Question

What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?

(a) 1.90 L of a 0.270 M solution of Fe(NO3)3 is diluted to a final volume of 2.90 L
(b) 2.30 L of a 0.380 M solution of C,H,OH is diluted to a final volume of 3.95 L
(c) 0.5200 L of a 0.1214 M solution of H PO, is diluted to a final volume of 1.068 L
(d) 21.70 mL of a 0.020 M solution of C12H22011 is diluted to 100.0 mL

Answer 1

The molarity of the diluted solutions is as follows: (a) 0.176 M, (b) 0.221 M, (c) 0.059 M, (d) 0.0043 M.

Step-by-step explanation:

(a) To find the molarity of the diluted solution, we can use the equation M1V1 = M2V2, where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume. Plugging in the values, we get:

M1 = 0.270 M, V1 = 1.90 L, V2 = 2.90 L.

M2 = (M1 x V1) / V2 = (0.270 M x 1.90 L) / 2.90 L = 0.176 M

(b) Using the same equation, we have:

M1 = 0.380 M, V1 = 2.30 L, V2 = 3.95 L.

M2 = (M1 x V1) / V2 = (0.380 M x 2.30 L) / 3.95 L = 0.221 M

(c) Again using the equation, we have:

M1 = 0.1214 M, V1 = 0.5200 L, V2 = 1.068 L.

M2 = (M1 x V1) / V2 = (0.1214 M x 0.5200 L) / 1.068 L = 0.059 M

(d) Applying the equation again, we have:

M1 = 0.020 M, V1 = 21.70 mL (convert to L), V2 = 100.0 mL (convert to L).

M2 = (M1 x V1) / V2 = (0.020 M x 0.02170 L) / 0.1000 L = 0.0043 M