Net Ionic Equation Calculator
To write a net ionic equation you have to write the balanced molecular equation. then write the balanced complete ionic equation. Cross out the present spectator ions. What is left is the Net ionic equation.
From Wikipedia:
An ionic equation is a chemical equation in which electrolytes are written as dissociated ions. Ionic equations are used for single and double displacement reactions that occur in aqueous solutions. For example in the following precipitation reaction: CaCl2(aq) + 2AgNO3(aq) --> Ca(NO3)2(aq) + 2AgCl(s)
The full ionic equation would be: Ca2+ + 2Cl− + 2Ag+ + 2NO3− ---> Ca2+ + 2NO3− + 2AgCl(s)
and the net ionic equation would be:2Cl−(aq) + 2Ag+(aq) --> 2AgCl(s)
or, in reduced balanced form,Ag+ + Cl− --> AgCl(s)
In this aqueous reaction the Ca2+ and the NO3− ions remain in solution and are not part of the reaction. They are termed spectator ions and do not participate directly in the reaction, as they exist with the same oxidation state on both the reactant and product side of the chemical equation. They are only needed for charge balance of the original reagents.
In a neutralization or acid / base reaction, the net ionic equation will usually be:H+ + OH− --> H2O
There are a few acid/base reactions that produce a precipitate in addition to the water molecule shown above. An example would be the reaction of barium hydroxide with phosphoric acid because the insoluble salt barium phosphate is produced in addition to water.
Double displacement reactions that feature a carbonate reacting with an acid have the net ionic equation:2 H+ + CO32− --> H2O + CO2
If every ion is a "spectator ion", then there was no reaction, and the net ionic equation is null.
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From Yahoo Answers
Question:a) 2AgNO3 (aq) + Na2SO4 (aq) ---> How would i write the ionic and net ionic equation for this without knowing the charge for Ag (silver)? I'm really lost =[ can someone give me an explaination as well? that would be really helpful!
Answers:Ag is +1 and Na is also +1 (remember HNO3 where H is +1)
Question:Write a balanced formula equation, complete ionic equation, and net ionic equation for the reaction between: (Be sure to include phases.) a. an alkaline earth salt and sulfuric acid, being sure to identify the precipitate. b a halogen with a less active halide, being sure to identify which is oxidized and reduced.
Answers:(A) Among the alkaline earth metals you can chose the soluble salts of calcium, strontium or barium as one of the reactants, because the sulfates of these salts are slightly soluble. The least soluble one is barium sulfate and suppose we choose it as the product. All nitrates of metals are soluble, therefore we can choose barium nitrate as the reactant. Formula equation; Ba(NO3)2(aq) + H2SO4(aq) -------> BaSO4(s) + 2HNO3(aq) Ionic equation: Ba^2+(aq) + 2NO3^-(aq) + 2H^+(aq) + SO4^2-(aq) -------> BaSO4(s) + 2H^+(aq) + 2NO3^-(aq) Net ionic equation: (obtained by eliminating the spectator ions from both sides) Ba^2+(aq) + SO4^2-(aq) -------> BaSO4(aq) (B) Activity of halogens decreases from top to bottom within the group ( F > Cl > Br > I ) In the elemental state all halogens are diatomic molecules. F2 and Cl2 are gases, Br2 is liquid and I2 is solid. F2 replaces all other halogens. Cl2 replaces Br2 and I2. Br2 can only replace I2. Since I2 is the least active one it cannot replace any halogen. Formula equation; Cl2(g) + 2NaBr(aq) -------> 2NaCl(aq) + Br2(l) (note: all salts of sodium, potassium and ammonium are soluble) Ionic equation: Cl2(g) + 2Na^+(aq) + 2Br^-(aq) ------> 2Na^+(aq) + 2Cl^- (aq) + Br2(l) Net ionic equation: Cl2(g) + 2Br^-(aq) ------>2Cl^- (aq) + Br2(l) As it is clearly seen from the net ionic equation, Cl2 is reduced from 0 to -1 and Br^- is oxidized from -1 to 0.
From Youtube:
Net Ionic Equation :Free Science Help at Brightstorm! brightstorm.com How to write a net ionic equation.
