# What is the proper way to prepare a solution from hydrate?

I am following a protocol that requires me to prepare $10~ \mathrm{mL}$ $\mathrm{1~M}~ \ce{Ca(NO3)2}$. However, there is only $\ce{Ca(NO3)2*4H2O}$ in the lab.

Originally I thought that all I have to do to figure how much $\ce{Ca(NO3)2}$ to weigh is

and then just add $10~ \mathrm{mL}$ water. However, that might dilute the solution and make the concentration less than $\mathrm{1~M}$ as there is already water in the hydrate.

So then I found a protocol and made new calculations as followed:

How can I verify that I got $\mathrm{1~M}$ $\ce{Ca(NO3)2}$ as opposed to $\mathrm{1~M}$ $\ce{Ca(NO3)2*4H2O}$?

Which protocol is correct?

• The hydro-molecular equation is used to determine the volume of water contained within any given mass of a hydrated compound. This volume is then subtracted from the final volume of the solution. – Holms Peterson Jul 23 '20 at 8:16

Originally I thought that all I have to do to figure how much $\ce{Ca(NO3)2}$ to weigh is
and then just add $10~ \mathrm{mL}$ water.
To properly make an aqueous solution of a specified concentration you should dissolve the desired amount of material in about $80\%$ ($8~ \mathrm{mL}$) the desired volume of water. Then dilute to the final solution volume (add water until the solution volume is $10~ \mathrm{mL}$).
How can I verify that I got $\mathrm{1~M}$ $\ce{Ca(NO3)2}$ as opposed to $\mathrm{1~M}$ $\ce{Ca(NO3)2*4H2O}$?