Solution powerpoints NOTES

Explain the process of an aqueous solution.

Particles dissociate. The particles  turn aqueous due to attractive forces between particles and water molecules 

Explain the process of insoluble solution

Insoluble substances don’t dissolve in a solvent, like water, because their molecular structure resists interaction. This happens when forces holding the molecules of insoluble substance together are stronger than the forces exerted by the solvent. Intermolecular forces are uneven.

Explain the process of tincture solution

Solvent is alcohol, dissociate particles into molecules, attracted into alcohol. Dissolve in solution.

Explain the process of electrolytes

Molecules are separated (dissociated) each ions having a separate charge. Then it becomes mobile in the solution creating 2 currents.

As size decreases, energy (temp) increases 

Concentration is the amount of solvent in a solute

Concentrated is when there is lots of solvent relative to solvent

Diluted is when there is less solute relative to solvent

Unsaturated is when there is some solute held but more can be dissolved

Saturated is when the max solute is helped and no more can be dissolved. 

Saturated talks about the state of solution and solution already held. Solubility tells how much it potentially can hold. Solubility" refers to the potential capacity of a solvent to dissolve a solute, essentially defining the maximum amount that can be dissolved at a specific temperature and pressure. 

Supersaturated is when to much solute is held. Formed when saturated at a high temp and cool forming crystals (crystallization).

Magnetic Removal

Filtration: if solid hasn’t dissolved you can remove it with a filter or by decanting (carefully pouring liquid but keeping the solid (solvent) in the bottom of it.

Crystallization is when you heat up a solution and the liquid parts evaporate leaving solute that turned into crystals

Distilling is when you heat up solutions at different temperatures and one turns to vapor and separates from the container and goes to another container as a liquid. 

Chromatography is when you separate parts of a mixture by making each part move at different speeds across a surface, like using a paper where some parts travel further than others. You find original colors/ingredients. The process involves a "stationary phase" (the surface, like paper) and a "mobile phase" (the solvent that carries the mixture). 

Physical Property is something you can see or measure about a substance without changing into something new. Ex: Colo, size, or how easily something floats

Chemical Property is about how a substance can change and turn into something completely different when it reacts with another substance

Ex:

• HCl is soluble in water: PP (its still HCl when dissolved)

• HCl is corrosive to metals: CP because HCl reacts with the metal, changing it and creating new substances (like hydrogen gas and salt) 

• HCl neutralizes a base: CP (when HCl reacts with a base, it changes into new substances like water and salt 

Intensive (doesnt depend on how density: color, odor, conductivity, hardness, melting/freezing point, boiling point, viscosity, Buoyancy

• An intensive property is defined as the ratio of two extensive properties

Archimedes’ principle:Buoyancy: objects float because a liquid or gas pushed up on them, and how much it can push up depends on how much liquid or gas the object moves out of the way, like when a ship sinks in water until it displaces enough water to match its weight.

• Anything with a density GREATER than 1g/mL will sink, anything less will float

Viscosity is how thick/sticky a liquid is and how easily it flows, If a liquid has high viscosity, like honey, it moves slowly because thee molecules have a hard time sliding past each other. If it has a low viscosity, like water, it flows easily because molecules move around without trouble. 

When you mix something like salt or sugar (called a solute) into a liquid like water (the solvent), it changes how the liquid behaves. These changes are called colligative properties, and they depend on how many solute particles are in the liquid, not what kind of particles they are.

 Here's how adding a solute affects the liquid:

1. Lower Vapor Pressure: The liquid doesn't evaporate as quickly.

2. Lower Freezing Point: The liquid freezes at a lower temperature.

3. Higher Boiling Point: The liquid boils at a higher temperature.

4. Increased Osmotic Pressure: This affects how water moves through barriers, like in plants or cells.

Miscible liquid is when you mix liquids together and they become one liquid (cocktail). Immiscible is when you mix 2 liquids together and they don't mix/become heterogeneous (water and oil).

Henrys law is basically how if pressure increases, the solubility of a gas increases (example coke:when you see bubbles in a carbonated drink, it means the liquid is releasing dissolved gas, indicating that the gas is less soluble under the current conditions)

Electronegativities dissolve like Electronegativities

Solvation is about being lower energy when dissolved.  If mixing the two chemicals lowers the energy of the system as a whole, mixing will occur.

ionization is the process where certain substances, like nitric acid, break apart into ions when they dissolve in water, allowing the solution to conduct electricity.

Dissociation (only for ions or do we assume that the compound is an ion)

How do we know ions are present in aqueous solutions?

Ions are ELECTROLYTES

–They dissociate completely (or nearly so) into ions.

–The charges move: conduct electricity

There are also some covalent compounds that ionize enough to be electrolytes.  The best examples being strong acids.

1. Nature of Solute / Solvent. - Like dissolves like (IMF)

2. Temperature -

  i) Solids/Liquids- Solubility increases with Temperature

  Increase K.E. increases motion and collision between solute / solvent.

  ii) Gas - Solubility decreases with Temperature

  Increase K.E. result in gas escaping to atmosphere.

3. Pressure Factor -

  i) Solids/Liquids - Very little effect

  Solids and Liquids are already close together, extra pressure will not increase solubility.

  ii) Gases - Solubility increases with Pressure

  Increase pressure pushes more gas solute into solvent.

Notice that all of these aspects are physical characteristics or are related to physical changes in the material

Measuring/Defining Solubility

–A lot like describing the concentration of the solution

–Maximum grams of solute that will dissolve in 100 g of solvent at a given temperature

Solubility = (amount that dissolves)/(amount of solvent)

–Varies with temp