Solutions Flashcards
What is a solution, solvent, solute, aqueous solution, solubility, unsaturated solution, saturated solution and a supersaturated solution?
Solution: Homogenous mixture of two or more cubstances
Solvent: the part of the solution that is present in the largest amount
Solute: the substances dissolved in a solvent
Aqueous solution: a solution that contains water
Solubility: the max amount of solute that will dissolve in a solvent at a given temperature
Unsaturated: a solution that could dissolve more solute
Saturated: a solution that cannot dissolve more solute
Supersaturated: a solution that contains more solute than a saturated solution at a given temperature
What is a soluble, sparingly soluble and insoluble solution?
Soluble: 1 g dissolves into 100 mL
Sparingly: dissolves 0.1 to 1 g into 100 mL
Insoluble: dissolves less than 0.1 g
What is water
The universal solvent. Is a bent molecule and therefore polar. Has positive h ends and negative o ends.
Explain miscible and immiscible
Miscible liquids can be combined in any proportions
Immisicble liquids do not dissolve in each other
What forces does the formation of solutions depend on?
Forces of attraction between solute particles
Forces of attractions between particles of solute and particles of solvent
Forces of attraction between so,vent particles
What happens to particles when a solute is formed
Particles of solute and so,vent are attracted. Forces between particles of solute are broken.
Explain hydrogen bonds
Can form between H atom and a negative atom from another molecule. Have only 1% of the strength from an ionic or covalent bond but stronger than any other dipole-dipole attraction.
Explain solubility of ionic compounds in water
Most are soluble in water.
Positive H ions attract negative ions. Negative O ions attract positive ions. As surface ions start to be pulled by e water, the ionic solid starts to dissolves. It dissociates into uts component ions, called hydrations.
Explain hydrated ions
Fully surrounded by water molecule. Can move in solution and therefore conduct electricity. Electrolytes.
Explain solutbility of polar molecules in water.
If the attraction between the water dipoles and dipoles of solute is stronger than dipoles within solute, the solute molecules become hydrated, they dissolve. The molecule remain intact. They are neutral and cannot conduct electricity.
Explain solubility of non polar molecules in water.
Do not dissolve in water. Only weakly attracted to water. H bonds between water molecules can’t be broken. Immisicobel.
What factors affect the solubility of ionic substances
Ion charge - compounds with ions with small charges are soluble, those with larger tend to be insoluble. (Increasing the charge increases the force holding the ions together)
Ion size- small ions bond more closely together. The bond is stronger and compounds with small ions are less soluble than larger ones.
Explain like dissolves like
Polar solvents dissolve polar or ionic solute
Non polar solvents dissolve non polar solute
Explain how temperature affects the solubility of the different states in liquids
Solid in a liquid - energy is required to break bonds in a solid. High temperatures = more energy, solubility of solids increases with temperature.
Liquid in liquid - liquid bonds don’t require much energy to break, additional energy isn’t needed. Solubility of liquid isn’t greatly affected by temperature
Gas in liquid - gas has a lot of kinetic energy. At high temperatures, dissolved gas gains energy and comes out of the solution. Solubility of gases in liquids decrease in higher temperatures.
How does pressure affect solubility.
Hardly any affect on solid or liquid solutions.
Solubility of gas is directly related to pressure of gas above the liquid. More gas molecules are soluble at higher pressures.
Ex. Opening pop bottle
