3.05 g hydrated copper sulfate produces 1.94 g of anhydrous salt.Assuming complete removal of all water of crystallisation,determine tha formula of hydrated copper sulfate.
3.05 g - 1.94 = 1.11 g H2O abd 1.94 g CuSO4
mols H2O = grams H2O/molar mass H2O
mols CuSO4 = grams CuSO4/molar mass CuSO4.
Now fine the ratio of the two to each other. The easy way to do that is to divide the smaller number by itself (thereby making sure it is 1.00). Then divide the other number by the same small number. Round to whole numbers and that will be the formula of the hydrated salt. You should get CuSO4.5H2O
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Well, let's break it down! We have 3.05 grams of hydrated copper sulfate, and after removing all the water of crystallization, we're left with 1.94 grams of anhydrous salt. Now, to find the formula of the hydrated salt, we need to determine the number of water molecules attached to each copper sulfate molecule.
To do that, we can find the mass of water that was present in the hydrated salt, by subtracting the mass of the anhydrous salt from the mass of the hydrated salt:
Mass of water = Mass of hydrated salt - Mass of anhydrous salt
Mass of water = 3.05 g - 1.94 g
Mass of water = 1.11 g
Now, we know that in copper sulfate, each copper ion (Cu2+) is surrounded by four sulfate ions (SO4^2-) and a certain number of water molecules. To find the number of water molecules, we can calculate the ratio of the mass of water to the molar mass of water.
Molar mass of water (H2O) = 18 g/mol
Number of moles of water = Mass of water / Molar mass of water
Number of moles of water = 1.11 g / 18 g/mol
Number of moles of water ≈ 0.06 mol
Since there is a 1:1 ratio between the copper sulfate molecule and the water molecule, we can conclude that the formula of the hydrated copper sulfate is: CuSO4·H2O.
So, the formula is a show-stopping Copper Sulfate tango with a single water molecule as its dance partner!
To determine the formula of hydrated copper sulfate, we need to find the number of moles of each component (copper sulfate and water) in the given weights and calculate the ratio between them.
Let's start by finding the number of moles of anhydrous copper sulfate (CuSO4). We can use the formula:
moles = mass / molar mass
The molar mass of CuSO4 is calculated by adding up the atomic masses of copper (Cu), sulfur (S), and four oxygen (O) atoms:
Cu: atomic mass = 63.55 g/mol
S: atomic mass = 32.07 g/mol
O: atomic mass = 16.00 g/mol
Molar mass of CuSO4 = (1 * 63.55) + (1 * 32.07) + (4 * 16.00) = 159.61 g/mol
Now, let's calculate the number of moles of anhydrous copper sulfate:
moles of CuSO4 = 1.94 g / 159.61 g/mol = 0.01214 mol
Next, we'll find the number of moles of water in the hydrated copper sulfate. To do this, we subtract the mass of anhydrous copper sulfate from the total mass of the compound:
moles of water = (3.05 g - 1.94 g) / 18.02 g/mol = 0.06104 mol
Now that we have the moles of copper sulfate and water, we need to determine their mole ratio. We divide the moles of water by the moles of copper sulfate to get the simplest whole number ratio:
0.06104 mol / 0.01214 mol ≈ 5
This tells us that for every 1 mole of anhydrous copper sulfate, there are approximately 5 moles of water.
Finally, we can write the formula of the hydrated copper sulfate:
CuSO4 · 5H2O
This means that each formula unit of hydrated copper sulfate contains one copper sulfate ion (CuSO4) and five water molecules (H2O).