Question

A) How many milliliters of a stock solution of 7.00 M HNO3 would you have to use to prepare 0.150 L of 0.530 MHNO3?

B) If you dilute 11.0 mL of the stock solution to a final volume of 0.340 L, what will be the concentration of the diluted solution?

Answer 1

Molarity of stock solution, M, = 7.00 M Let volume of stock solution required = 1 Molarity of dilute solution to be prepared, M₂ = 0.530 M Volume of dilute solution to be prepared, V₂ = 0.150L (12=1000 mL) ' V2 = 0.150 x 1000 ml = 150 mL By dilution equation . (Mindow = (M₂ V) dilute . IM, M2 must be in ) same units (7.00 M) (V) = (0.530M) (150 ml) Mi, Vz must be in ) same units . Vi = 0.530 M X ISO mL = 11.36 mL 7:00M So volume e stuck solution required = 11. 36 mL (11=1000 mL) Molarity of stock solution, M, - 7.00 M Volume of stock solution, Vi=110 mL het Melarity of dilute solution prepared = M₂ Volume of dilucte Lolution prepared = V2 = 0.340L 2 2 0.340 X 1000 mL = 340 mL by dilution equation (M.V.) stock = (M242) dinite (7.00M) (11 mL) = (M2) (340 ml) M₂ = 1,00 mx 11 ml = 0.226 M. Зчь mp so Molasity of dilute solution prepared = 0,226 M