Solutions a and b contain the same compound dissolved in water. solution a is 5.0l at 0.020m and solution b is 50.0 ml at 0.60m. how many liters of solution a are needed to contain the same number of moles as the 50.0 ml of solution b?

The volume of solution A required is 0.15 L

Explanation:

To calculate the molarity of solution, we use the equation:

       .......(1)

Molarity of solution B = 0.60 M

Volume of solution B = 50.0 mL  = 0.050 L    (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

Now, calculating the volume of solution A required for the same number of moles as solution B.

Moles of solution A = 0.003 moles

Molarity of solution A = 0.020 M

Putting values in equation 1, we get:

Hence, the volume of solution A required is 0.15 L

i believe you are right for all except the 3rd ( look at sqdancefan his answer is much better)