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What is the proper way to prepare a solution from hydrate?
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Nidal Blake Zianga
What is the proper way to prepare a solution from hydrate?
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 $\mathrm{1~M}$ $\ce{Ca(NO3)2*4H2O}$?
Hydrates are for the solid state. You do not have "hydrates" in the aqueous phase. Therefore the two solutions are identical and indistinguishable.
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 $\mathrm{1~M}$ $\ce{Ca(NO3)2*4H2O}$?
Hydrates are for the solid state. You do not have "hydrates" in the aqueous phase. Therefore the two solutions are identical and indistinguishable.
But the volumes of water added are different. How can they be the same solutions? I want it such that the concentration of Ca(NO3)2 is 1 M, no more, no less.More
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 $10~ \mathrm{mL}$).
Hydrates are for the solid state. You do not have "hydrates" in the aqueous phase. Therefore the two solutions are identical and indistinguishable.
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 $10~ \mathrm{mL}$).
Hydrates are for the solid state. You do not have "hydrates" in the aqueous phase. Therefore the two solutions are identical and indistinguishable.
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