What is the molarity of the dilute solution when each of the following solution related to the given final volume?

(a) 1.00 L of a 0.250-M solution of Fe (NO3) 3 is diluted to a final volume of 2.00L

(b) 0.5000 L of a 0.1222-M solution of C3H7OH isdiluted to a final volume of 1.250 L

(c) 2.3 5 L of a 0.350-M solution of H3PO4 diluted to a final volume of 4.00 L

(d) 22. 50 mL of 0.025-M solution of C12H22O11 is diluted to 100.0 mL

a) 0.125 M

b) 0.04888 M

c) 0.2056 M

d) 0.005625 M

Explanation:

(a) Given:

V₁ = 1.00 L

M₁ = 0.250-M

V₂ = 2.00 L

Now,

We know,

M₁V₁ = M₂V₂

where, M₂ is the molarity of the final solution

Thus,

0.250 * 1.00 = M₂ * 2.00

or

M₂ = 0.125 M

b) Given:

V₁ = 0.5000 L

M₁ = 0.1222-M

V₂ = 1.250 L

Now,

We know,

M₁V₁ = M₂V₂

Thus,

0.1222 * 0.5000 = M₂ * 1.250

or

M₂ = 0.04888 M

c) Given:

V₁ = 2.35 L

M₁ = 0.350 M

V₂ = 4.00 L

Now,

We know,

M₁V₁ = M₂V₂

Thus,

0.350 * 2.35 = M₂ * 4.00

or

M₂ = 0.2056 M

d) Given:

V₁ = 22.50 L

M₁ = 0.025 M

V₂ = 100.0 L

Now,

We know,

M₁V₁ = M₂V₂

Thus,

0.025 * 22.50 = M₂ * 100.0

or

M₂ = 0.005625 M