Calculate the volume needed to dissolve 11.2g CuSO4 to prepare 0.140M?

Answer 1

How many moles do you have in 11.2 g?
mols = grams/molar mass.

MCuSO4 = moles CuSO4/L CuSO4
You have M and moles, solve for L.

Answer 2

Calculate the volume required to dissolve 11.2 g of CuSO4 to prepare a 0.140M solution.

Answer 3

Calculate the volume required to dissolve 11.2 g of CuSO4 to prepare a 0.140M solution

Answer 4

Let‘s walk through the steps. We know that M = moles of solute/L of solution. To find the number of moles of CuSO4, we need to put 11.2 grams over its atomic mass, 159.62 grams. The quotient is 0.07, meaning we have .07 moles. We also know that the final molarity is 0.140M.
We can rearrange the equation to be L of solution = moles of solute/molarity (M). Using this, let‘s plug in the numbers:
L = 0.07/0.140
L = 0.5
You‘ll need 0.5 liters of solution, or 500 milliliters.

Answer 5

Calculate the volume needed to dissolve 11.2g CuSO4 to prepare 0.140M?

Answer 6

We can use the formula:

moles = mass/molar mass

First, we need to calculate the number of moles of CuSO4 in 11.2 g:

moles = 11.2 g / 159.61 g/mol = 0.070 moles

Next, we can use the formula:

Molarity = moles of solute / volume of solution

to find the volume of solution required to prepare a 0.140 M solution:

0.140 M = 0.070 moles / volume of solution

Solving for the volume of solution:

volume of solution = 0.070 moles / 0.140 M = 0.5 L

Therefore, the volume needed to dissolve 11.2 g CuSO4 to prepare a 0.140 M solution is 0.5 L.