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