# Question #b3e90

##### 2 Answers

**!! LONG ANSWER !!**

Here's how you'd go about solving this problem.

Both silver nitrate and calcium chloride are soluble in aqueous solution, but when mixed together will form a precipitate, silver chloride,

Notice that **1 mole** of silver nitrate produces **1 mole** of **1 mole** of **1 mole** of calcium chloride produces **1 mole** of **2 moles** of

Use the molarities of the two solutions to determine how many moles of each ion you get

This corresponds to

The balanced chemical equation for this double replacement reaction will be

The complete ionic equation will be

The net ionic equation for this reaction looks like this

The important thing to notice here is that *be equal to* the number of moles of each added when the two solutions are mixed.

Since the *not be equal* to the number of moles of each added.

The volume of the final solution will be

Now, according to the *net ionic equation*, the silver cations and the chloride anions react in a **twice as many** moles of

In other words, all the **by half** in the process.

Therefore, the concentrations of the ions present in solution will be

The overall equation is:

The ionic equation is:

So

The number of moles of

The number of moles of

This is because there are 2 moles of

So after the

The

After reaction all the

The nitrate(V) ions are spectators so the no. moles

The total volume

So to find the final concentration of each ion we divide the number of moles by the total volume, noting that