I have a Salt (548.7 g/mol) that is required to be dissolved in a buffer solution of 0.16 M citrate phosphate, pH = 5.0. I was thinking the salt has its own molarity, and the solvent in which I am dissolving is a buffer that has a molarity of 0.16M. Can the molarity of the solvent affect the molarity of the solute? If yes than how we can calculate for the serial dilution to reach 1 M as a total molarity, or do I need to perform calculations considering only the salt molarity for serial dilutions?
If I understood your description, the buffer citrate phosphate 0,16 M, pH = 5.0 is your solvent, and your solute is the salt (548.7 g/mol)!
The Molarity is calculated for a particular solute in a solution. So, the molarity of the solvent (Buffer) can not affect the molarity of the solute (salt): Just consider the buffer as distilled water for the preparation of a given salt (solute) molarity .
But, if the salt (solute) is not chosen correctly , the constituents of the buffer (solvent) may react with the salt and alter it concentration.
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