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Chapter 4: Problem 56

Using the activity series (Table 4.5 ), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Nickel metal is added to a solution of copper(II) nitrate; (b) a solution of zinc nitrate is added to a solution of magnesium sulfate; (c) hydrochloric acid is added to gold metal; (d) chromium metal is immersed in an aqueous solution of cobalt(II) chloride; (e) hydrogen gas is bubbled through a solution of silver nitrate.

Short Answer

Expert verified
(a) \(Ni(s) + Cu(NO_3)_2(aq) \rightarrow Ni(NO_3)_2(aq) + Cu(s)\) (b) NR (c) NR (d) \(Cr(s) + 2CoCl_2(aq) \rightarrow 2Co(s) + CrCl_2(aq)\) (e) \(2AgNO_3(aq) + H_2(g) \rightarrow 2Ag(s) + 2HNO_3(aq)\)

Step by step solution

01

Use the activity series

In order to determine if a reaction will occur or not, we first need to consult the activity series of elements. From the table, the order of elements from the most to the least reactive is: K > Ca > Na > Mg > Al > Zn > Fe > Ni > Sn > Pb > H > Cu > Hg > Ag > Pt > Au. Now, let's discuss each subpart.
02

(a) Nickel metal is added to a solution of copper(II) nitrate

Since Nickel (Ni) is more reactive than Copper (Cu), a reaction will occur. Using the activity series, we can deduce that Nickel will displace Copper from its nitrate solution: Ni(s) + Cu(NO3)2(aq) -> Ni(NO3)2(aq) + Cu(s)
03

(b) A solution of zinc nitrate is added to a solution of magnesium sulfate

In this case, Zinc (Zn) is less reactive than Magnesium (Mg), so no reaction will occur. Thus, we simply write "NR."
04

(c) Hydrochloric acid is added to gold metal

Gold (Au) is one of the least reactive metals, and Hydrogen (H) is relatively more reactive. So, no reaction will occur when hydrochloric acid (which contains hydrogen ions) is added to gold metal. Thus, we simply write "NR."
05

(d) Chromium metal is immersed in aqueous solution of cobalt(II) chloride

Chrome (Cr) is more reactive than Cobalt (Co), so it will displace the latter from its chloride solution: Cr(s) + 2CoCl2(aq) -> 2Co(s) + CrCl2(aq)
06

(e) Hydrogen gas is bubbled through a solution of silver nitrate

Hydrogen (H) is more reactive than Silver (Ag), so it will displace the latter from its nitrate solution: 2AgNO3(aq) + H2(g) -> 2Ag(s) + 2HNO3(aq) In summary, the balanced chemical equations for each subpart are: (a) Ni(s) + Cu(NO3)2(aq) -> Ni(NO3)2(aq) + Cu(s) (b) NR (c) NR (d) Cr(s) + 2CoCl2(aq) -> 2Co(s) + CrCl2(aq) (e) 2AgNO3(aq) + H2(g) -> 2Ag(s) + 2HNO3(aq)

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Most popular questions from this chapter

Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3}(a q)\) and \(\mathrm{MgSO}_{4}(a q)\) (b) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) and \(\mathrm{Na}_{2} \mathrm{~S}(a q)\) (c) \(\left(\mathrm{NH}_{4}\right)_{3} \mathrm{PO}_{4}(a q)\) and \(\mathrm{CaCl}_{2}(a q)\)

When methanol, \(\mathrm{CH}_{3} \mathrm{OH},\) is dissolved in water, a nonconducting solution results. When acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) dissolves in water, the solution is weakly conducting and acidic in nature. Describe what happens upon dissolution in the two cases, and account for the different results.

Indicate the concentration of each ion present in the solution formed by mixing (a) \(42.0 \mathrm{~mL}\) of \(0.170 \mathrm{M} \mathrm{NaOH}\) and \(37.6 \mathrm{~mL}\) of \(0.400 \mathrm{M} \mathrm{NaOH}\), (b) \(44.0 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) and \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and \(25.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{KCl},(\mathrm {c}) 3.60 \mathrm{~g} \mathrm{KCl}\) in \(75.0 \mathrm{~mL}\) of \(0.250 \mathrm{M}\) \(\mathrm{CaCl}_{2}\) solution. Assume that the volumes are additive.

Using the activity series (Table 4.5 ), write balanced chemical equations for the following reactions. If no reaction occurs, simply write NR. (a) Iron metal is added to a solution of copper(II) nitrate; (b) zinc metal is added to a solution of magnesium sulfate; (c) hydrobromic acid is added to tin metal; (d) hydrogen gas is bubbled through an aqueous solution of nickel(II) chloride; (e) aluminum metal is added to a solution of cobalt(II) sulfate.

Federal regulations set an upper limit of 50 parts per million (ppm) of \(\mathrm{NH}_{3}\) in the air in a work environment [that is, 50 molecules of \(\mathrm{NH}_{3}(g)\) for every million molecules in the air]. Air from a manufacturing operation was drawn through a solution containing \(1.00 \times 10^{2} \mathrm{~mL}\) of \(0.0105 \mathrm{M} \mathrm{HCl}\). The \(\mathrm{NH}_{3}\) reacts with \(\mathrm{HCl}\) as follows: $$\mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q)$$ After drawing air through the acid solution for \(10.0 \mathrm{~min}\) at a rate of \(10.0 \mathrm{~L} / \mathrm{min},\) the acid was titrated. The remaining acid needed \(13.1 \mathrm{~mL}\) of \(0.0588 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point. (a) How many grams of \(\mathrm{NH}_{3}\) were drawn into the acid solution? (b) How many ppm of \(\mathrm{NH}_{3}\) were in the air? (Air has a density of \(1.20 \mathrm{~g} / \mathrm{L}\) and an average molar mass of \(29.0 \mathrm{~g} / \mathrm{mol}\) under the conditions of the experiment.) (c) Is this manufacturer in compliance with regulations?
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