Writing Ionic Equations
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Writing Ionic Equations

Next, I would like you to get some practice writing equations to represent ionic compounds going into and out of solution.

Example

Let me point out what I mean by this using sodium chloride as an example.
When solid sodium chloride dissolves in water, that process can be represented by this equation.

NaCl(s) --> Na+(aq) + Cl-(aq)
Conversely, when solid sodium chloride crystallizes out of solution, that process can be represented by this equation.

Na+(aq) + Cl-(aq) --> NaCl(s)

Practice

Now try your hand at writing equations for dissolution and precipitation reactions which you observed earlier in the lesson by doing exercise 15 (shown here and in your workbook). Then continue with the lesson after checking your answers below.

For each of the soluble compounds in exercise 8, write a balanced equation showing the species formed as the compound goes into solution and indicating whether each one is solid, liquid, gas or aqueous.
For each of the insoluble combinations in exercise 9, write a balanced equation showing the precipitate formed and again indicating whether each specie shown is solid, liquid, gas or aqueous.
For the experiment in exercise 10, write a balanced equation for the dissolution of sodium acetate and for its crystallization.

 

Answers

Exercise 8 - Dissolution Reactions
NaOH(s) --> Na+(aq) + OH-(aq)
MgSO4(s) --> Mg2+(aq) + SO42-(aq)
Ba(NO3)2(s) --> Ba2+(aq) + 2 NO3-(aq)
Exercise 9 - Precipitation Reactions (Note: slightly soluble compounds are included below)
Ba2+(aq) + SO42-(aq) --> BaSO4(s)
2 Ag+(aq) + SO42-(aq) --> Ag2SO4(s)
Cu2+(aq) + 2 OH-(aq) --> Cu(OH)2(s)
Ba2+(aq) + 2 OH-(aq) --> Ba(OH)2(s)
Ag+(aq) + OH-(aq) --> AgOH(s)
Ag+(aq) + Cl-(aq) --> AgCl(s)
Exercise 10 - Dissolution and Crystallization Reactions
NaC2H3O2(s) --> Na+(aq) + C2H3O2-(aq)
Na+(aq) + C2H3O2-(aq) --> NaC2H3O2(s)
or together as NaC2H3O2(s) <--> Na+(aq) + C2H3O2-(aq)

 

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