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Chapter 8: Problem 93

Predict the products of the following oxides with water: \(\mathrm{Na}_{2} \mathrm{O}, \mathrm{BaO}, \mathrm{CO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{SO}_{3} .\) Write an equation for each of the reactions. Specify whether the oxides are acidic, basic, or amphoteric.

Short Answer

Expert verified
Na2O and BaO are basic oxides, and they react to form NaOH and Ba(OH)2 respectively; CO2, N2O5, P4O10, and SO3 are acidic oxides and they react to form H2CO3, HNO3, H3PO4, and H2SO4 respectively.

Step by step solution

01

Understanding the behavior of the oxides

Metals form basic oxides whereas non-metals form acidic oxides. Sodium (Na) and Barium (Ba) are metals, that's why Na2O and BaO are basic oxides. Carbon (C), Nitrogen (N), Phosphorus (P) and Sulfur (S) are non-metals, therefore CO2, N2O5, P4O10 and SO3 are acidic oxides.
02

Reacting basic oxides with water

Basic oxides react with water to form metal hydroxides. The reaction of Na2O and BaO with water can be written as: \[Na_2O + H_2O \rightarrow 2NaOH\] \[BaO + H_2O \rightarrow Ba(OH)_2\] Both NaOH and Ba(OH)2 are bases.
03

Reacting acidic oxides with water

Acidic oxides react with water to form acids. The reactions of CO2, N2O5, P4O10 and SO3 can be written as: \[CO_2 + H_2O \rightarrow H_2CO_3\] \[N_2O_5 + H_2O \rightarrow 2HNO_3\] \[P_4O_{10} + 6H_2O \rightarrow 4H_3PO_4\] \[SO_3 + H_2O \rightarrow H_2SO_4\] The resulting compounds H2CO3, HNO3, H3PO4, and H2SO4 are all acids.
04

Determining the nature of the oxides

Na2O and BaO, which react to form bases, are basic oxides. CO2, N2O5, P4O10, and SO3, which react to form acids, are acidic oxides. In this exercise, none of the given oxides are amphoteric (oxides of elements that shows both acidic and basic behavior).

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