Question

(1 point) How many mL of water is added to dilute a 10 mL of 0.4 M solution to a new concentration of 0.1 M?

Answer 1

Answer:

The volume of water added is 30 mL

Explanation:

Given data

• Initial concentration (C₁): 0.4 M

• Initial volume (V₁): 10 mL

• Final concentration (C₂): 0.1 M

• Final volume (V₂): ?

We can find V₂ using the dilution rule.

C₁ × V₁ = C₂ × V₂

0.4 M × 10 mL = 0.1 M × V₂

V₂ = 40 mL

The volume of water added is

V₂ - V₁ = 40 mL - 10 mL = 30 mL

Answer 2

Answer:

We have to add 30 mL to bring the new solution to 0.1M

Explanation:

Step 1: Data given

Volume = 10.0 mL

Molarity = 0.4M

New molarity = 0.1M

Step 2: Calculate moles of the original solution

moles = molarity * volume

Moles = 0.4M * 0.01 L

Moles = 0.004 moles

The number of moles will not change, the volume will.

Step 3: Calculate volume that we have to add

Volume = moles / molarity

Volume = 0.004 moles / 0.1 M

Volume = 0.04 L = 40 mL = The total new volume

Step 4: Calculate the volume that has to be added:

Volume added = 40 mL - 10 mL = 30 mL

We have to add 30 mL to bring the new solution to 0.1M