Question | Answer |
What affects rate of solvation? | increase temperature of solvent, increase surface area (decrease particle size), agitate (stir) |
How does pressure affect solubility of a gas in a liquid? | Increased pressure increases the solubility of a gas. (soda can is pressurized to keep gas in solution) |
electrolyte | ionic compounds which dissociate in water to form solutions that conduct electricity; ionizes |
miscible | two LIQUIDS that are soluble in each other |
immiscible | two LIQUIDS that are NOT soluble in each other |
What makes water a good solvent? | It is polar. |
Will water dissolve ionic compounds? | Yes |
like dissolves like means | polar dissolves polar; nonpolar dissolves nonpolar |
How does temperature affect the solubility of a gas in a liquid? | As temperature increases the solubility of a gas decreases, particles are moving around too much to say in solution. |
Why do electrolytes conduct electricity? | The compound dissociates into ions. |
Saturated solution | a solution that holds the maximum amount of solvent; disoociation and crystallization are in equilibrium |
Unsaturated solution | a solution that holds less than the maximum amount of solute; more solute can be added |
Supersaturated solution | a solution that holds more than the maximum amount of solute |
What is the difference between tap water and distilled water? | Tap water has dissolved minerals, distilled water does not |
Soluble | solute can dissolve in solvent |
Insoluble | solute cannot dissolve in solvent |
Salt is dissolved in water. Compare the attraction between the sodium and chloride and between the water and sodium and chloride ions | The attraction between the water and the sodium and chloride ions is stronger than the attraction between the sodium and chloride ions that is why salt dissolves in water. |
What is the molarity of a solution in which 58g of NaCl are dissolved in 1.0L of solution? | .99 mol/L |
How many grams of KNO3 should be used to prepare 2.00 L of a 0.500 M solution? | 101 g KNO3 |
To what volume should 5.0g of KCl be diluted in order to prepare a 0.25 M solution. | 0.27 L |
If 100 mL of 18M sulfuric acid is diluted to 250 mL, what is the new concentration? | 7 M |
To what volume should 25 mL of 15 M nitric acid be diluted to prepare a 3.0 M solution? | .13 L |
Be able to read a solubility graph. | Analyze the graph, determine type of solution |
solvent | one doing the dissolving; greater portion |
solute | one being dissolved; smaller portion |
dissociation | separation of ions; splitting apart |
solvation | surrounding solute particles by solvent particles |
hydration | solvation where water is the solvent |
How would an increase in temperature affect the solubility of a liquid? | In general, the solubility would increase. |
How would an increase in temperature affect the solubility of a gas? | the solubility would decrease. |
strong electrolyte | ions dissociate completely |
weak electrolyte | ions partially dissociate |
nonelectrolyte | compounds that dissolve in solution but do not conduct electricity |