Principles Of Chem Review Flashcards
What are the common poly atomic ions that are singly charged anions?
- Acetate (CH3CO2-)
- Cyanide (CN-)
- Hypochlorite (ClO-)
- Chlorite (ClO2-)
- Chlorate (ClO3-)
- Perchlorate (ClO4-)
- Dihydrogen phosphate (h2PO4-)
- Hydrogen carbonate (HCO3-)
- Hydrogen sulfate (HSO4-)
- Hydroxide (OH-)
- Permanganate (MnO4-)
- Nitrite (NO2-)
- Nitrate (NO3-)
What is the poly atomic ion that is a cation?
NH4+
What are the poly atomic ions that are doubly charged anions?
- Carbonate (CO3 2-)
- Chromate ( CrO3 2-)
- Dichromate (Cr2O7 2-)
- Peroxide (O2 2-)
- Hydrogen phosphate ( HPO4 2-)
- Sulfite ( SO3 2-)
- Sulfate (SO4 2-)
- Thiosulfate ( S2O3 2-)
What is the common poly atomic ion that is a triply charged anion?
Phosphate ( PO4 3-)
What are the 10 common strong electrolytes?
Hcl, hbr, hi, hclo4, hno3, h2so4, kbr, nacl, naoh, koh
What are some common weak electrolytes?
Ch3co2h and hf
What are some common nonelectrolytes?
H20, ch3oh, c2h5oh, c12h22o11
What is the rule for cations for solubility for ionic compounds in water?
It is probably soluble if it contains…
- Li+
- Na+
- K+
- Rb+
- Cs+
- NH4+
A compound is probably soluble if it contains one of the following anions?
Halides: cl-, br-, I- Nitrate: no3- Perchlorate clo4- Acetate ch3co2- Sulfate so4 2-
What are the anions that don’t work in the specific groups?
Ag+ hg2+ pb2+ ba2+ hg2 2+ pb2+
Name some common strong acids
Hclo4- perchloric acid H2so4 - sulfuric acid Hbr - hydrobromic acid Hcl- hydrochloric acid Hno3- nitric acid
What are some common weak acids
H3po4- phosphoric acid
Hf- hydrofluoric acid
Ch3co2h- acetic acid
What are some common strong bases
Naoh sodium hydroxide
Koh potassium hydroxide
Ba(oh)2 barium hydroxide
Ca(oh)2 calcium hydroxide
What are some common weak bases?
Nh3 ammonia
Common oxoacids
Hno2 nitrous acid Hno3 nitric acid H3po4 phosphoric acid H2so3 sulfurous acid H2so4 sulfuric acid Hclo hypochlorous acid Hclo2 chlorous acid Hclo3 chloric acid Hclo4 perchloric acid
Common oxoanions
No2- nitrite ion No3- nitrate ion Po4 3- phosphate ion So3 2- sulfite ion So4 2- sulfate ion ClO- hypochlorite ion Clo2- chlorite ion Clo3- Chlorate ion Clo4- perchlorate ion
Molarity
Mol solute / L solution
Mole fraction
Mole a/ mole a+ mole b
Unit less
Mass %
G solvent/ g of solution (100)
Molality
Mole solute/ kg solvent
Volume percentage
Parts by volume of solute per 100 parts by volume of solution
Parts per million
Ppm - parts by mass of solute per million parts by mass of solution
Parts per billion
Ppb- parts by mass of solute per billion parts by mass of solution
Normality
N - number of equivalents of solute per liter of solution
Rate of solution-= rate of dissolution depends on 3 things…
- Nature of the solute and solvent- strength of the imf
- Temperature - higher temperatures increase the rate with which solute molecules diffuse through the solvent
- Surface area- the greater the surface area, the higher the rate of dissolution
Saturated solution
At equilibrium rate of solution= rate of crystallization
A solution containing the maximum possible amount of dissolved solute at equilibrium
Supersaturated solution
A solution containing a great than equilibrium amount of solute
Henry’s law
For solutions of gases in liquids, the solubility of a gas is directly proportional to the partial pressure of the gas above the solution
Solubility = kP
