Write balanced equation for proton transfer reaction

Question

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 

• (CH3)2NH2+
• HSeO3-

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

• C6H12O6
• NaOH
• K2SO4
• NH3

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-