Question
Prepare a 0.0200 mM dye solution at low pH by dilution 0.40 ml of the stock 0.100 mM chemical X into the appropriate volume of 2.5 M HCl.
What is the amount of HCL required for dilution, the final concentration of HCl in the solution, and the pH?
I know there's the MV = MV, but I'm not sure how to begin to solve this. The 2.5 M HCl throws me off since there's two concentrations now (2.5 and the .02)
What is the amount of HCL required for dilution, the final concentration of HCl in the solution, and the pH?
I know there's the MV = MV, but I'm not sure how to begin to solve this. The 2.5 M HCl throws me off since there's two concentrations now (2.5 and the .02)
Answers
The 2.5 M HCl is the diluting agent and has nothing to do with the calculation for the dye. (Another way of saying it is that the 2.5 M HCl is just water as far as the dye dilution is concerned.). My MV = MV gets 2 mL.
The HCl is 2.5 x (1.6/2.0) = ?? if we assume the volumes are additive.
The HCl is 2.5 x (1.6/2.0) = ?? if we assume the volumes are additive.
How were you able to get the 1.6?
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