Which of the following oxides yield an acidic solution when dissolved into water?
P4O10
Na2O
ClO7
Fe2O3
Thanks for any help.
The nonmetal oxides.
To determine which of the given compounds will yield an acidic solution when dissolved in water, we need to look at the chemical properties of each compound.
1. P4O10: This is diphosphorus pentoxide. It is a molecular compound containing both phosphorus and oxygen. When dissolved in water, it reacts with water to form phosphoric acid (H3PO4). Since phosphoric acid is a weak acid, the resulting solution will be acidic.
2. Na2O: This is sodium oxide. It is an ionic compound consisting of sodium ions (Na+) and oxide ions (O2-). When dissolved in water, it dissociates into sodium hydroxide (NaOH). Sodium hydroxide is a strong base, so the resulting solution will be basic, not acidic.
3. ClO7: This formula does not represent a known compound. It is not possible to determine its properties without more information.
4. Fe2O3: This is iron (III) oxide, also known as rust. It is an ionic compound consisting of iron (III) ions (Fe3+) and oxide ions (O2-). When dissolved in water, it does not react to produce any significant amount of acid or base. Therefore, the resulting solution will neither be acidic nor basic.
Based on the given compounds, the only oxide that yields an acidic solution when dissolved in water is P4O10 (diphosphorus pentoxide).