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Net Ionic Equations, Self-Ionization, Equilibrium, Conjugate Pairs and Isoelectronic Ions

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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)

2. Define the following terms:
(a.) conjugate acid-base pairs
(b.) self-ionization
(c.) amphirotic

3. Write a balanced net ionic equation for the reaction of each of the following compounds with water
(a.) NH4NO3
(b.) KCN
(c.) NaHSO4

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

5. Using liquid ammonia as a solvent what is
(a.) the strongest acid
(b.) the strongest base

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.

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

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

9. Identify the following oxyanions as neutral, weakly basic, moderately basic, or strongly basic: {see attachment}

10. The ion XeO64- is moderately basic. What degree of basicity would you expect for the isoelectronic ions: {see attachment}

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