Question

When calcium nitrate, Ca(NO3)2, dissolves in water, it dissociates into its ions. We can represent that process by the following equation: Ca(NO3)2(s) → Ca2+(aq) + 2NO3-(aq) When 1.5 mol calcium nitrate dissolves in water, how many moles of ions should be present in solution? Group of answer choices

Answer 1

4.5 moles

Step-by-step explanation:

The given reaction is

`Ca(NO_3)_2(s)\rightarrow Ca^(+2)(aq)+2NO_3^-(aq)`

Moles of calcium nitrate is 1.5

`Ca(NO_3)_2` produces 2 moles of
`Ca^(+2)` and 1 mole of
`2NO_3^-`

So the total moles of the ions of the products are 3

Therefore in the solution the moles of ions present are

`3*1.5=4.5\ \text{moles}`

Moles of ions present in solution is 4.5.