Solutions Unit Test

Solution

A homogenous mixture (the same throughout) of two or more substances (physical change)

Solvent

The substance present in larger quantity

Solute

The substance present in smaller quality and dissolves

Why are chemicals dissolved in a solvent to better facilitate reactions?

Being dissolved is like having maximum surface area, allows for more collisions and therefore a better reaction

Unsaturated solution

A solution that can still dissolve more solute

Saturated solution

A solution that cannot dissolve more solute

Supersaturated solution

A solution has dissolved more solute than the maximum amount possible

Water - universal solvent

Water is a bend, polar molecule that surrounds the solute, forming attractions and pulling molecules apart.

Electrolytes

When ionic compounds dissociate in water

Strong electrolytes

Conduct current efficently

Weak electrolyte

Conduct only a small current due to small amount of ions present

Non-electrolytes

No current flows, only molecules present

How does temperature affect solubility?

Greater kinetic energy, more collisions between solute and solvent  

How does agitation affect solubility?

More collisions with solute and solvent  

How does particle size effect solubility?

Increase the surface area for dissolution by grinding or crushing the solute into powder  

How does pressure affect gas solubility?

Gases have too much energy to stay in solution so gas particles must be “forced” into solution with greater pressure  

Solution Colour

The identity of a metal ion can be inferred by the colour of aqueous solution it forms

Flame test

The identity of a metal (atom or ion) can be inferred by the colour of the flame  containing the metal

Arrhenius Acid  

A substance that dissociates in water to yield H⁺ ions. Forms H₃O⁺

Arrhenius Base  

A substance that dissociates in water to yield OH^- ions  

Brönsted Lowry Acid  

Proton donor 

Brönsted Lowry Base  

Proton acceptor   

Amphiprotic substance

Can behave as an acid or base and can accept or donate protons (water)

Polyprotic Acids 

Acids that contain more than one active proton. When polyprotic acids dissociate, they donate one proton at a time                       

Oxyacids

Strength increases as number of oxygen are added to the anion  Example: H₂SO₃ versus H₂SO4 

Mineral (binary) acids

Strength decreases with electronegativity of atom bonded directly to the hydrogen. HF < HCl < HBr < HI 

Conjugate Acid Base Pairs  

Substances that differ only by a single proton. If an acid is a strong donor, then its conjugate is a weak acceptor.