Term
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Definition
| A homogenous mixture of two or more substances in a single phase. |
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Term
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Definition
| Occurs when the particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated. |
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Term
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Definition
| Particles that are intermediate in size between those in solutions and suspensions from mixtures known as colloidal dispersions |
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Term
| What is the Tyndall Effect? |
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Definition
| Occurs when light is scattered by colloidial particles dispersed in a transparent medium. Used to distunguish between a solution and a colloid. |
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Term
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Definition
| A substance that dissovles in water to give a solution that conducts electric current and decreases its dielectric constant. |
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Term
| What types of substances are electrolytes? |
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Definition
| Includes nonmetal-metal, ionic substances and highly polar molecules |
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Term
| What is an dielectric constant? |
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Definition
| The permitivity of free space pertaining to certain particles |
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Term
| What is a non-electrolyte? |
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Definition
| A substance that dissolves in water and does not increase the conductivity and can increase the dielectric constant. |
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Term
| What factors affect the rate of dissolution? |
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Definition
| Increasing the surface area of the solute, agitating a solution, heating a solvent. |
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Term
| What is a solution equilibrium? |
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Definition
| The physical state in which thew opposing processes of dissolution and crystallization of a solute occur at equal rates. |
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Term
| What does miscibilty refer to? |
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Definition
| Refers to the solubility of liquids into one another. |
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Term
| What is the effect of an increase in pressure of the solubility of a gas? |
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Definition
| Increases a gas's solubility in liquids. |
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Term
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Definition
| The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid. |
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Term
| What is the effect of an increase in temperature on gas solubility? |
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Definition
| Results in a decrease in gas's solubility due to an increase in kinectic energy keeping attraction from occurring |
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Term
| What is effect of an increase in temperature on a liquid's solubility? |
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Definition
| Results in an incresase in the solubility of solids |
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Term
| What is enthalpy of solution? |
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Definition
| The net amount of energy absorbed a s heat by the solution when a specific a amount of solute dissolves in a solvent. |
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Term
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Definition
| A solution is a measure of the amount of solute in a given amount of solvent or solution. |
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Term
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Definition
| The number of moles of solute in one liter of solution. |
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Term
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Definition
| The concentration of a solution expressed in moles of solute per kilogram of solvent. |
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Term
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Definition
| The separation of ions that occurs when an ionic compound dissolves. |
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Term
| What is a net ionic equation? |
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Definition
| A equation that includes only thos compounds and ions that undergo a chemical change ( form a precipitate) in a reaction in an aqueous solution. |
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Term
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Definition
| Ions that do not take part in a chemical reaction and are found in solution both before and after reaction. |
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Term
| What is a complete ionic equation? |
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Definition
| An equation that made up of a net ionic equation including spectator ions. |
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Term
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Definition
| Ions are formed from solute molecules by the action of the solvent in a process. |
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Term
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Definition
| Consists of 3 parts hydrogen and 1 part oxygen, created when hydrogen chloride is dissolved into water. |
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Term
| What is a strong electrolyte? Example? |
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Definition
| Any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions. Includes hydrogen will all halogens except fluorine. |
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Term
| What is a weak electrolyte? |
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Definition
| Any compound whose dilute aqueous solutions conduct electricity poorly; this is due to the presence of a small amount of the dissolved compound in the form of ions. |
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Term
| What is a colligative property? |
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Definition
| A property that depends on the concentration of solute parties but not on their identity. |
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Term
| What are the four colligative properties? |
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Definition
| Vapor-pressure lowering, freezing-point depression, boiling-point elevation, and osmotic pressure |
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Term
| What is a nonvolatile substance? |
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Definition
| A substance that has little tendency to become a gas under existing conditions. |
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Term
| What characterizes vapor-pressure lowering? |
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Definition
| As the number of solute particles increases in a given volume of solution, the proportion of solvent molecules decreases, allowing less water to escape, which decreases vapor pressure |
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Term
| How are molality and concentration related? |
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Definition
| Same molality = same concentration |
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Term
| What is a molal freezing-point constant? |
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Definition
| Refers to the freezing-point depression of the solvent in a 1-molality solution of a nonvolatile, nonelectrolye solute. |
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Term
| What is the freezing-point depression? |
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Definition
| The difference between the freezing point of the pure solvent and a solution of a non-electrolyte in that solvent,and it is directly proportional to the molal concentration of the solution. |
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Term
| What is the molal boiling-point constant? |
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Definition
| The boiling-point elevation of the solvent in a 1-molal solution of a nonvolatile, nonelectrolye solute. |
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Term
| What is the boling-point elevation? |
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Definition
| The difference between the boiling points of the pure solvent and a nonelectrolyte solution of that solvent, directly proportional to the molal concentration of the solution. |
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Term
| What is osmotic pressure? |
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Definition
| The external pressure that must be applied to stop osmosis. |
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Term
| What is the relationship between electrolytes and colligative properties? |
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Definition
| Electroyles increase the intensity of colligative properties by a factor of the number of ionizable parts in the electrolytes |
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Term
| What is the Van Hoff factor? |
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Definition
| Factor proportional to the total molality of all dissolved particles. |
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