How many grams of cuso4.5h2o are require to prepare 100ml of 500ppm cu

500E-6*100grams=50E-3grams=.05grams Cu

Now, grams of copperIIsulfate pentahydrate..
mass=.05*formulamass/atomicmassCu
= .05*250/63.4 grams

8g

To determine the number of grams of CuSO4.5H2O needed to prepare a 100 mL solution with 500 ppm (parts per million) of Cu, we will follow these steps:

Step 1: Convert ppm to mg/L
Since 1 ppm = 1 mg/L, 500 ppm is equivalent to 500 mg/L.

Step 2: Determine the molar mass of CuSO4.5H2O
The molar mass of CuSO4 is calculated as follows:
Cu: 1 atom x 63.55 g/mol = 63.55 g/mol
S: 1 atom x 32.07 g/mol = 32.07 g/mol
O: 4 atoms x 16.00 g/mol = 64.00 g/mol

The molar mass of H2O is calculated as follows:
H: 2 atoms x 1.01 g/mol = 2.02 g/mol
O: 1 atom x 16.00 g/mol = 16.00 g/mol

Therefore, the molar mass of CuSO4.5H2O is:
(63.55 + 32.07 + 64.00) + 5 x (2.02 + 16.00) = 249.68 g/mol

Step 3: Calculate the number of moles of Cu required
To convert mg/L to moles, we need to divide by the molar mass:
500 mg/L x (1 g/1000 mg) x (1 mol/249.68 g) = 0.002 mol/L

Step 4: Calculate the number of moles for the desired volume
Since we want to prepare a 100 mL solution:
0.002 mol/L x 0.1 L = 0.0002 mol

Step 5: Convert moles to grams
To convert moles to grams, we need to multiply by the molar mass:
0.0002 mol x 249.68 g/mol = 0.04994 g

Therefore, approximately 0.0499 grams (or 49.9 mg) of CuSO4.5H2O are required to prepare 100 mL of a 500 ppm Cu solution.

To calculate the number of grams of CuSO4.5H2O required to prepare a 100 ml solution with a concentration of 500 ppm Cu, we need to follow these steps:

Step 1: Understand the problem
First, we need to know the molecular weight of CuSO4.5H2O. You can find this information by looking up the atomic weights of each element in CuSO4 and H2O and then multiplying by the number of atoms of each element present in the compound.

The atomic weights are: Cu = 63.55 g/mol, S = 32.07 g/mol, O = 16 g/mol, and H = 1.01 g/mol. There are four O atoms and two H atoms in the water molecule, so the molecular weight of H2O is 2(1.01 g/mol) + 4(16 g/mol) = 18.02 g/mol.

Step 2: Calculate the molecular weight
Next, we calculate the molecular weight of CuSO4.5H2O by adding up the atomic weights of each element in the compound. The molecular weight is: Cu = 63.55 g/mol, S = 32.07 g/mol, O = 16 g/mol, and H2O = 18.02 g/mol.

The molecular weight of CuSO4.5H2O is: 63.55 + 32.07 + (4 * 16) + (5 * 18.02) = 249.69 g/mol.

Step 3: Calculate the amount of CuSO4.5H2O needed
Now, we can calculate the amount of CuSO4.5H2O needed using the formula:

Amount (g) = (Concentration (ppm) * Volume (L) * Molecular weight (g/mol)) / 1000

Concentration (ppm) = 500 ppm = 500 mg/L

Volume (L) = 100 ml = 0.1 L

Amount (g) = (500 mg/L * 0.1 L * 249.69 g/mol) / 1000

Amount (g) = 12.485 g

Therefore, you would need approximately 12.485 grams of CuSO4.5H2O to prepare 100 ml of a 500 ppm Cu solution.