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lianna [129]
2 years ago
3

A sample of commercial perchloric acid is 70.0% HClO4 by mass; its density is 1.664 g/mL. How many milliliters of this concentra

ted HClO4 would be required to prepare 500. mL of 1.50 M HClO4 solution?
Chemistry
1 answer:
Gennadij [26K]2 years ago
5 0

Answer:

We need 64.7 mL of this concentrated HClO4 solution

Explanation:

Step 1: Data given

Percentage of HClO4 solutions = 70.0 %

Density of HClO4 = 1.664 g/mL

Volume of prepared HClO4 solution  =  500.0 mL

Molarity of the prepared HClO solution = 1.50 M

Step 2: Calculate mass HClO4

Let's assume we have 1 L = 1000 mL of solution

Density = mass / volume

Mass = density * volume

Mass = 1.664 g/mL * 1000 mL

Mass = 1664 grams

For a 70.0 M HClO4 solution the mass HClO4 is:

1664 g * 0.70 = 1165 grams HClO4

Step 3: Calculate molarity

1165 g HClO4 / 100.5 g  = 11.59 moles HClO4 per L = 11.59 M  

Step 4: Calculate the volume needed

C1V1 = C2V2  

⇒with C1 = the molarity of the 70.0 % HClO4 = 11.59 M

⇒with V1 = the volume of the 70.0 % HClO4 = TO BE DETERMINED

⇒with C2 = the molarity of the prepared HClO4 solution = 1.50 M

⇒with V2 = the volume of the prepared HClO4 solution = 500.0 mL = 0.500 L

11.59 * V2 = 1.50 M * 0.500

V2 = (1.50 * 0.500) / 11.59

V2 = 0.0647 L = 64.7 mL

We need 64.7 mL of this concentrated HClO4 solution

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