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Chapter 21: Problem 8

Write the formula of the acid formed when each of these acidic oxides reacts with water. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{Cl}_{2} \mathrm{O}\) (c) \(\mathrm{P}_{4} \mathrm{O}_{6}\)

Short Answer

Expert verified
Answer: The acids formed are: (a) H₂SO₃ (sulfurous acid), (b) HOCl (hypochlorous acid), and (c) H₃PO₃ (phosphorous acid).

Step by step solution

01

(a) SO₂ acidic oxide

Since sulfur has a valence of +4 in SO₂ and oxygen has a valence of -2 in oxides, we will use these valencies to form a balanced chemical equation when SO₂ reacts with water. The balanced chemical equation for the reaction with water is: SO₂ + H₂O → H₂SO₃ Hence, the formula of the acid formed when SO₂ reacts with water is H₂SO₃ (sulfurous acid).
02

(b) Cl₂O acidic oxide

In Cl₂O, chlorine has a valence of +1 and oxygen has a valence of -2 in oxides. Using these valencies, we can form a balanced chemical equation for the reaction with water. The balanced chemical equation for the reaction with water is: 2 Cl₂O + 2 H₂O → 4 HOCl Hence, the formula of the acid formed when Cl₂O reacts with water is HOCl (hypochlorous acid).
03

(c) P₄O₆ acidic oxide

For P₄O₆, phosphorus has a valence of +3 and oxygen has a valence of -2 in oxides. We can now form a balanced chemical equation for the reaction with water. The balanced chemical equation for the reaction with water is: P₄O₆ + 6 H₂O → 4 H₃PO₃ Hence, the formula of the acid formed when P₄O₆ reacts with water is H₃PO₃ (phosphorous acid).

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Most popular questions from this chapter

The average concentration of bromine (as bromide) in seawater is \(65 \mathrm{ppm} .\) Calculate (a) the volume of seawater \(\left(d=64.0 \mathrm{lb} / \mathrm{ft}^{3}\right)\) in cubic feet required to produce one kilogram of liquid bromine. (b) the volume of chlorine gas in liters, measured at \(20^{\circ} \mathrm{C}\) and \(762 \mathrm{~mm}\) \(\mathrm{Hg}\), required to react with this volume of sea water.

The amount of sodium hypochlorite in a bleach solution can be determined by using a given volume of bleach to oxidize excess iodide ion to iodine; \(\mathrm{ClO}^{-}\) is reduced to \(\mathrm{Cl}^{-}\). The amount of iodine produced by the redox reaction is determined by titration with sodium thiosulfate, \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3} ; \mathrm{I}_{2}\) is reduced to \(\mathrm{I}^{-}\). The sodium thiosulfate is oxidized to sodium tetrathionate, \(\mathrm{Na}_{2} \mathrm{~S}_{4} \mathrm{O}_{6}\). In this analysis, potassium iodide was added in excess to \(5.00 \mathrm{~mL}\) of bleach \(\left(d=1.00 \mathrm{~g} / \mathrm{cm}^{3}\right)\). If \(25.00 \mathrm{~mL}\) of \(0.0700 \mathrm{M} \mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) was required to reduce all the iodine produced by the bleach back to iodide, what is the mass percent of \(\mathrm{NaClO}\) in the bleach?

Write a balanced net ionic equation for the disproportionation reaction (a) of iodine to give iodate and iodide ions in basic solution. (b) of chlorine gas to chloride and perchlorate ions in basic solution.

Explain why (a) acid strength increases as the oxidation number of the central non- metal atom increases. (b) nitrogen dioxide is paramagnetic. (c) the oxidizing strength of an oxoanion is inversely related to \(\mathrm{pH}\). (d) sugar turns black when treated with concentrated sulfuric acid.

Write a balanced equation for the reaction of hydrofluoric acid with \(\mathrm{SiO}_{2}\). What volume of \(2.0 \mathrm{M} \mathrm{HF}\) is required to react with one gram of silicon dioxide?
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