Solubility Test Review – Flashcards
Unlock all answers in this set
Unlock answers| Supersaturated |
Containing an amount of a substance greater than that required for saturation as a result of having been cooled from a higher temperature to a temperature below that at which saturation occurs |
| Saturated |
a solution that is unable to absorb or dissolve any more of a solute at a given temperature and pressure. |
| Unsaturated |
capable of dissolving more of a solute at the same temperature. |
| Miscible |
Relating to two or more substances that can be mixed together or can dissolve into one another in any proportion without separating. |
| Immiscible |
Incapable of being mixed or blended together. |
| Hygroscopic |
a property of a substance to absorb water from its surroundings. |
| Deliquescent |
| Property that inclines a substance to absorb moisture from the atmosphere until it dissolves. |
Solvent |
| The component of a solution that is present in the greatest amount. It is the substance in which the solute is dissolved. |
Precipitate |
| an insoluble solid that emerges from a liquid solution. |
| Solute |
| the chemical dissolved in a solution. |
Concentrated |
| a solution that contains a large amount of solute relative to the amount that could dissolve |
| Dilute |
| a solution containing a relatively small quantity of solute as compared with the amount of solvent |
Homogeneous |
mixture which has uniform composition and properties throughout. Examples include Solutions and all pure substances: salt water, water, oxygen |
Heterogeneous |
made of different substances that remain physically separate. Examples include colloids such as jello and suspension such as oil and water. |
Colloid |
| a heterogeneous mixture that has particles ranging between 1 and 1000 nanometers in diameter, yet are still able to remain evenly distributed throughout the solution |
| Solution |
| homogeneous mixture of two or more substances. |
Suspension |
| a heterogeneous mixture in which particles settle out some time after their introduction |
Pure substance |
A material that is composed of only one type of particle Elements and compounds are pure substances |
| Electrolyte |
| substance that conducts electric current as a result of a dissociation into positively and negatively charged particles called ions |
| Nonelectrolyte |
| substance that does not readily ionize when dissolved or melted and is a poor conductor |
Ionic bond |
| when a positively charged ion forms a bond with a negatively charged ions and one atom transfers electrons to another. |
Non-polar covalent bond |
| a bond that occurs when two atoms share electrons equally. |
| Polar Covalent Bond |
a covalent bond between two atoms where the electrons forming the bond are unequally distributed. |
| Examples of Pure substance |
Elements (oxygen, carbon, etc.)
Compounds (water, sodium chloride) |
Examples of Solutions |
| Salt Water, Kool Aid, Soda, |
| Examples of Colloids |
| Milk, jello, fog |
| Examples of Suspensions |
| Orange juice, Salad Dressing, things that you have to shake before using to get them to mix. |
| Mole Ratio Formula |
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| Molarity Formula |
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| Molality Formula |
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| % Mass Formula |
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| % Volume Formula |
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| Freezing Point Depression Formula |
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| Boiling Point Elevation |
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| Most common solvent |
| Water |
| How does temperature effect solubility of solids? |
| In most cases an increase in temperature will result in an increases the solubility of solids |
| How does temperature effect solubility of Gases? |
| An increase in temperature will result in a decrease in the solubility of a gas. |
| How does pressure effect solubility of solids and liquids? |
| Pressure has no effect on the solubility of solids and liquids. |
| How does pressure effect solubility of gases? |
| An increase in pressure will result in an increase in gas solubility. |
| What 3 things increase the rate of solubilty of a solid? |
1. Mixing 2. Increase in Temperature 3. Breaking up the solute (increasing the surface area of the solute) |
