Chapter 4 Flashcards
Precipitation
Formation of a solid
Acid-base neutralization
Formation of H2O (liquid) or a gas
Solution
Homogeneous mixture that contains solute and solvent
Solute
Material dissolved in the solvent to produce the solution (you have less of it)
Solvent
The major component of the mixture (determines the phase)
Electrolyte
An aqueous solution that contains ions
Strong electrolyte
Solute dissolved in solution are all ions (100% dissociation)
Identifying strong electrolytes
Strongly conduct electricity, all ionic compounds, strong acids, and strong bases
Weak electrolyte
Solute dissolved in solution are some ions and some intact neutral molecules (not 100% dissociation)
Identifying weak electrolytes
Weakly conduct electricity, weak acids and weak bases
Non-electrolyte
Solute dissolved forms no ions in solution (0% dissociation)
Identifying non-electrolytes
Don’t conduct electricity, molecular compounds (covalent compounds)
7 strong acids
HCl, HBr, HI, H2SO4, HClO4, HClO3, HNO3
Full ionic equation
Shows how substances actually exist in solutions (split aqueous electrolytes; don’t split electrolytes of the other phases)
Net ionic equation
Shows what species actually react (remove spectator ions from full ionic equation)
Spectator ions
Ions that do not participate in the reaction (appear the same on both the reactant and product side of full ionic equation)
Acid
A substance that can donate H+
Base
A substance that can donate OH-
Strong bases
Group 1A metal hydroxides (LiOH, NaOH), group 2A metal hydroxides (Ca(OH)2)
The only weak base we need to know for Chem 1210
Ammonia (NH3)
Oxidized
A substance that loses electrons (oxidation number increases)
Reduction
A substance that gains electrons (oxidation number decreases)
The oxidation number of an element in its elemental form (H2, O2, Fe, Mg)
0
Oxidation number of a monatomic ion
Its charge (H+ is 1+, Zn2+ is 2+)
Sum of oxidation numbers of all atoms in a compound or polyatomic ion always equals…
Its overall charge
(NO3)-
N + (-2 • 3) = -1
N = 5+
Reducing agent
The reactant that is oxidized
Oxidizing agent
The reactant that is reduced
Molarity equation
Molarity (M) = moles of solute / liters of solution
Dilution
A process where more solvent is added to a solution, thus decreasing the overall concentration (moles of solute remain the same, but volume increases, which is what decreases the concentration)
Dilution of solutions equation
M(i) • V(i) = M(f) • V(f)
