
| What is the formula for calculating the change in boiling point? | change in bp = molality x 0.51 C/m |
| What is the formula for calculating the change in freezing point? | change in fp = molality x 1.86 C/m |
| What is the formula for Molality? | molality = moles of solute / kilograms of solvent |
| What is an electrolyte and why does it have a greater effect on colligative properties than a non-electrolyte? | An electrolyte is an ionic substance, acid, or base that dissociates into multiple mobile ions in water; because it produces more total particles per mole, it causes a greater boiling point elevation or freezing point depression. |
| What is a non-electrolyte? | A covalent substance (made of all nonmetals) that does not break apart into ions when dissolved in water, meaning it yields fewer particles per mole. |
Created by:
markoii