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Chapter 4: Problem 58

The following reactions (note that the arrows are pointing only one direction) can be used to prepare an activity series for the halogens: $$ \begin{array}{c} \mathrm{Br}_{2}(a q)+2 \mathrm{NaI}(a q) \longrightarrow 2 \mathrm{NaBr}(a q)+\mathrm{I}_{2}(a q) \\ \mathrm{Cl}_{2}(a q)+2 \mathrm{NaBr}(a q) \longrightarrow 2 \mathrm{NaCl}(a q)+\mathrm{Br}_{2}(a q) \end{array} $$ (a) Which elemental halogen would you predict is the most stable, upon mixing with other halides? (b) Predict whether a reaction will occur when elemental chlorine and potassium iodide are mixed. (c) Predict whether a reaction will occur when elemental bromine and lithium chloride are mixed.

Short Answer

Expert verified
(a) Iodine is the most stable elemental halogen when mixed with other halides. (b) Yes, a reaction will occur when elemental chlorine and potassium iodide are mixed: \[ Cl_2(aq) + 2 KI(aq) \longrightarrow 2 KCl(aq) + I_2(aq) \] (c) No, a reaction will not occur when elemental bromine and lithium chloride are mixed because bromine cannot displace chlorine from the compound.

Step by step solution

01

Reaction 1: Bromine and sodium iodide

The first reaction is: \[ Br_2(aq) + 2 NaI(aq) \longrightarrow 2 NaBr(aq) + I_2(aq) \] In this reaction, bromine (Br2) displaces iodine (I2) from its sodium iodide (NaI) compound, forming sodium bromide (NaBr).
02

Reaction 2: Chlorine and sodium bromide

The second reaction is: \[ Cl_2(aq) + 2 NaBr(aq) \longrightarrow 2 NaCl(aq) + Br_2(aq) \] In this reaction, chlorine (Cl2) displaces bromine (Br2) from its sodium bromide (NaBr) compound, forming sodium chloride (NaCl).
03

Activity series of halogens

From the given reactions, we can prepare an activity series for the halogens. In reaction 1, bromine is able to displace iodine from the compound, and in reaction 2, chlorine can displace bromine from the compound. This indicates the following activity series for the halogens: 1. Chlorine 2. Bromine 3. Iodine
04

(a) Stability of elemental halogens

According to the activity series, iodine is at the bottom, which means it is the least reactive or most stable halogen when mixed with other halides.
05

(b) Reaction between elemental chlorine and potassium iodide

From the activity series, chlorine is more reactive than iodine. So, when elemental chlorine is mixed with potassium iodide (KI), a reaction will occur, and chlorine will displace iodine from the compound. This can be represented as: \[ Cl_2(aq) + 2 KI(aq) \longrightarrow 2 KCl(aq) + I_2(aq) \]
06

(c) Reaction between elemental bromine and lithium chloride

From the activity series, bromine is less reactive than chlorine. So, when elemental bromine is mixed with lithium chloride (LiCl), no reaction will occur, as bromine cannot displace chlorine from the compound. Therefore, there is no reaction in this case, and the substances remain unchanged.

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Most popular questions from this chapter

A \(0.5895-\mathrm{g}\) sample of impure magnesium hydroxide is dissolved in \(100.0 \mathrm{~mL}\) of \(0.2050 \mathrm{MHCl}\) solution. The excess acid then needs \(19.85 \mathrm{~mL}\) of \(0.1020 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percentage by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

A person suffering from hyponatremia has a sodium ion concentration in the blood of \(0.118 \mathrm{M}\) and a total blood volume of \(4.6 \mathrm{~L}\). What mass of sodium chloride would need to be added to the blood to bring the sodium ion concentration up to \(0.138 \mathrm{M}\), assuming no change in blood volume?

Suppose you have a solution that might contain any or all of the following cations: \(\mathrm{Ni}^{2+}, \mathrm{Ag}^{+}, \mathrm{Sr}^{2+},\) and \(\mathrm{Mn}^{2+}\). Addition of HCl solution causes a precipitate to form. After filtering off the precipitate, \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution is added to the resulting solution and another precipitate forms. This is filtered off, and a solution of \(\mathrm{NaOH}\) is added to the resulting solution. No precipitate is observed. Which ions are present in each of the precipitates? Which of the four ions listed above must be absent from the original solution?

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 \(_{3}\)

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{MHCl} .\( The \)\mathrm{NH}_{3}$ reacts with HCl according to: $$ \mathrm{NH}_{3}(a q)+\mathrm{HCl}(a q) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(a q) $$ 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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