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TWHS Solutions
Solutions
| 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 |
Created by:
dshepard
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