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Chapter 21: Problem 89

Assuming that water, common reagents (acids, bases, salts), and simple laboratory equipment are available, give a practical method to prepare (a) \(\mathrm{MgCl}_{2}\) from \(\mathrm{MgCO}_{3}(\mathrm{s}) ;\) (b) \(\mathrm{NaAl}(\mathrm{OH})_{4}\) from \(\mathrm{Na}(\mathrm{s})\) and \(\mathrm{Al}(\mathrm{s}) ;\) and (c) \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) from \(\mathrm{NaCl}(\mathrm{s}).\)

Short Answer

Expert verified
The synthesis of \( \mathrm{MgCl}_{2} \) from \( \mathrm{MgCO}_{3} \) involves an acid-base reaction with \( \mathrm{HCl} \). The synthesis of \( \mathrm{NaAl}(\mathrm{OH})_{4} \) from \( \mathrm{Na}(\mathrm{s}) \) and \( \mathrm{Al}(\mathrm{s}) \) involves two steps, where \( \mathrm{Na} \) is first reacted with water to produce \( \mathrm{NaOH} \), and then \( \mathrm{Al} \) is reacted with \( \mathrm{NaOH} \) and water. The synthesis of \( \mathrm{Na}_{2} \mathrm{SO}_{4} \) from \( \mathrm{NaCl} \) involves a series of reactions with \( \mathrm{H}_{2}\mathrm{SO}_{4} \) to create \( \mathrm{Na}_{2}\mathrm{SO}_{4} \) and \( \mathrm{HCl} \).

Step by step solution

01

Preparation of MgCl2 from MgCO3

To prepare \( \mathrm{MgCl}_{2} \) from \( \mathrm{MgCO}_{3} \), an acid-base reaction needs to be performed. The mineral magnesite, \( \mathrm{MgCO}_{3} \), is heated in the presence of hydrochloric acid, \( \mathrm{HCl} \), to produce \( \mathrm{MgCl}_{2} \), \( \mathrm{CO}_{2} \) gas, and water. The reaction is as follows: \( \mathrm{MgCO}_{3}(\mathrm{s}) + 2 \mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{MgCl}_{2}(\mathrm{aq}) + \mathrm{CO}_{2}(\mathrm{g}) + \mathrm{H}_{2}\mathrm{O}(\mathrm{l}) \)
02

Preparation of NaAl(OH)4 from Na(s) and Al(s)

To prepare \( \mathrm{NaAl}(\mathrm{OH})_{4} \) from \( \mathrm{Na}(\mathrm{s}) \) and \( \mathrm{Al}(\mathrm{s}) \), a reaction with sodium hydroxide \( \mathrm{NaOH} \) is necessary. Sodium (Na) is reacted with water to produce \( \mathrm{NaOH} \) and Hydrogen \( \mathrm{H}_{2} \). The aluminium is then reacted with \( \mathrm{NaOH} \) in the presence of water to produce \( \mathrm{NaAl}(\mathrm{OH})_{4} \) and \( \mathrm{H}_{2} \). The reactions are as follows: \( 2\mathrm{Na} + 2\mathrm{H}_{2}\mathrm{O} \rightarrow 2\mathrm{NaOH} + \mathrm{H}_{2} \), and \( \mathrm{Al} + 4\mathrm{NaOH} + \mathrm{H}_{2}\mathrm{O} \rightarrow \mathrm{NaAl}(\mathrm{OH})_{4} + \mathrm{H}_{2} \)
03

Preparation of Na2SO4 from NaCl

To prepare \( \mathrm{Na}_{2} \mathrm{SO}_{4} \) from \( \mathrm{NaCl} \), a series of reactions needs to be performed. Firstly, \( \mathrm{NaCl} \) is reacted with concentrated \( \mathrm{H}_{2}\mathrm{SO}_{4} \) to form \( \mathrm{NaHSO}_{4} \). Subsequently, \( \mathrm{NaHSO}_{4} \) is reacted with \( \mathrm{NaCl} \) to form \( \mathrm{Na}_{2}\mathrm{SO}_{4} \) and \( \mathrm{HCl} \). The reaction is performed in two steps as follows: \( \mathrm{NaCl} + \mathrm{H}_{2}\mathrm{SO}_{4} \rightarrow \mathrm{NaHSO}_{4} + \mathrm{HCl} \) , and \( \mathrm{NaHSO}_{4} + \mathrm{NaCl} \rightarrow \mathrm{Na}_{2}\mathrm{SO}_{4} + \mathrm{HCl} \)

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Most popular questions from this chapter

Mono Lake in eastern California is a rather unusual salt lake. The lake has no outlets; water leaves only by evaporation. The rate of evaporation is great enough that the lake level would be lowered by three meters per year if not for fresh water entering through underwater springs and streams originating in the nearby Sierra Nevada mountains. The principal salts in the lake are the chlorides, bicarbonates, and sulfates of sodium. An approximate "recipe" for simulating the lake water is to dissolve 18 tablespoons of sodium bicarbonate, 10 tablespoons of sodium chloride, and 8 teaspoons of Epsom salt (magnesium sulfate heptahydrate) in 4.5 liters of water (although the lake water actually contains only trace amounts of magnesium ion). Assume that 1 tablespoon of any of the salts weighs about \(10 \mathrm{g} .(1 \text { tablespoon }=3\) teaspoons.) (a) Expressed as grams of salt per liter, what is the approximate salinity of Mono Lake? How does this salinity compare with seawater, which is approximately 0.438 M NaCl and 0.0512 M MgCl_? (b) Estimate an approximate pH for Mono Lake water. How does your estimate compare with the observed \(\mathrm{pH}\) of about \(9.8 ?\) Actually, the recipe for the lake water also calls for a pinch of borax. How would its presence affect the pH? [Borax is a sodium salt, \(\mathrm{Na}_{2} \mathrm{B}_{4} \mathrm{O}_{7} \cdot 10 \mathrm{H}_{2} \mathrm{O},\) related to the weak monoprotic boric acid \(\left(\mathrm{pK}_{\mathrm{a}}=9.25\right) \cdot\) (c) Mono Lake has some unusual limestone formations called \(t u f\). They form at the site of underwater springs and grow only underwater, although some project above water, having formed at a time when the lake level was higher. Explain how the tufa form. [Hint: What chemical reaction(s) is(are) involved?]

Write plausible equations for the (a) reaction of \(\mathrm{Al}(\mathrm{s})\) with \(\mathrm{Br}_{2}(1)\) (b) production of \(\mathrm{Cr}\) from \(\mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})\) by the thermite reaction, with Al as the reducing agent; (c) separation of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) impurity from bauxite ore.

Write a chemical equation to represent (a) the reaction of potassium cyanide solution with silver nitrate solution; (b) the combustion of \(\mathrm{Si}_{3} \mathrm{H}_{8}\) in an excess of oxygen; (c) the reaction of dinitrogen with calcium carbide to give calcium cyanamide (CaNCN).

Describe two methods for determining the identity of an unknown compound that is either \(\mathrm{Li}_{2} \mathrm{CO}_{3}\) or \(\mathrm{K}_{2} \mathrm{CO}_{3}.\)

Briefly describe each of the following ideas, methods, or phenomena: (a) diagonal relationship; (b) preparation of deionized water by ion exchange; (c) thermite reaction; (d) inert pair effect.
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