Question

 How many ml of water must be added to 200 ml of .65 M HCl to dilute the solution to .20 M *

(a) 450 mL

(b) 400 mL

(c) 350 mL

(d) 500 mL


How many gram of solute is required to prepare 1.0 L of 1 M CaCl₂.6H₂O? *


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Answer 1

Answer:

(a)450mL or 0.45mL

Hope this helps

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Answer 2

(a) 450 mL

The equation used for calculating dilution is $M_{1} V_{1} = M_{2}V_{2}$ . Here M denotes molarity and V denotes volume.

Here, molarity of stock solution , $M_{1}$  = 0.65 M

Volume of stock solution , $V_{1}$ = 200 ml

molarity of diluted solution , $M_{2}$ = 0.20 M

we have to find amount of water that must be added to dilute solution into 0.20 M.

0.65 x 200 = 0.20 x $V_{2}$

$V_{2} =$ $\frac{0.65}{0.20}$ × 200

   = 650 ml

Thus the volume of diluted solution is 650 ml. i.e., the volume of solution after adding water to initial 200 ml is 650 ml.

So, the amount of water added to dilute the solution to o.20 M is

650 - 200 ml = 450 ml.

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