Net ionic equations and self-ionization

Question

Assignment:

Question 1. Write net ionic equations to correspond with each of the following molecular equations.

(a.) HCl(aq) + NaOH(aq)    NaOH(aq) + H₂O(l)

(b.) Na₂CO₃(aq) + CoCl₂(aq)  2 NaCl(aq) + CoCO₂(s)

(c.) NH₃OH(aq) + CH₃COOH(aq)     CH₃COONH₄(aq) + H₂O(l)

Question 2. Define the following terms:

(a.) conjugate acid-base pairs

(b.) self-ionization

(c.) amphirotic

Question 3. Write a balanced net ionic equation for the reaction of each of the following compounds with water

(a.) NH₄NO₃

(b.) KCN

(c.) NaHSO₄

Question 4. Pure sulfuric acid can be used as a solvent.  Write an equilibrium to represent the self-ionization reaction.

Question 5. Using liquid ammonia as a solvent what is

(a.) the strongest acid

(b.) the strongest base

Question 6. Hydrogen fluoride behaves as a base when dissolved in pure sulfuric acid.  Write a chemical equation to represent the acid-base equilibrium and identify the conjugate acid-base pairs.

Question 7. Identify the conjugate acid-base pairs in the following equilibrium.

Question 8. Hydrogen selenide, H₂Se, is stronger acid than hydrogen sulfide.  Use bond strength arguments to explain your reasoning.

Question 9. Identify the following  oxyanions as neutral, weakly basic, moderately basic, or strongly basic:

(a.) WO₄^2-

(b.) TcO₄^-

(c.) AsO₄^3-

(d.) GeO₄^4-

Question 10. The ion XeO₆^4- is moderately basic.  What degree of basicity  would you expect for the isoelectronic ions

(a.) IO₆^5-

(b.) TeO₆^6-

Provide complete and step by step solution for the question and show calculations and use formulas.