Phosphorous (V) oxide reacts with aquous sodium hydroxide to form a salt containing th phosphate ion. Water is the only other product. Write a balanced chemical reaction between phosphorous (V) oxide and aqueous sodium hydroxide.
Answers
Answer:
Na2O+H2O→2NaOH(1)
Reaction with acids: As a strong base, sodium oxide also reacts with acids. For example, it reacts with dilute hydrochloric acid to produce sodium chloride solution.
Na2O+2HCl→2NaCl+H2O(2)
Magnesium oxide
Magnesium oxide
Magnesium oxide is another simple basic oxide, which also contains oxide ions. However, it is not as strongly basic as sodium oxide because the oxide ions are not as weakly-bound. In the sodium oxide, the solid is held together by attractions between 1+ and 2- ions. In magnesium oxide, the attractions are between 2+ and 2- ions. Because of the higher charge on the metal, more energy is required to break this association. Even considering other factors (such as the energy released from ion-dipole interactions between the cations and water), the net effect is that reactions involving magnesium oxide will always be less exothermic than those of sodium oxide.
Reaction with water: At first glance, magnesium oxide powder does not appear to react with water. However, the pH of the resulting solution is about 9, indicating that hydroxide ions have been produced. In fact, some magnesium hydroxide is formed in the reaction, but as the species is almost insoluble, few hydroxide ions actually dissolve. The reaction is shown below:
MgO+H2O→Mg(OH)2(3)
Reaction with acids: Magnesium oxide reacts with acids as predicted for a simple metal oxide. For example, it reacts with warm dilute hydrochloric acid to give magnesium chloride solution.
MgO+2HCl→MgCl2+H2O(4)
Aluminum Oxide
Describing the properties of aluminum oxide can be confusing because it exists in a number of different forms. One of those forms is very unreactive (known chemically as alpha-Al2O3) and is produced at high temperatures. The following reactions concern the more reactive forms of the molecule. Aluminium oxide is amphoteric. It has reactions as both a base and an acid.
Reaction with water: Aluminum oxide is insoluble in water and does not react like sodium oxide and magnesium oxide. The oxide ions are held too strongly in the solid lattice to react with the water.
Al2O3+6HCl→2AlCl3+3H2O(5)
This reaction and others display the amphoteric nature of aluminum oxide.
Reaction with bases: Aluminum oxide also displays acidic properties, as shown in its reactions with bases such as sodium hydroxide. Various aluminates (compounds in which the aluminum is a component in a negative ion) exist, which is possible because aluminum can form covalent bonds with oxygen. This is possible because the electronegativity difference between aluminum and oxygen is small, unlike the difference between sodium and oxygen, for example (electronegativity increases across a period)
Aluminum oxide reacts with hot, concentrated sodium hydroxide solution to produce a colorless solution of sodium tetrahydroxoaluminate:
Al2O3+2NaOH+3H2O→2NaAl(OH)4(6)
Silicon dioxide (silicon(IV) oxide)
Silicon is too similar in electronegativity to oxygen to form ionic bonds. Therefore, because silicon dioxide does not contain oxide ions, it has no basic properties. In fact, it is very weakly acidic, reacting with strong bases.
SiO2+2NaOH→Na2SiO3+H2O(7)
In another example of acidic silicon dioxide reacting with a base, the Blast Furnace extraction of iron, calcium oxide from limestone reacts with silicon dioxide to produce a liquid slag, calcium silicate:
SiO2+CaO→CaSiO3(8)
Phosphorus Oxides
Two phosphorus oxides, phosphorus(III) oxide, P4O6, and phosphorus(V) oxide, P4O10, are considered here.
Phosphorus(III) oxide: Phosphorus(III) oxide reacts with cold water to produce a solution of the weak acid, H3PO3—known as phosphorous acid, orthophosphorous acid or phosphonic acid:
P4O6+6H2O→4H3PO3(9)
The fully-protonated acid structure is shown below:
NaOH+H3PO3→NaH2PO3+H2O(10)
2NaOH+H3PO3→Na2HPO3+2H2O(11)
In the first reaction, only one of the protons reacts with the hydroxide ions from the base. In the second case (using twice as much sodium hydroxide), both protons react.
4NaOH+P4O6+2H2O→4NaH2PO3(12)
9NaOH+P4O6→4Na2HPO3+2H2O(13)
Phosphorus(V) oxide: Phosphorus(V) oxide reacts violently with water to give a solution containing a mixture of acids, the nature of which depends on the reaction conditions. Only one acid is commonly considered, phosphoric(V) acid, H3PO4 (also known as phosphoric acid or as orthophosphoric acid).
P4O10+6H2O→4H3PO4(14)
This time the fully protonated acid has the following structure:
NaOH+H3PO4→NaH2PO4+H2O(15)
2NaOH+H3PO4→Na2HPO4+2H2O(16)
3NaOH+H3PO4→Na3PO4+3H2O(17)
Similar to phosphorus (III) oxide, if phosphorus(V) oxide reacts directly with sodium hydroxide solution, the same possible salt as in the third step (and only this salt) is formed:
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