A student added 1 liter of a 1.0\(M\) \(\mathrm{KCl}\) solution to 1 liter of a 1.0 \(M\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) solution. A lead chloride precipitate formed, and nearly all of the lead ions disappeared from the solution. Which of the following lists the ions remaining in the solution in order of decreasing concentration? (A) \(\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{K}^{+}\right]>\left[\mathrm{Pb}^{2+}\right]\) (B) \(\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{Pb}^{2+}\right]>\left[\mathrm{K}^{+}\right]\) (C) \(\left[\mathrm{K}^{+}\right]>\left[\mathrm{Pb}^{2+}\right]>\left[\mathrm{NO}_{3}^{-}\right]\) (D) \(\left[\mathrm{K}^{+}\right]>\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{Pb}^{2+}\right]\)

Short Answer

Expert verified
The correct order of remaining ion concentrations from highest to lowest is: \(\left[\mathrm{NO}_{3}^{-}\right]>\left[\mathrm{K}^{+}\right]>\left[\mathrm{Pb}^{2+}\right]\). So, the answer is (A).

Step by step solution

01

Analyze the chemical reaction

The lead nitrate and potassium chloride react to form a precipitate of lead chloride and potassium nitrate. The chemical reaction is: \(\mathrm{Pb(NO}_{3})_{2} + 2\mathrm{KCl} \rightarrow \mathrm{PbCl}_{2}(s) + 2\mathrm{KNO}_{3}\).
02

Consider the moles of each ion

Initially, there are 1 mol of \(\mathrm{Pb}^{2+}\), 2 mol of \(\mathrm{NO}_{3}^{-}\), 1 mol of \(\mathrm{K}^{+}\), and 1 mol of \(\mathrm{Cl}^{-}\) in the solution. After the reaction, nearly all lead ions precipitate out, thus, the greatest concentration ions left in the solution are \(\mathrm{NO}_{3}^{-}\) and \(\mathrm{K}^{+}\), followed by the small remaining concentration of \(\mathrm{Pb}^{2+}\).
03

Identify the correct order

The order of ion concentrations from highest to lowest is therefore: \(\mathrm{NO}_{3}^{-}\), \(\mathrm{K}^{+}\) and finally, \(\mathrm{Pb}^{2+}\). The small remaining concentration of \(\mathrm{Pb}^{2+}\) is due to the slight solubility of \(\mathrm{PbCl}_{2}\).

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Most popular questions from this chapter

A gaseous mixture at \(25^{\circ} \mathrm{C}\) contained 1 mole of \(\mathrm{CH}_{4}\) and 2 moles of \(\mathrm{O}_{2}\) and the pressure was measured at 2 \(\mathrm{atm}\) . The gases then underwent the reaction shown below. \(\mathrm{CH}_{4}(g)+2 \mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) What was the pressure in the container after the reaction had gone to completion and the temperature was allowed to return to \(25^{\circ} \mathrm{C} ?\) (A) 1 atm (B) 2 \(\mathrm{atm}\) (C) 3 \(\mathrm{atm}\) (D) 4 \(\mathrm{atm}\)

In which of the following reactions is entropy increasing? (A) \(2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{SO}_{3}(g)\) (B) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow \mathrm{H}_{2}(g)+\mathrm{CO}_{2}(g)\) (C) \(\mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightarrow 2 \mathrm{HCl}(g)\) (D) \(2 \mathrm{NO}_{2}(g) \rightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g)\)

Which substance would have the highest vapor pressure? (A) Ethanol, because of the hybridization of its carbon atoms (B) Actone, because it exhibits the weakest intermolecular forces (C) Ethylene glycol, because it has the most lone pairs assigned to individual atoms (D) All three substances would have similar vapor pressure because they have a similar number of electrons.

How many moles of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) must be added to 500 milliliters of water to create a solution that has a 2 -molar concentration of the Na' ion? (Assume the volume of the solution does not change). (A) 0.5 \(\mathrm{mol}\) (B) 1 \(\mathrm{mol}\) (C) 2 \(\mathrm{mol}\) (D) 5 \(\mathrm{mol}\)

The following reaction is found to be at equilibrium at 25°C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) Which of the following would cause a reduction in the value for the equilibrium constant? (A) Increasing the amount of \(\mathrm{SO}_{3}\) (B) Reducing the amount of \(\mathrm{O}_{2}\) (C) Raising the temperature (D) Lowering the temperature

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