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solutions test
| Question | Answer |
|---|---|
| Solution | A homogeneous mixture composed of a solute and a solvent. |
| Solute vs. Solvent | Solute: The substance being dissolved (smaller amount). Solvent: The substance doing the dissolving (larger amount). |
| Miscible vs. Immiscible | Miscible: Two liquids that mix completely (e.g., food coloring and water). Immiscible: Liquids that do NOT mix (e.g., oil and water). |
| Electrolyte | A substance (usually an ionic compound) that produces ions when dissolved in water and can conduct electricity. |
| "Like Dissolves Like" | The rule that polar solvents dissolve polar/ionic solutes, and nonpolar solvents dissolve nonpolar solutes. |
| Unsaturated | A solution that contains less than the maximum amount of solute at a given temperature. |
| Saturated | A saturated solution already holds the maximum amount of solute possible at that temperature, so no more will dissolve. |
| Supersaturated | An unstable solution containing more than the maximum amount of solute; formed by heating then cooling slowly. |
| Temperature effect: Solids | Solubility generally increases as temperature increases. |
| Temperature & Pressure effect: Gases | Solubility decreases with higher temperature but increases with higher pressure. |
| Factors affecting Rate of Dissolving | 1. Increasing temperature, 2. Stirring/Agitation, 3. Increasing surface area (crushing). |
| Colligative Properties | Properties that depend only on the number of solute particles, not their identity. |
| The "Big Three" Effects | 1. Vapor Pressure lowers 2. Boiling Point elevates (increases) 3. Freezing Point depresses (decreases) |
| Ionic vs. Molecular Solutes | Ionic solutes have a greater effect because they break into multiple ions |
| The "Greater Effect" Rule | The higher the concentration (Molarity) or the more ions in the formula, the more the boiling/freezing points change. |
| Molarity | Molarity is defined specifically as the number of moles of solute per liter of solution. |
| According to the 'Factors Affecting Solubility' in your notes, increasing the pressure on a system would significantly increase the solubility of: | Pressure only significantly affects the solubility of gases in liquids. |
| when Using the dilution equation can you use ml and what do you | yes you can use ml and you multiply M1 by V1 and set it equal to M2 by V2 |
| Your notes mention that 'like dissolves like.' Which substance would be most soluble in the polar solvent water? | Polar substances dissolve in other polar substances due to similar intermolecular attractions. |
| Which process is occurring when the positive ends of water molecules are attracted to negative ions in a crystal lattice? | Dissolution involves the solvent particles surrounding and separating the solute ions, often called hydration or solvation. |
| Which change will cause the solubility of KNO3(s) in water to increase? | For most solid solutes, solubility increases as the kinetic energy of the solvent increases. |
| How do you know what equation to use | if theres 3 numbers use the dilution equation if 2 molarity |
| solute | describes the substance that is dissolved. It is typically the substance that is present in the smaller amount. |
| solvent | describes the substance that does the dissolving. It is typically the substance present in the larger amount and typically stays in the same phase as it was originally. |
| Miscible | describes two or more substances that are completely able to mix together, for example food coloring and water. |
| immiscible | describes when substances will not mix together, like oil and water. The place where the two substances touch is called an interface. |
| Concentrated | is used to describe solutions with a relatively large amount of solute particles. |
| Dilute | is used if there is a relatively small amount of solute particles. |
| concentration of a solution | is a description of how many solute particles are in a given amount of solvent or solution.Molarity |
| Method 1: Dissolving a solid to form a solution 1,2 | 1. Calculate the moles of solute that you will need. Convert the moles to mass using the molar mass. 2. Weigh the mass of solute. Place the weigh boat on the balance and tare to subtract the mass of the weigh boat, then add solute to the desired mass. |
| Method 1: Dissolving a solid to form a solution 3,4 | 3. Add around half of the solvent to a volumetric flask of the desired final volume for the solution. Then transfer the solute to the flask and swirl to dissolve 4. Add more solvent if needed and continue to swirl until all of the solute has dissolved |
| Method 1: Dissolving a solid to form a solution 5 | 5. Fill the volumetric flask with solvent so that the bottom of the meniscus is at the calibration line on the neck of the volumetric flask. Stopper and invert to ensure that the solution is homogeneous. |
| Method 2: Diluting a "stock" solution 1. | 1. Calculate the volume of the stock solution needed. You can do this with dimensional analysis or you can use the dilution equation. |
| Method 2: Diluting a "stock" solution 2 | 2.Measure your desired volume stock solution. Use a graduated pipette or the smallest graduated cylinder that will fit your sample.to be as accurate as possible |
| Method 2: Diluting a "stock" solution 3,4 | 3. Add approximately half of the solvent to the volumetric flask. Then add your measured stock solution. 4. Rinse the pipette or graduated cylinder with more of your solvent and add that to the volumetric flask. Mix and repeat. |
| Method 2: Diluting a "stock" solution 5 | 5. Fill the volumetric flask so that the bottom of the meniscus is at the calibration line on the neck of the volumetric flask. Stopper and invert to ensure that the solution is homogeneous. |
| the more you dissolve or how much particles leads to | higher boiling point ,lowering freezing point , and vapor pressuure lowering |
| What property of water helps an ionic solute dissolve? | Polarity. |
| Which part of a water molecule is attracted to the cation? | The negative side of the water molecule. |
| Which part of a water molecule is attracted to the anion? | The positive side of the water molecule. |
| What is the term for the process of a solute dissolving into a solvent? | Dissolution |
| When ions are surrounded by water molecules in a solution, they are described as... | Solvated. |
| What happens if you add more solute to a Saturated solution? | The extra solute will not dissolve; it will precipitate (settle) at the bottom. The concentration stays the same. |
| Concentrated | Concentrated means there is a large amount of solute compared to the solvent. |
| What happens to Boiling Point when you add solute? | It increases. |
| What happens to Freezing Point when you add solute? | It decreases. |
| When is a gas MOST soluble in water? | At high pressure and low temperature. |
| What is "dynamic equilibrium" in a solution? | When the rate of dissolving equals the rate of crystallization (occurs in saturated solutions with extra solid). |
| what are the colligative properties | Vapor pressure lowering boiling point elevation freezing point depression |
| Why does adding a solute lower vapor pressure? | Solute particles are attracted to solvent particles, giving them less kinetic energy to escape into the gas phase. Fewer gas molecules = lower pressure. |
| when theres a chart like you asked mrs scribona what do you do | if it asks most soluble you divide the grams given by the grams of water so 10/100 H2O |
| How does pressure affect the solubility of a gas in a liquid? | Solubility increases as pressure increases. Higher pressure "forces" more gas molecules into the solvent. |
| Under what specific conditions is Carbon dioxide (CO_2) most soluble in water? | High pressure and low temperature. (Think of a cold, sealed can of soda—it's highly carbonated until you open it and let it get warm!) |
| Does adding more solute make a solution freeze at a higher or lower temperature? | Lower. The more solute you add, the more you depress (lower) the freezing point. |
| What does "more solute in less solvent" (higher concentration) do to the boiling and freezing points? | Higher Boiling Point: It elevates the temperature needed to boil. Lower Freezing Point: It depresses the temperature needed to freeze |
| What happens to the concentration if you add more solute to an unsaturated solution? | The concentration increases. Because the solution isn't "full" yet, the new solute dissolves, making the solution stronger. |
| What happens if you add more solute to a supersaturated solution? | The concentration decreases. |
| How do you tell if a solution is "concentrated" or "dilute" just by looking at Table G? | Concentrated: The line or point is high up on the graph (usually 50g or more per 100g of water). Dilute: The line or point is low down on the graph (usually 10g or less) |
Created by:
Fernando.Quezada