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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

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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Write a balanced net ionic equation for the reaction of sulfuric acid with (a) \(\mathrm{CaCO}_{3}(s)\) (b) a solution of \(\mathrm{NaOH}\). (c) Cu; assume the \(\mathrm{SO}_{4}{ }^{2-}\) ion is reduced to \(\mathrm{SO}_{2}\).

Write a balanced equation for the preparation of (a) \(\mathrm{N}_{2}\) from \(\mathrm{Pb}\left(\mathrm{N}_{3}\right)_{2}\) (b) \(\mathrm{O}_{2}\) from \(\mathrm{O}_{3}\) (c) \(\mathrm{S}\) from \(\mathrm{H}_{2} \mathrm{~S}\)

If an electrolytic cell producing fluorine uses a current of \(7.00 \times 10^{3} \mathrm{~A}\) (at \(10.0 \mathrm{~V})\), how many grams of fluorine gas can be produced in two days (assuming that the cell operates continuously at \(95 \%\) efficiency)?
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