An ionic chemical reaction involves the interactions of ionic species to form a new compound. For example, if we add a solution of barium chloride (BaCl2) with a solution of sodium sulphate (Na2SO4), it forms an insoluble solid (precipitate) of barium sulphate (BaSO4). The molecular and ionic equation for the given reaction would be;
A total ionic equation indicates all soluble ionic materials like ions with subscript (aq). For insoluble ionic solids, (s) stands for their solid state. Those ions which are remain same before and after reaction are called as spectator ions. For writing a net ionic equation, subtract these spectator ions from ionic equation. Let’s see what is a net ionic equation for is given reaction. Here sodium and chloride ions are common and have to eliminate from net-ionic-equation;
2Na+(aq) +
SO42-(aq) +
Ba2+(aq) +
2Cl-(aq)
2Na+(aq) +
2Cl-(aq) +
BaSO4(s)
Let’s see how to writing net ionic equations of reaction of sodium phosphate and calcium chloride to form an insoluble white solid form of calcium phosphate. The molecular equation for this reaction is as follow;
First write complete ionic equation with the use of chemical reaction. It shows all ions involve in reaction in their physical state and also indicate the correct formula, charge and number of each ion.
Hence ionic equation would be;
6 Na+ (aq)
+ 2 PO43- (aq)
+ 3 Ca2+ (aq)
+ 6
Cl- (aq)
6
Na+ (aq)
+
6 Cl- (aq)
+ Ca3(PO4)2 (s)
Overall net ionic equations show soluble, strong electrolytes reacting in the form of ions. Now days many net ionic equation Solver are available to solve equation from molecular equation. For writing ionic equations, you must remember that most alkali metal compounds, ammonium compounds, halide, nitrates, chlorate compounds are soluble in nature. Carbonate, phosphate, oxalates, sulphide, chromate compounds are insoluble in nature. Except group-1, oxides are insoluble in water and form acids or bases. Only HCl, HBr, HI, HNO3, H2SO4, HClO4 are strong acids and ionize completely while all other are weak acids.
Na2SO4
+ BaCl2
2NaCl + BaSO4
2Na+(aq) +
SO42-(aq) +
Ba2+(aq) +
2Cl-(aq)
2Na+(aq) +
2Cl-(aq) +
BaSO4(s)
A total ionic equation indicates all soluble ionic materials like ions with subscript (aq). For insoluble ionic solids, (s) stands for their solid state. Those ions which are remain same before and after reaction are called as spectator ions. For writing a net ionic equation, subtract these spectator ions from ionic equation. Let’s see what is a net ionic equation for is given reaction. Here sodium and chloride ions are common and have to eliminate from net-ionic-equation;
Ba2+(aq) +
SO42-(aq)
BaSO4(s)
Let’s see how to writing net ionic equations of reaction of sodium phosphate and calcium chloride to form an insoluble white solid form of calcium phosphate. The molecular equation for this reaction is as follow;
2Na3PO4(aq)
+ 3 CaCl2(aq)
6 NaCl(aq) + Ca3(PO4)2(s)
First write complete ionic equation with the use of chemical reaction. It shows all ions involve in reaction in their physical state and also indicate the correct formula, charge and number of each ion.
Hence ionic equation would be;
6 Na+ (aq)
+ 2 PO43- (aq)
+ 3 Ca2+ (aq)
+ 6 Cl- (aq)
6
Na+ (aq)
+ 6 Cl- (aq)
+ Ca3(PO4)2 (s)
Now subtract spectator ions
(Na+, Cl-) from reaction to get net ionic equation.
2 PO43- (aq)
+ 3 Ca2+ (aq)
Ca3(PO4)2(s)
Overall net ionic equations show soluble, strong electrolytes reacting in the form of ions. Now days many net ionic equation Solver are available to solve equation from molecular equation. For writing ionic equations, you must remember that most alkali metal compounds, ammonium compounds, halide, nitrates, chlorate compounds are soluble in nature. Carbonate, phosphate, oxalates, sulphide, chromate compounds are insoluble in nature. Except group-1, oxides are insoluble in water and form acids or bases. Only HCl, HBr, HI, HNO3, H2SO4, HClO4 are strong acids and ionize completely while all other are weak acids.
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