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Chapter 3: Problem 65

Name the acids: (a) \(\mathrm{HClO}_{2} ;\) (b) \(\mathrm{H}_{2} \mathrm{SO}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{Se}\) (d) HNO \(_{2}\).

Short Answer

Expert verified
The names of the acids are: (a) chlorous acid; (b) sulfurous acid; (c) hydroselenic acid; (d) nitrous acid.

Step by step solution

01

Identifying Type of Acid and Naming HClO2

The molecule HClO2 is an oxyacid, so it's named by using prefix 'hydro-', the root of the anion, and the suffix '-ic', followed by the word 'acid'. The anion ClO2 is called 'chlorite', so when it's an acid, the name will become 'chlorous acid'.
02

Naming H2SO3

The molecule H2SO3 is another oxyacid. The anion here is SO3, which is known as 'sulfite'. So, when it forms an acid, it would be 'sulfurous acid'.
03

Naming H2Se

The molecule H2Se is a binary acid. For binary acids in aqueous solution, we use the prefix 'hydro-', the root of the element, and the suffix '-ic', along with the word 'acid'. Therefore, H2Se becomes 'hydroselenic acid'.
04

Naming HNO2

HNO2 is also an oxyacid. The anion NO2 is known as 'nitrite'. So, when it forms an acid, it would be 'nitrous acid'.

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Most popular questions from this chapter

A \(0.1888 \mathrm{g}\) sample of a hydrocarbon produces \(0.6260 \mathrm{g}\) \(\mathrm{CO}_{2}\) and \(0.1602 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) in combustion analysis. Its molecular mass is found to be 106 u. For this hydrocarbon, determine its (a) mass percent composition; (b) empirical formula; (c) molecular formula.

A piece of gold (Au) foil measuring \(0.25 \mathrm{mm} \times\) \(15 \mathrm{mm} \times 15 \mathrm{mm}\) is treated with fluorine gas. The treatment converts all the gold in the foil to \(1.400 \mathrm{g}\) of a gold fluoride. What is the formula and name of the fluoride? The density of gold is \(19.3 \mathrm{g} / \mathrm{cm}^{3}\)

Without doing detailed calculations, explain which of these compounds produces the greatest mass of \(\mathrm{H}_{2} \mathrm{O}\) when \(1.00 \mathrm{g}\) of the compound is burned in an excess of oxygen: \(\mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{C}_{10} \mathrm{H}_{8}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\)

For the compound \(\operatorname{Ge}\left[\mathrm{S}\left(\mathrm{CH}_{2}\right)_{4} \mathrm{CH}_{3}\right]_{4},\) determine (a) the total number of atoms in one formula unit (b) the ratio, by number, of C atoms to H atoms (c) the ratio, by mass, of Ge to \(S\) (d) the number of \(g\) S in 1 mol of the compound (e) the number of \(C\) atoms in 33.10 g of the compound

Liquid ethyl mercaptan, \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{S},\) has a density of \(0.84 \mathrm{g} / \mathrm{mL} .\) Assuming that the combustion of this compound produces only \(\mathrm{CO}_{2}, \mathrm{H}_{2} \mathrm{O},\) and \(\mathrm{SO}_{2},\) what masses of each of these three products would be produced in the combustion of \(3.15 \mathrm{mL}\) of ethyl mercaptan?
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