To calculate the molar mass of CuSO4 x H2O and the value of x, first we need to determine the number of moles of CuSO4 in the 500 cm3 of water.
Molarity (M) is defined as moles of solute per liter of solution. In this case, the concentration is given as 0.072 M, so:
0.072 M = moles of CuSO4 / 0.5 L
Rearranging the equation, we find:
moles of CuSO4 = 0.072 M * 0.5 L = 0.036 mol
The molar mass of CuSO4 is calculated by adding the atomic masses of copper (Cu), sulfur (S), and four oxygen atoms (O):
Molar mass of CuSO4 = (1 Cu * 64 g/mol) + (1 S * 32 g/mol) + (4 O * 16 g/mol) = 159 g/mol
Now, we can find the molar mass of CuSO4 x H2O by adding the molar mass of CuSO4 to the molar mass of water (H2O):
Molar mass of CuSO4 x H2O = 159 g/mol + molar mass of water
Let's assume the molar mass of water is m g/mol. Since we have 9.0 g of hydrated CuSO4 x H2O, we can write:
9.0 g = 0.036 mol * (159 g/mol + m g/mol)
Solving for m:
m = (9.0 g - 0.036 mol * 159 g/mol) / 0.036 mol
m ≈ 144 g/mol
So, the molar mass of CuSO4 x H2O is approximately 159 g/mol + 144 g/mol = 303 g/mol.
Finally, to determine the value of x, the water of crystallization, we divide the molar mass of water by the molar mass of CuSO4 x H2O:
x = (molar mass of water) / (molar mass of CuSO4 x H2O)
x = 144 g/mol / 303 g/mol ≈ 0.475
Therefore, the value of x, the water of crystallization, is approximately 0.475.
To find the number of Cu2+ ions in 100 cm3 of the prepared solution, we need to know the concentration of Cu2+ ions in the solution. Since CuSO4 is a 1:1 salt, the concentration of Cu2+ ions is equal to the concentration of CuSO4 in the solution, which is given as 0.072 M.
The number of moles of Cu2+ ions in 100 cm3 of solution is calculated as:
moles of Cu2+ ions = concentration of Cu2+ ions * volume of solution
moles of Cu2+ ions = 0.072 M * 0.1 L = 0.0072 mol
Since 1 mole contains 6.02x10^23 particles, the number of Cu2+ ions in 100 cm3 of the prepared solution is:
number of Cu2+ ions = moles of Cu2+ ions * Avogadro's number
number of Cu2+ ions = 0.0072 mol * 6.02x10^23 mol^-1 = 4.33x10^21 ions.
Therefore, the number of Cu2+ ions in 100 cm3 of the prepared solution is approximately 4.33x10^21 ions.
9.0g of hydrated salted CuSO4 x H2O was dissolved in 500cm3 of water and it's concentration in moldm3 was experimentally found to be 0.072M . Calculate, the molar mass of CuSO4 x H2O and the value of x, the water of crystallization.[Cu=64 S=32 O=16 H=1]
The number of cu2+ ions in 100cm3 of prepared solution.(L=6.02x10^23)
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