Acids and Bases Test
What is a solution
-A combination of a solute and a solvent
-Anything dissolved in anthing else (liquid, gas, solid)
-A physical change not a chemical one
-Generally reversable
Universal solvent
-Water, because it's bent, polar and small
-This makes it good at aurrounding a solute and forming attractions with it
-Called hydration
Why do things dissolve
-In order for something to dissolve, the solute must be capable of being attracted to the solvent
-*some ionic compounds will not dissolve*
Predicting solubility of Molecular compounds
-Like dissolves like
-Polar dissolves polar
-Non polar dissolves non polar
-Size is also a factor (bigger things are harder to dissolve)
Dissociation Equations for ionic compounds in a solution
-Write complete equation (ensure balanced)
-Break into bits (dissociation)
-Keep only the bits reacting
Lattice enthalpy and Solubility rules
-Solubility is related to lattice enthalpy
-Ionic solids with high lattice enthalpies (small size, big charge) tend to be leas soluble in H2O
Factors that affect solubility
-Temperature
-Pressure
Temperature re solubility
-Solids have higher solubility in higher temperaturs
-Liquids are unaffected by temperature
-Gases are less soluble in high temperatures
Pressure re solubility
Changes in pressure are directly porportional to gas solubility, more pressure = more soluble
Factors that affect rate of dissolving
-Temperature
-Particle size
-Agitation
Temperature re dissolution rates
Higher temperature = more kinetic engergy, more collisions between solute and solvent
Particle size re dissolution rates
Smaller particles = more surface area, more space for collisions
Agitation re dissolution factors
-Agitation (stirring or shaking) causes more collisions
pH scale
-pH is a way of measuring the H+ in a solution
-We use H+ knowing that is H3O+
-The more H+ present, the more acidic
-The more OH- present, the more basic
-0= very acidic, 7= neutral, 14 = very basic
pH, pOH, H+, OH- calculations
pH= -log(H3O+)
pOH= -log(OH-)
pH+pOH=14
H3O+=10^(-pH)
differences between strong acids and weak acids, ways to experimentally differentiate them
l
Arrhenius
An arrhenius acid is something that donates a proton to water
An arrhenius base is a compound that increases the OH- in water
typical reactions of acids and bases
r
lab technique titration, solution preparation
r
balancing equations
nope
uncertainty
a
stoichiometry
w
solubility curve
We ball
sequential analysis using solubility table
w
Conjuagte base
the substance produced after an acid has donated its proton (hydrogen ion)
Conjugate acid
the substance formed when a base acceptes a proton (Hydrogen ion)
Bronsted-Lowry
a bronsted lowry acid is a solution that donates a proton and is a known proton donor
a bronsted lowry base is a solution that accepts a proton
Lewis
a lewis acid is any substance that can accept a pair of non bonding electrons
a lewis acid is vice versa