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Chapter 4: Problem 55

Using the activity series (Table 4.5 ), write balanced chemical equations for the following reactions. If no reaction occurs, 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.

Short Answer

Expert verified
(a) Fe + Cu(NO₃)₂ -> Fe(NO₃)₂ + Cu (b) NR (c) Sn + 2 HBr -> SnBr₂ + H₂ (d) NR (e) 2 Al + 3 CoSO₄ -> Al₂(SO₄)₃ + 3 Co

Step by step solution

01

(a) Iron metal with copper(II) nitrate

First, check the activity series to determine whether a reaction will occur. Iron (Fe) is more reactive than Copper (Cu), so a reaction will occur. Write the unbalanced equation: Fe + Cu(NO₃)₂ -> Fe(NO₃)₂ + Cu Now, balance the equation: Fe + Cu(NO₃)₂ -> Fe(NO₃)₂ + Cu.
02

(b) Zinc metal with magnesium sulfate

Check the activity series to determine whether a reaction will occur. Zinc (Zn) is less reactive than Magnesium (Mg), so no reaction will occur. Write NR.
03

(c) Hydrobromic acid with tin metal

Check the activity series to determine whether a reaction will occur. Tin (Sn) is more reactive than Hydrogen (H), so a reaction will occur. Write the unbalanced equation: Sn + HBr -> SnBr₂ + H₂ Now, balance the equation: Sn + 2 HBr -> SnBr₂ + H₂.
04

(d) Hydrogen gas with nickel(II) chloride solution

Check the activity series to determine whether a reaction will occur. Hydrogen (H) is less reactive than Nickel (Ni), so no reaction will occur. Write NR.
05

(e) Aluminum metal with cobalt(II) sulfate

Check the activity series to determine whether a reaction will occur. Aluminum (Al) is more reactive than Cobalt (Co), so a reaction will occur. Write the unbalanced equation: Al + CoSO₄ -> Al₂(SO₄)₃ + Co Now, balance the equation: 2 Al + 3 CoSO₄ -> Al₂(SO₄)₃ + 3 Co.

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Most popular questions from this chapter

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or neutralization reactions. (a) $\mathrm{P}_{4}(s)+10 \mathrm{HClO}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ (b) \(\mathrm{Br}_{2}(l)+2 \mathrm{~K}(s) \longrightarrow 2 \mathrm{KBr}(s)\) (c) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l)+3 \mathrm{O}_{2}(g) \longrightarrow 3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{CO}_{2}(g)$ (d) $\mathrm{ZnCl}_{2}(a q)+2 \mathrm{NaOH}(a q) \longrightarrow \mathrm{Zn}(\mathrm{OH})_{2}(s)+$

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) \(\mathrm{Hg}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{NH}_{4} \mathrm{OH}\), (c) \(\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\) (d) \(\mathrm{AgNO}_{3}\), (e) FeCO \(_{3}\)

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

You know that an unlabeled bottle contains an aqueous solution of one of the following: \(\mathrm{AgNO}_{3}, \mathrm{CaCl}_{2},\) or \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3} . \mathrm{A}\) friend suggests that you test a portion of the solution with \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) and then with NaCl solutions. According to your friend's logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle? (a) Barium sulfate could precipitate. (b) Silver chloride could precipitate. (c) Silver sulfate could precipitate. (d) More than one, but not all, of the reactions described in answers a-c could occur. (e) All three reactions described in answers a-c could occur.

(a) You have a stock solution of \(14.8 \mathrm{M} \mathrm{NH}_{3}\). How many milliliters of this solution should you dilute to make \(1000.0 \mathrm{~mL}\) of \(0.250 \mathrm{MNH}_{3} ?\) (b) If you take a \(10.0-\mathrm{mL}\) portion of the stock solution and dilute it to a total volume of \(0.500 \mathrm{~L},\) what will be the concentration of the final solution?
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