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Reaction 2. The second reaction is of zinc nitrate with sodium hydroxide to form insoluble white zinc hydroxide, Zn(OH)2: molecular equation: Zn(NO3)2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaNO3(aq) What is the ionic and net ionic equations for this reaction? (review text if needed) This reaction does not go to completion because the reverse reaction also is occurring to some extent. Equilibrium occurs when the speeds of both forward and reverse reactions are equal. K = • How would the relative amount of Zn2+ be changed by increasing the OH- concentration? • What happens to the concentration of the [OH-] ion in solution if HCl were added to the solution? (Remember: H+ + OH- → H2O) • Therefore, would the equilibrium shift to the left or right if HCl were added? ___________ Obtain 3 small test tubes and make the following: 1.5 mL of 0.1 M Zn(NO3)2. 1.5 mL of 6 M NaOH. 1.5 mL of 6 M HCl. Take the test tube with your Zn(NO3)2 solution and add 1–3 drops of 6 M NaOH to it. Mix well using a clean stirring rod or carefully shake the lower section of the test tube. Caution: The drops vary in size due to the different droppers, be sure to add reagents drop by drop, stir, and make careful observations after each drop or two. • Does a precipitate (cloudiness) form? • What compound is precipitating? Add 3–4 drops of 6 M hydrochloric acid (HCl) and mix well. Does the amount of precipitate increase or decrease? Is the equilibrium shifting to the left (reactant) or right? Carefully add 6 M NaOH until a precipitate (cloudiness) reforms. • What compound is precipitating? Now, add 5–6 more drops of 6 M NaOH to the test tube (NaOH needs to be in excess). • Does the amount of precipitate increase or decrease?

          Reaction 2.
The second reaction is of zinc nitrate with sodium hydroxide to form insoluble white zinc hydroxide, Zn(OH)2:
molecular equation:
Zn(NO3)2(aq) + 2 NaOH(aq) → Zn(OH)2(s) + 2 NaNO3(aq)

What is the ionic and net ionic equations for this reaction? (review text if needed)

This reaction does not go to completion because the reverse reaction also is occurring to some extent. Equilibrium occurs when the speeds of both forward and reverse reactions are equal.
K =

• How would the relative amount of Zn2+ be changed by increasing the OH- concentration?

• What happens to the concentration of the [OH-] ion in solution if HCl were added to the solution? (Remember: H+ + OH- → H2O)

• Therefore, would the equilibrium shift to the left or right if HCl were added? ___________

Obtain 3 small test tubes and make the following:

1.5 mL of 0.1 M Zn(NO3)2.
1.5 mL of 6 M NaOH.
1.5 mL of 6 M HCl.

Take the test tube with your Zn(NO3)2 solution and add 1–3 drops of 6 M NaOH to it. Mix well using a clean stirring rod or carefully shake the lower section of the test tube. Caution: The drops vary in size due to the different droppers, be sure to add reagents drop by drop, stir, and make careful observations after each drop or two.

• Does a precipitate (cloudiness) form?
• What compound is precipitating?

Add 3–4 drops of 6 M hydrochloric acid (HCl) and mix well. Does the amount of precipitate increase or decrease? Is the equilibrium shifting to the left (reactant) or right?

Carefully add 6 M NaOH until a precipitate (cloudiness) reforms.
• What compound is precipitating?

Now, add 5–6 more drops of 6 M NaOH to the test tube (NaOH needs to be in excess).
• Does the amount of precipitate increase or decrease?

Added by Wayne W.

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