1 mole of AgNO3 has a mass of (107.87+14.01+3 x 16.00) g = 169.87 g. One thousandth of a mole is 0.16987 g. Prepare an aqueous solution with an AgNO3 concentration of 0.16987 g/L. And how to do this practically depends on what concentration accuracy is required. I.e. from which chemical reagent, or from a portion dried to constant mass and under what conditions, how to weigh the necessary amount of this reagent, what scale to use, whether to use a volumetric flask and with what capacity, and maybe make a dilution by weight (based on the mass and density of the solution), how store the solution, etc. In your case, high accuracy in preparing this solution is probably not needed, e.g. the required accuracy may be 0.100 ± 0.005 mM. Check if this is specified in your procedure.

Michelle Darmawan The basic description above by Zbigniew Jońca is correct. I would add that all preparation and storage should be in the dark (cover the containers with aluminum foil) as AgNO3 is easily decomposed by light to silver metal. The classic route of determining the concentration is by gravimetric means - precipitation of silver chloride with excess of sodium chloride.

Thank you for your explanation and guidance Sir Zbigniew Jońca Alan F Rawle

Hi Michelle Darmawan,

You may use the web tool to calculate

https://www.alfa-chemistry.com/solution-dilution-calculator.htm

https://www.alfa-chemistry.com/mass-molarity-calculator.htm

Thank You for your help ! Chen Jingwen