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Copper(II) chloride and lead(II) nitrate react in aqueous solutions by double replacement. Write...

Question:

Copper(II) chloride and lead(II) nitrate react in aqueous solutions by double replacement. Write the balanced chemical equation, the overall ionic equation, and the net ionic equation for this reaction.

If 10.27 g of copper(II) chloride react, what is the maximum amount of precipitate that could be formed?

Chemical Equations and Ionic Equations

The chemical equation for a reaction is a precise shorthand for communicating information about the reacting species and the products formed from the reaction. The atoms of each element present need to be balanced by introducing coefficients in front of the species.

When the soluble compounds present are allowed to dissociate into constituent ions, we arrive at the overall ionic equation. Insoluble products (precipitates) are left undissociated, as are gases.

Canceling out spectator ions (those that appear on both sides) leaves us with the net ionic equation.

Answer and Explanation: 1

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The balanced chemical equation is:

{eq}CuCl_2 (aq) + Pb(NO_3)_2 (aq) \rightarrow PbCl_2(s) + Cu(NO_3)_2(aq) {/eq}

Now, noting that lead (II)...

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Precipitation Reactions: Predicting Precipitates and Net Ionic Equations

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Chapter 10 / Lesson 9
126K

Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.


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