The issue of preparing metal nitrate solutions
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Most metal nitrates contain crystalline water; if one wishes to prepare a solution of a certain concentration of a metal nitrate, taking Mg(NO3)2·6H2O as an example. For newly purchased chemicals, should one weigh them according to their molecular weight and then prepare the solution, or should the crystal water be removed first before preparing the solution? If the medication has been used with the cap removed, the amount of crystal water may change; is it necessary to remove the crystal water first before preparing the solution? If it is necessary to remove crystal water, what is the basis for selecting the drying temperature? Looking forward to the answers from experts!
If a highly accurate solution is not being prepared as a standard solution, then calculations can be carried out directly using the molecular formula indicated on the label of the commercial reagent, and the solution can be prepared in the desired amount. If a solution is prepared for use as a standard solution, apart from the reference substance, the concentration of the prepared solution must be calibrated. For this kind of knowledge, it would be best for the poster to refer to a textbook or resource on basic analytical chemistry, such as an analytical chemistry handbook or a manual for laboratory technicians. For magnesium nitrate, calibration is necessary if a solution of precise concentration is to be prepared.
Hmm, I see. Thank you so much!