1. Label the Bronsted Lowry acids and bases, tell which equations are conjugate acid base pairs
- CO3^2- (aq)+ HCl(aq)>HCO3-(aq)+Cl-(aq)
- H3PO4(aq)+NH3(aq)>H2PO4-(aq)+NH4+(aq)
- NH4+(aq)+ CN-(aq)<>NH3(aq)+HCN(aq)
- HBr(aq)+OH-(aq)>H2O(l)+Br-(aq)
- H2PO4-(aq)+N2H4(aq)<>HPO4^2-(aq)+N2H5+(aq)
2. Write the formula for the conjugate bases
3.Write balanced equation for proton transfer reaction. Indicate the conjugate pairs and determine the direction for each equilibrium
- HCl and PO4^3-
- HCN and SO4^2-
- HClO4 and NO2-
- CH3O- and HF
4. Write and equation for the dissolving of the following solutes in water. Determine whether the resultant solution will have mainly ions, molecules or both
5. Write equation for the ionization of the following acids in water, use a double headed arrow to indicate a weak acid
- Gaseous HF, weak acid
- Gaseous HCl, strong acid
- Liquid HNO3, strong acid
6. Write equations for the ionization of the following bases in water
- Gaseous NH3 weak base
- Solid Mg(OH)2 strong base
- Solid NaOH strong base
7. Write neutralization equations for the reactions
- hydrochloric acid and magnesium hydroxide
- sulfuric acid and ammonia
- phosphoric acid and sodium hydroxide
- sulfuric acid and sodium hydroxide
- nitric acid and potassium hydroxide
8. State whether each of following represents a buffer system and explain why or why not
- HCl and NaCl
- K2SO4
- H2CO3
- H2CO3 and NaHCO3
9. Solutions at 25 C, Find H3O+, OH-, pH
- OH-= 1.0x10^-12 Find H3O+ and pH
- pH 8.32 find H3O+ and OH-
- pH 7 find H3O+ and OH-