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zalisa [80]
3 years ago
9

If you needed to make 100 mL of a 0.2 M fruit drink solution from the 1.0 M fruit drink solution, how would you do it? (Hint: Us

e MsVs = MdVd to find the amount of concentrated solution you need, then add water to reach 100 mL.) Show your work.
Chemistry
2 answers:
grigory [225]3 years ago
8 0

Answer:

We take 20.0 mL of the 1.0 M fruit drink solution and then add 80.0 mL of water to  make 100 mL of a 0.2 M fruit drink solution.

Explanation:

  • Using the rule that: the no. of millimoles of a solution before dilution is equal to the no. of millimoles of the solution after the dilution.

<em>(MV) before dilution = (MV) after dilution.</em>

M before dilution = 1.0 M, V before dilution = ??? mL.

M after dilution = 0.2 M, V after dilution = 100 mL.

<em>∴ V before dilution = (MV) after dilution / M before dilution </em>= (0.2 M)(100 mL) / (1.0 M) = <em>20.0 mL.</em>

<em>So, we take 20.0 mL of the 1.0 M fruit drink solution and then add 80.0 mL of water to  make 100 mL of a 0.2 M fruit drink solution.</em>

aleksandr82 [10.1K]3 years ago
7 0

Answer:

The volume of the 1.0 M juice solution is 20 mL.

Explanation:

Concentration of juice = M_1=1.0m

Volume of the juice = V_1

Concentration of Juice we need = 0.2

Volume of the 0.2 M juice we need V_2= 100 mL=0.1L

Using dilution formula :

M_1V_1=M_2V_2

1.0M \times V_1=0.2 M\times 0.1 L

V_1=0.02 L = 20 mL

We have to add 80 mL of water to 20 ml of solution which has concentration of juice equal to 1.0 M.

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Answer:

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Explanation:

<em>A chemist prepares a solution of potassium dichromate by measuring out 13.1 g of potassium dichromate into a 150 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mol/L of the chemist's potassium dichromate solution. Be sure your answer has the correct number of significant digits.</em>

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