What mass of water is need to dissolve 34.8 g of copper (ii) sulfate in order to prepare a 0.521 m solution?

419.2 g of water

Explanation:

0.521 = 0.521 moles of CuSO4 in 1000 ml (1 kg) of water

moles = mass/molar mass

34.8 g of CuSO4 = 34.8/159.6086 moles

                                 = 0.2180 moles

0.521 moles of CuSO4 is in 1 kg of water gives 0.521 M

Therefore, 0.2180 moles of CuSO4 in X kg of water will give 0.521 M

X  = 0.218/0.52

          = 0.4192 kg

                  = 419.2 g

Therefore, 419.2 g of water will be needed to dissolve 34.8 g of CuSO4 in order to prepare 0.521 molar solution.

in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume