10.6gram of hydrated zinc tetraoxosulphate (vi) on heating to constant mass gave 5.95g of the anhydrous form.Calculate the number of molecules(x) of water of crystalization in the hydrated salt.(zn=65,s=32,o=16,h=1)
10.6-5.95 = g H2O = 4.65
mols H2O = 4.65/18 = ?
mols ZnSO4 = 5.95/molar mass ZnSO4.
Find the ratio of water to 1 mol ZnSO4. The easy way to do that is to divide the mols H2O by mols ZnSO4 and round to a whole number. If I punched in the right numbers on my calculator that shouldb e ZnSO4.7H2O
To calculate the number of water molecules of crystallization (x) in the hydrated salt, we need to find the molar mass of the hydrated salt.
1. Start by finding the molar mass of zinc tetraoxosulphate (VI):
- Zinc (Zn) has a molar mass of 65 g/mol.
- Tetraoxosulphate (SO4) has a molar mass of (32 g/mol) + (4 * 16 g/mol) = 96 g/mol.
- To calculate the molar mass of the hydrated salt, we add the molar mass of Zn and SO4:
Molar mass = 65 g/mol + 96 g/mol = 161 g/mol.
2. Next, we need to find the number of moles of the hydrated salt:
Number of moles = mass / molar mass = 10.6 g / 161 g/mol = 0.0658 mol.
3. The molar ratio between the hydrated salt and the anhydrous form indicates how many moles of water are lost during the heating process. For zinc tetraoxosulphate (VI), this ratio is 4:1.
Therefore, the number of moles of water lost = 0.0658 mol / 4 = 0.0165 mol.
4. Finally, we can calculate the number of water molecules (x) by multiplying the moles of water lost by Avogadro's number, which is approximately 6.022 × 10^23.
Number of water molecules (x) = 0.0165 mol * (6.022 × 10^23 molecules/mol) = 9.9313 × 10^21 molecules.
Therefore, the number of water molecules of crystallization (x) in the hydrated salt is approximately 9.9313 × 10^21 molecules.
To calculate the number of water molecules (x) in the hydrated salt, we need to determine the mass of the water lost during heating.
First, let's calculate the molar mass of the hydrated zinc tetraoxosulphate (VI):
Molar mass of ZnSO4 = (1 × Zn) + (1 × S) + (4 × O)
= (1 × 65) + (1 × 32) + (4 × 16)
= 65 + 32 + 64
= 161 grams/mole
Next, let's determine the molar mass of the anhydrous form of zinc tetraoxosulphate (VI):
Anhydrous mass = 5.95 grams
Molar mass of anhydrous ZnSO4 = 161 grams/mole
Now, we can calculate the number of moles of the anhydrous form:
Number of moles = Mass of anhydrous form / Molar mass of anhydrous form
= 5.95 g / 161 g/mol
Now that we have the number of moles of the anhydrous form, we can relate it to the number of moles of the hydrated form. The hydrated form contains x moles of water molecules for each mole of hydrated salt.
Number of moles of water = Number of moles of the anhydrous form × x
Since the mass of the water is given in the question, we can equate it to the moles of water using the molar mass of water:
Mass of water = Number of moles of water × Molar mass of water
= Number of moles of water × [(2 × 1) + 16]
= Number of moles of water × 18
From the question, we know that the hydrated salt lost water during heating and the mass decreased. Therefore, we can set up an equation:
Initial mass of hydrated salt - Mass of anhydrous form = Mass of water lost
Using this equation, we can solve for the number of moles of water:
10.6 g - 5.95 g = Number of moles of water × 18
Simplifying the equation:
4.65 g = Number of moles of water × 18
To find the number of moles of water, divide both sides by 18:
Number of moles of water = 4.65 g / 18
Finally, we can calculate the number of molecules (x) of water of crystallization using Avogadro's number:
Number of molecules of water = Number of moles of water × Avogadro's number
Avogadro's number = 6.022 × 10^23 molecules/mol
Therefore,
Number of molecules (x) of water of crystallization = 4.65 g / 18 × 6.022 × 10^23 molecules/mol