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Chapter 4: Problem 22

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}\) and \(\mathrm{NaOH}\), (b) \(\mathrm{NaOH}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\), (c) \(\mathrm{Na}_{2} \mathrm{~S}\) and \(\mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\).

Short Answer

Expert verified
The precipitates and balanced reactions are as follows: (a) Precipitate: \(\mathrm{Ni(OH)_{2}}\), Balanced Reaction: \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2} + 2\mathrm{NaOH} \rightarrow \mathrm{Ni(OH)_{2}}\downarrow + 2\mathrm{NaNO}_{3}\) (b) No precipitate, Balanced Reaction: \(\mathrm{NaOH} + \mathrm{K}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{KO} + \mathrm{Na}_{2}\mathrm{SO}_{4}\) (c) Precipitate: \(\mathrm{CuS}\), Balanced Reaction: \(\mathrm{Na}_{2}\mathrm{S} + \mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2} \rightarrow \mathrm{CuS}\downarrow + 2\mathrm{NaCH}_{3}\mathrm{COO} \)

Step by step solution

01

(a) Identify possible products and check solubility rules

When \(\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}\) and \(\mathrm{NaOH}\) are mixed, the possible products are \(\mathrm{Ni(OH)_{2}}\) and \(\mathrm{NaNO}_{3}\). According to solubility rules, most hydroxides are generally insoluble, with some exceptions. \(\mathrm{Ni(OH)_{2}}\) is insoluble in water, and \(\mathrm{NaNO}_{3}\) is soluble as all nitrates are soluble. Therefore, a precipitate of \(\mathrm{Ni(OH)_{2}}\) will form.
02

(a) Write the balanced equation

The balanced equation for this reaction is: \[ \mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2} + 2\mathrm{NaOH} \rightarrow \mathrm{Ni(OH)_{2}}\downarrow + 2\mathrm{NaNO}_{3} \]
03

(b) Identify possible products and check solubility rules

When \(\mathrm{NaOH}\) and \(\mathrm{K}_{2} \mathrm{SO}_{4}\) are mixed, the possible products are \(\mathrm{KO}\) and \(\mathrm{Na}_{2}\mathrm{SO}_{4}\). Both potassium compounds (like \(\mathrm{KO}\)) and sodium compounds (like \(\mathrm{Na}_{2}\mathrm{SO}_{4}\)) are soluble in water, so there is no precipitate formed in this case.
04

(b) Write the balanced equation

Since there are no precipitates, the balanced equation will be: \[ \mathrm{NaOH} + \mathrm{K}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{KO} + \mathrm{Na}_{2}\mathrm{SO}_{4} \]
05

(c) Identify possible products and check solubility rules

Given, \(\mathrm{Na}_{2} \mathrm{S}\) and \(\mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\), the possible products are \(\mathrm{CuS}\) and \(\mathrm{NaCH}_{3}\mathrm{COO}\). According to the solubility rules, most sulfides are insoluble, with some exceptions. In this case, \(\mathrm{CuS}\) is insoluble, and \(\mathrm{NaCH}_{3}\mathrm{COO}\) is soluble given most acetates are soluble. Therefore, a precipitate of \(\mathrm{CuS}\) will form.
06

(c) Write the balanced equation

The balanced equation for this reaction is: \[ \mathrm{Na}_{2}\mathrm{S} + \mathrm{Cu}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2} \rightarrow \mathrm{CuS}\downarrow + 2\mathrm{NaCH}_{3}\mathrm{COO} \]

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Most popular questions from this chapter

Can oxidation occur without accompanying reduction? Explain.

A solution of \(100.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{KOH}\) is mixed with a solution of \(200.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{NiSO}_{4}\). (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?

(a) How many grams of solute are present in \(50.0 \mathrm{~mL}\) of \(0.488 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} ?\) (b) If \(4.00 \mathrm{~g}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) is dissolved in enough water to form \(400 \mathrm{~mL}\) of solution, what is the molarity of the solution? (c) How many milliliters of \(0.0250 \mathrm{M} \mathrm{CuSO}_{4}\) contain \(1.75 \mathrm{~g}\) of solute?

You know that an unlabeled bottle contains a solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2}\), or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\). A friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with \(\mathrm{NaCl}\) solutions. Explain how these two tests together would be sufficient to determine which salt is present in the solution.

Which element is oxidized and which is reduced in the following reactions? (a) \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)\) (b) \(3 \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}(a q)+2 \mathrm{Al}(s) \longrightarrow\) \(3 \mathrm{Fe}(s)+2 \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) (c) \(\mathrm{Cl}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow \mathrm{I}_{2}(a q)+2 \mathrm{NaCl}(a q)\) (d) \(\mathrm{PbS}(s)+4 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow \mathrm{PbSO}_{4}(s)+4 \mathrm{H}_{2} \mathrm{O}(l)\)
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