High School

What is the molarity of the solution prepared by diluting 35.0 mL of 1.25 M AgNO₃ to each of the following final volumes?

a. 57.7 mL
b. 98.1 mL
c. 680 mL
d. 2.06 L

Answer :

Final answer:

The molarity of the solution after dilution to the given final volumes are approximately:

a. 0.76 M

b. 0.44 M

c. 0.064 M

d. 0.021 M

Explanation:

To calculate the molarity of the solution after dilution, we can use the formula:

M₁V₁ = M₂V₂

Where:

  • M₁ is the initial molarity of the solution
  • V₁ is the initial volume of the solution
  • M₂ is the final molarity of the solution
  • V₂ is the final volume of the solution

Let's calculate the molarity for each of the given final volumes:

a. 57.7 mL:

Using the formula, we have:

1.25 M x 35.0 mL = M₂ x 57.7 mL

Solving for M₂:

M₂ = (1.25 M x 35.0 mL) / 57.7 mL

M₂ ≈ 0.76 M

b. 98.1 mL:

Using the formula, we have:

1.25 M x 35.0 mL = M₂ x 98.1 mL

Solving for M₂:

M₂ = (1.25 M x 35.0 mL) / 98.1 mL

M₂ ≈ 0.44 M

c. 680 mL:

Using the formula, we have:

1.25 M x 35.0 mL = M₂ x 680 mL

Solving for M₂:

M₂ = (1.25 M x 35.0 mL) / 680 mL

M₂ ≈ 0.064 M

d. 2.06 L:

Using the formula, we have:

1.25 M x 35.0 mL = M₂ x 2.06 L

Solving for M₂:

M₂ = (1.25 M x 35.0 mL) / 2.06 L

M₂ ≈ 0.021 M

Learn more about molarity and dilution here:

https://brainly.com/question/32049446

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