There are a few common acids and bases that you should know:
Strong Acids
Hydrochloric acid:
HCl (aq) --> H+ (aq) + Cl- (aq) Hydrochloric acid + water --> Hydrogen ions and chlorine ions. Nitric acid: HNO3 (aq) --> H+ (aq) + NO3- (aq) Nitric acid + water --> Hydrogen ions + nitrate ions Sulfuric acid: H2SO4 (aq) --> H+ (aq) + HSO4- (aq) Sulfuric acid + water --> hydrogen ions + sulfate ions |
Weak AcidHydrofluoric acid:
HF (aq) --> H+ (aq) + F- (aq) Hydrofluoric acid + water --> hydrogen ions + fluorine ions |
Strong BasesSodium hydroxide:
NaOH (aq) --> Na+ (aq) + OH- (aq) Sodium hydroxide + water --> Sodium ions + hydroxide ions Potassium Hydroxide: KOH (aq) --> K+ (aq) + OH- (aq) potassium hydroxide + water --> potassium ions + hydroxide ions Calcium hydroxide: Ca(OH)2 (aq) --> Ca+2 (aq) + 2OH- (aq) calcium hydroxide + water --> calcium ions + hydroxide ions |
Weak BaseAmmonia:
NH3 (aq) + H2O (l) --> NH4+ (aq) OH- (aq) Ammonium hydroxide + water --> Ammonium ions + hydroxide ions |
Difference between strong and weak acid:
The difference between a strong and a weak acid is that a strong acid can dissociate in water to form more H+ ions then a weak acid. Therefore, an acid with a higher pH is stronger then an acid with a lower pH. |
Difference between strong and weak base:
The difference between a strong and a weak base is that a strong base can dissociate in water to form more OH- ions then a weak base. |
Concentration
Concentration is the amount of substance per unit volume.
Molarity however is the most common way of finding a particular concentration of a solution. Molarity = moles per liter. The equation is written as: M= m/L
For example: If there was 5 liters of a substance with 10 moles of a solute the molarity would be 2.
Molarity however is the most common way of finding a particular concentration of a solution. Molarity = moles per liter. The equation is written as: M= m/L
For example: If there was 5 liters of a substance with 10 moles of a solute the molarity would be 2.