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Chapter 22: Problem 82

What is the anhydride for each of the following acids: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(\mathrm{HClO}_{3}\) (c) \(\mathrm{HNO}_{2}\), (d) \(\mathrm{H}_{2} \mathrm{CO}_{3},\) (e) \(\mathrm{H}_{3} \mathrm{PO}_{4} ?\)

Short Answer

Expert verified
The anhydrides for the given acids are as follows: (a) H2S2O7, (b) Cl2O6, (c) N2O3, (d) CO2 (for H2CO3), (e) H4P2O7.

Step by step solution

01

(a) Anhydride of H2SO4

To find the anhydride of H2SO4, we will first combine two molecules of H2SO4 and then remove a water molecule: \[2 \; (\mathrm{H}_{2} \mathrm{SO}_{4}) - \mathrm{H}_{2} \mathrm{O} = \mathrm{H}_{2} \mathrm{S}_{2} \mathrm{O}_{7}\] Thus, the anhydride of H2SO4 is H2S2O7.
02

(b) Anhydride of HClO3

To find the anhydride of HClO3, we will first combine two molecules of HClO3 and then remove a water molecule: \[2 \; (\mathrm{HClO}_{3}) - \mathrm{H}_{2} \mathrm{O} = \mathrm{Cl}_{2} \mathrm{O}_{6}\] Thus, the anhydride of HClO3 is Cl2O6.
03

(c) Anhydride of HNO2

To find the anhydride of HNO2, we will first combine two molecules of HNO2 and then remove a water molecule: \[2 \; (\mathrm{HNO}_{2}) - \mathrm{H}_{2} \mathrm{O} = \mathrm{N}_{2} \mathrm{O}_{3}\] Thus, the anhydride of HNO2 is N2O3.
04

(d) Anhydride of H2CO3

To find the anhydride of H2CO3, we will first combine two molecules of H2CO3 and then remove a water molecule: \[2 \; (\mathrm{H}_{2} \mathrm{CO}_{3}) - \mathrm{H}_{2} \mathrm{O} = \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{5}\] However, H2C2O5 does not exist under normal conditions as the anhydride of carbonic acid. Carbonic acid H2CO3 instead decomposes directly into water and carbon dioxide (CO2): \[\mathrm{H}_{2} \mathrm{CO}_{3} \longrightarrow \mathrm{H}_{2} \mathrm{O} + \mathrm{CO}_{2}\] Thus, CO2 is considered the anhydride of H2CO3.
05

(e) Anhydride of H3PO4

To find the anhydride of H3PO4, we will first combine two molecules of H3PO4 and then remove a water molecule: \[2 \; (\mathrm{H}_{3} \mathrm{PO}_{4}) - \mathrm{H}_{2} \mathrm{O} = \mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}\] Thus, the anhydride of H3PO4 is H4P2O7.

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Most popular questions from this chapter

Write a balanced net ionic equation for each of the following reactions: (a) Dilute nitric acid reacts with zinc metal with formation of nitrous oxide. (b) Concentrated nitric acid reacts with sulfur with formation of nitrogen dioxide. (c) Concentrated nitric acid oxidizes sulfur dioxide with formation of nitric oxide. (d) Hydrazine is burned in excess fluorine gas, forming \(\mathrm{NF}_{3}\). (e) Hydrazine reduces \(\mathrm{CrO}_{4}^{2-}\) to \(\mathrm{Cr}(\mathrm{OH})_{4}^{-}\) in base (hydrazine is oxidized to \(\mathrm{N}_{2}\) ).

Write a molecular formula for each compound, and indicate the oxidation state of the group \(5 \mathrm{~A}\) element in each formula: (a) phosphorous acid, (b) pyrophosphoric acid, (c) antimony trichloride, (d) magnesium arsenide, (e) diphosphorus pentoxide, (f) sodium phosphate.

Explain the following observations: (a) For a given oxidation state, the acid strength of the oxyacid in aqueous solution decreases in the order chlorine \(>\) bromine \(>\) iodine. (b) Hydrofluoric acid cannot be stored in glass bottles. (c) HI cannot be prepared by treating NaI with sulfuric acid. (d) The interhalogen \(\mathrm{ICl}_{3}\) is known, but \(\mathrm{BrCl}_{3}\) is not.

A friend tells you that the "neon" in neon signs is a compound of neon and aluminum. Can your friend be correct? Explain.

Write a chemical formula for each compound or ion, and indicate the oxidation state of the group \(5 \mathrm{~A}\) element in each formula: (a) phosphate ion, (b) arsenous acid, (c) antimony(III) sulfide, (d) calcium dihydrogen phosphate, (e) potassium phosphide, (f) gallium arsenide.
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