How many milliliters of a stock solution of 6.80 MM HNO3HNO3 would you have to use to prepare 0.110 LL of 0.470 MM HNO3HNO3 ?

We need 7.60 mililiters of the stock solution

Explanation:

Step 1: Data given

Molarity stock solution = 6.80 M HNO3

Volume of the new solution = 0.110 L

Molarity of the new solution = 0.470M

Step 2: Calculate volume needed

C1*V1 = C2*V2

⇒ with C1 = the concentration of stock = 6.80 M

⇒ with V1 = volume of stock solution = TO BE DETERMINED

⇒ with C2 = the new concentration = 0.470 M

⇒ with V2 = the new volume = 0.110 L

6.80 M * V1 = 0.470 * 0.110

V1 = 0.00760 L = 7.60 mL

We need 7.60 mililiters of the stock solution

c. is the answer

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