In: Chemistry
What is the concentration of a 5.0 M Na3PO4 solution whose volume is doubled by added water? Wanna know? Make up a volume calculate the number of moles in that volume if it's 5.0 M and then put that number of moles in twice the volume and recalculate the new molarity.
250. mL of a 5.00 M stock solution is diluted to a final volume of 1.25 x 103 mL. What is its concentration in molarity?
Calculate the final mass in grams of Na3PO4 in a 5.00 M stock solution that is diluted from an initial volume of 25.0 mL to a final volume of 67.5 mL. Here's how you do it: Original concentration times its volume = number of moles present times F.W. = number of grams. These are also present in the diluted solution since you didn't add any more of the analyte, just water.
When a solution is diluted Number of moles in solution remains conserved (Moles of intial solution = Moles of final solution).
Number of moles = Molarity of the soluton * Volume(in L)