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Chapter 13: Q34 E (page 752)

What would happen to the color of the solution in part (b) if a small amount of \({\bf{NaOH}}\) were added and \({\bf{Fe}}\left( {{\bf{OH}}} \right){\bf{3}}\) precipitated? Explain your answer.

Short Answer

Expert verified


The solution will become lighter.

Step by step solution

01

Step 1: What would happen to the color of the solution.

The reaction

  • The solution is dark because of the concentration of\({\rm{Fe}}{({\rm{SCN}})^{2 + }}\)
    A small amount of \({\rm{NaOH}}\)were added and\(\begin{array}{l}{\rm{Fe}}{({\rm{OH}})_3}\\\end{array}\)precipitated

The formation of\(\begin{array}{l}{\rm{Fe}}{({\rm{OH}})_3}\\\end{array}\), decreases the concentration of\({\rm{F}}{{\rm{e}}^{3 + }}\).
The decrease in the\({\rm{F}}{{\rm{e}}^{3 + }}\)concentration shifts the equilibrium to the left, decreasing the concentration of\({\rm{Fe}}{({\rm{SCN}})^{2 + }}\), and the solution becomes lighter.

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Most popular questions from this chapter

Nitrogen and oxygen react at high temperatures.

(a) Write the expression for the equilibrium constant \(\left( {{K_c}} \right)\)for the reversible reaction

\(\Delta H = 181kJ\)

(b) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if more \({O_2}\)is added?

(c) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if \({N_2}\)is removed?

(d) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if \(NO\)is added?

(e) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\)at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if the temperature of the system is increased?

(g) What will happen to the concentrations of \({N_2},{O_2}, and\;NO\) at equilibrium if a catalyst is added?

Question: Butane exists as two isomers, n−butane and isobutane.

\({K_P} = 2.5\;at\;2{5^o}C\)

What is the pressure of isobutane in a container of the two isomers at equilibrium with a total pressure of 1.22 atm?

For which of the reactions in Exercise 13.16 does \({K_c}\) (calculated using concentrations) equal \({K_p}\)(calculated using pressures)?

(a) \({N_2}(g) + 3{H_2}(g)\rightleftharpoons 2N{H_3}(g)\)

(b) \(4N{H_3}(g) + 5{O_2}(g)\rightleftharpoons 4NO(g) + 6{H_2}O(g)\)

(c) \({N_2}{O_4}(g)\rightleftharpoons 2N{O_2}(g)\)

(d) \(C{O_2}(g) + {H_2}(g)\rightleftharpoons CO(g) + {H_2}O(g)\)

(e) \(N{H_4}Cl(s)\rightleftharpoons N{H_3}(g) + HCl(g)\)

(f) \(2\;Pb{\left( {N{O_3}} \right)_2}(s)\rightleftharpoons 2PbO(s) + 4N{O_2}(g) + {O_2}(g)\)

(g) \(2{H_2}(g) + {O_2}(g)\rightleftharpoons 2{H_2}O(l)\)

(h) \({S_8}(g)\rightleftharpoons 8\;S(g)\)

Question: In a 3.0-L vessel, the following equilibrium partial pressures are measured: \({{\rm{N}}_2}\),190 torr;\({{\rm{H}}_2}\), 317 torr;\({\rm{N}}{{\rm{H}}_3}\)\(1.00 \times {10^3}\)torr.

  1. How will the partial pressures of\({{\rm{H}}_2},{{\rm{N}}_2}\)and \({\rm{N}}{{\rm{H}}_3}\)change if \({{\rm{H}}_2}\) is removed from the system? Will they increase, decrease, or remain the same?
  2. Hydrogen is removed from the vessel until the partial pressure of nitrogen, at equilibrium, is 250 torr. Calculate the partial pressures of the other substances under the new conditions.

How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each?

a. \(2{\rm{N}}{{\rm{H}}_3}(g)\rightleftharpoons {{\rm{N}}_2}(g) + 3{{\rm{H}}_2}(g)\) \({\rm{\Delta }}H = 92{\rm{kJ}}\)

b. \({{\rm{N}}_2}(g) + {{\rm{O}}_2}(g)\rightleftharpoons 2{\rm{NO}}(g)\) \({\rm{\Delta }}H = 181{\rm{kJ}}\)

c. \(2{{\rm{O}}_3}(g)\rightleftharpoons 3{{\rm{O}}_2}(g)\) \({\rm{\Delta }}H = - 285{\rm{kJ}}\)

d.\({\rm{CaO(s) + C}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}}\rightleftharpoons {\rm{CaC}}{{\rm{O}}_{\rm{3}}}{\rm{(s)}}\) \({\rm{\Delta }}H = - 176{\rm{kJ}}\)
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