Question

You are given 100.0 ml of a 2.00 M solution of KOH. What would be the molarity of the solution if it is diluted to a volume of 1000 ml?

Answer 1

The molarity of a solution of KOH that is diluted from 100.0 ml at 2.00 M to a final volume of 1000 ml will be 0.200 M.

Step-by-step explanation:

If we start with 100.0 ml of a 2.00 M solution of KOH and dilute it to a final volume of 1000 ml, we can determine the new molarity using the dilution equation M1V1 = M2V2, where M1 and V1 are the molarity and volume of the initial solution, and M2 and V2 are the molarity and volume of the diluted solution.

To find the final molarity (M2) after dilution, we rearrange the equation to solve for M2: M2 = (M1V1) / V2. Plugging in the values we have: M2 = (2.00 M * 100.0 ml) / 1000 ml = 200.0 mmol / 1000 ml. This simplifies to: M2 = 0.200 M.

Therefore, the molarity of the solution after dilution to 1000 ml is 0.200 M.