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Chapter 21: Problem 72

The reaction of borax, calcium fluoride, and concentrated sulfuric acid yields sodium hydrogen sulfate, calcium sulfate, water, and boron trifluoride as products. Write a balanced equation for this reaction.

Short Answer

Expert verified
The balanced chemical reaction equation is \(Na_2B_4O_7 + 2CaF_2 + 7H_2SO_4 \rightarrow 2NaHSO_4 + 2CaSO_4 + 5H_2O + 2BF_3\).

Step by step solution

01

Identify the Formulas of the Chemical Compounds

First, identify and write down the formulas of the chemical compounds: Borax is \(Na_2B_4O_7\), Calcium Fluoride is \(CaF_2\), and Sulfuric acid is \(H_2SO_4\). The products are Sodium Hydrogen Sulfate (\(NaHSO_4\)), Calcium Sulfate (\(CaSO_4\)), Water (\(H_2O\)), and Boron Trifluoride (\(BF_3\)).
02

Write the Unbalanced Chemical Equation

Combine all the reactants and products to write the unbalanced chemical equation: \(Na_2B_4O_7 + CaF_2 + H_2SO_4 \rightarrow NaHSO_4 + CaSO_4 + H_2O + BF_3\)
03

Balance the Chemical Equation

Balance the chemical equation by ensuring that the number of atoms for each element on the reactant side equals the number on the product side. After adjustments, the balanced equation will be: \(Na_2B_4O_7 + 2CaF_2 + 7H_2SO_4 \rightarrow 2NaHSO_4 + 2CaSO_4 + 5H_2O + 2BF_3\)

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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?]

An aluminum production cell of the type pictured in Figure \(21-24\) operates at a current of \(1.00 \times 10^{5} \mathrm{A}\) and a voltage of 4.5 V. The cell is \(38 \%\) efficient in using electrical energy to produce chemical change. (The rest of the electrical energy is dissipated as thermal energy in the cell.) (a) What mass of \(\mathrm{Al}\) can be produced by this cell in \(8.00 \mathrm{h} ?\) (b) If the electrical energy required to power this cell is produced by burning coal \((85 \%\) C; heat of combustion of \(C=32.8 \mathrm{kJ} / \mathrm{g}\) ) in a power plant with \(35 \%\) efficiency, what mass of coal must be burned to produce the mass of Al determined in part (a)?

Write plausible chemical equations for the (a) dissolving of lead(II) oxide in nitric acid; (b) heating of \(\operatorname{snCO}_{3}(\mathrm{s}) ;\) (c) reduction of lead(II) oxide by carbon; (d) reduction of \(\mathrm{Fe}^{3+}(\mathrm{aq})\) to \(\mathrm{Fe}^{2+}(\mathrm{aq})\) by \(\mathrm{Sn}^{2+}(\mathrm{aq});\) (e) formation of lead(II) sulfate during high-temperature roasting of lead(II) sulfide.

Lithium superoxide, \(\mathrm{LiO}_{2}(\mathrm{s}),\) has never been isolated. Use ideas from Chapter \(12,\) together with data from this chapter and Appendix \(D\), to estimate \(\Delta H_{f}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) and assess whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}).\) (a) Use the Kapustinskii equation, along with appropriate data below, to estimate the lattice energy, \(U,\) for \(\left.\mathrm{LiO}_{2}(\mathrm{s}) . \text { (See exercise } 126 \text { in Chapter } 12 .\right)\) The ionic radii for \(L\) i \(^{+}\) and \(O_{2}^{-}\) are \(73 \mathrm{pm}\) and \(144 \mathrm{pm},\) respectively. (b) Use your result from part (a) in the BornFajans-Haber cycle to estimate \(\Delta H_{\mathrm{f}}^{2}\) for \(\mathrm{LiO}_{2}(\mathrm{s})\) [Hint: For the process \(\mathrm{O}_{2}(\mathrm{g})+\mathrm{e}^{-} \rightarrow \mathrm{O}_{2}^{-}(\mathrm{g}), \Delta H^{\circ}=.\) \(-43 \mathrm{kJ} \mathrm{mol}^{-1} .\) See Table 21.2 and Appendix \(\mathrm{D}\) for the other data that are required.] (c) Use your result from part (b) to calculate the enthalpy change for the decomposition of \(\mathrm{LiO}_{2}(\mathrm{s})\) to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) For \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s}), \Delta H_{\mathrm{f}}^{\circ}=-598.73\) \(\mathrm{kJmol}^{-1}.\) (d) Use your result from part (c) to decide whether \(\mathrm{LiO}_{2}(\mathrm{s})\) is thermodynamically stable with respect to \(\mathrm{Li}_{2} \mathrm{O}(\mathrm{s})\) and \(\mathrm{O}_{2}(\mathrm{g}) .\) Assume that entropy effects can be neglected.

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.
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