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Chapter 4: Problem 53

Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid, (b) chromium with hydrobromic acid, (c) tin with hydrochloric acid, (d) aluminum with formic acid, \(\mathrm{HCOOH}\).

Short Answer

Expert verified
The short versions of the balanced molecular and net ionic equations for each reaction are: (a) Mn + H2SO4 -> MnSO4 + H2 Net ionic: Mn + 2H+ -> Mn2+ + H2 (b) 2Cr + 6HBr -> 2CrBr3 + 3H2 Net ionic: 2Cr + 6H+ -> 2Cr3+ + 3H2 (c) Sn + 2HCl -> SnCl2 + H2 Net ionic: Sn + 2H+ -> Sn2+ + H2 (d) 2Al + 6HCOOH -> 2Al(HCOO)3 + 3H2 Net ionic: 2Al + 6H+ -> 2Al3+ + 3H2

Step by step solution

01

Write the unbalanced molecular equation

\(Mn + H_2SO_4 \rightarrow MnSO_4 + H_2\)
02

Balance the molecular equation

The equation is already balanced.
03

Write the ionic equation

\(Mn + 2H^+ + SO_4^{2-} \rightarrow Mn^{2+} + SO_4^{2-} + H_2\)
04

Write the net ionic equation

\(Mn + 2H^+ \rightarrow Mn^{2+} + H_2\) (b) Reaction between chromium and hydrobromic acid
05

Write the unbalanced molecular equation

\(Cr + HBr \rightarrow CrBr_3 + H_2\)
06

Balance the molecular equation

\(2Cr + 6HBr \rightarrow 2CrBr_3 + 3H_2\)
07

Write the ionic equation

\(2Cr + 6H^+ + 6Br^- \rightarrow 2Cr^{3+} + 6Br^- + 3H_2\)
08

Write the net ionic equation

\(2Cr + 6H^+ \rightarrow 2Cr^{3+} + 3H_2\) (c) Reaction between tin and hydrochloric acid
09

Write the unbalanced molecular equation

\(Sn + HCl \rightarrow SnCl_2 + H_2\)
10

Balance the molecular equation

\(Sn + 2HCl \rightarrow SnCl_2 + H_2\)
11

Write the ionic equation

\(Sn + 2H^+ + 2Cl^- \rightarrow Sn^{2+} + 2Cl^- + H_2\)
12

Write the net ionic equation

\(Sn + 2H^+ \rightarrow Sn^{2+} + H_2\) (d) Reaction between aluminum and formic acid
13

Write the unbalanced molecular equation

\(Al + HCOOH \rightarrow Al(HCOO)_3 + H_2\)
14

Balance the molecular equation

\(2Al + 6HCOOH \rightarrow 2Al(HCOO)_3 + 3H_2\)
15

Write the ionic equation

\(2Al + 6H^+ + 6HCOO^- \rightarrow 2Al^{3+} + 6HCOO^- + 3H_2\)
16

Write the net ionic equation

\(2Al + 6H^+ \rightarrow 2Al^{3+} + 3H_2\)

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Most popular questions from this chapter

An \(8.65-g\) sample of an unknown group 2 metal hydroxide is dissolved in $85.0 \mathrm{~mL}$ of water. An acid-base indicator is added and the resulting solution is titrated with \(2.50 \mathrm{M}\) \(\mathrm{HCl}(a q)\) solution. The indicator changes color, signaling that the equivalence point has been reached, after \(56.9 \mathrm{~mL}\) of the hydrochloric acid solution has been added. (a) What is the molar mass of the metal hydroxide? (b) What is the identity of the metal cation: \(\mathrm{Ca}^{2+}, \mathrm{Sr}^{2+},\) or $\mathrm{Ba}^{2+} ?$

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate (b) lead nitrate and lithium sulfide (c) ammonium phosphate and calcium chloride

(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?

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) $\mathrm{NH}_{4} \mathrm{I}\( and \)\mathrm{CuCl}_{2},\( (b) LiOH and \)\mathrm{MnCl}_{2}$, (c) \(\mathrm{K}_{3} \mathrm{PO}_{4}\) and \(\mathrm{CoSO}_{4}\)

An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of \(\mathrm{NaCl}\) of the same concentration. Which of the following substances could the unknown be: \(\mathrm{KOH}\), $\mathrm{NH}_{3}, \mathrm{HNO}_{3}, \mathrm{KClO}_{2}, \mathrm{H}_{3} \mathrm{PO}_{3}, \mathrm{CH}_{3} \mathrm{COCH}_{3}$ (acetone)?
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