A 0.755-g sample of hydrated copper(II) sulfate CuSO4 ·x H2 O was heated carefully until it had

A 0.755-g sample of hydrated copper(II) sulfate CuSO4 ·x H2...

A 0.755-g sample of hydrated copper(II) sulfate $$\mathrm{CuSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}$$ was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO_) with a mass of 0.483 g. Determine the value of $x .$ [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit of $\mathrm{CuSO}_{4}$ in the hydrated crystal.]

A 0.755-g sample of hydrated copper(II) sulfate
$$\mathrm{CuSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}$$
was heated carefully until it had changed completely to anhydrous copper(II) sulfate (CuSO_) with a mass of 0.483 g. Determine the value of $x .$ [This number is called the number of waters of hydration of copper(II) sulfate. It specifies the number of water molecules per formula unit of $\mathrm{CuSO}_{4}$ in the hydrated crystal.]

Key Concepts

Hydrates

Hydrates are solids that incorporate water molecules into their crystalline structure. They consist of a non-water component and water molecules in a fixed ratio, and their properties can change significantly when the water is removed, typically by heating.

Waters of Hydration

Waters of hydration refer to the water molecules that are integrated into the crystal lattice of a hydrated compound. Determining the number of these water molecules is essential for establishing the compound’s formula and understanding its chemical composition.

Molar Mass and Stoichiometry

Molar mass and stoichiometry are fundamental concepts used to relate the mass of a substance to the number of moles. In problems involving hydrates, stoichiometry allows one to calculate the number of moles of the anhydrous compound and water molecules from their masses, revealing their molar ratio.

Thermal Decomposition

Thermal decomposition is the process of breaking down a compound by heating. For hydrates, heating causes the water of hydration to be removed, and analyzing the loss in mass helps determine the number of water molecules associated with each formula unit in the original hydrated compound.

Transcript

00:01 So we have a copper sulfate hydrate with unknown number of water being bound to each of the in the crystal.

00:08 So when we have silver from 755 grams of copper hydrate being heated, the water is being removed.

00:15 So and we have a 0 .43 gram of sulphate we remain.

00:19 So water will be removed as a gas.

00:24 Alright, so what would be the, we are going to find what would be the value of eggs.

00:28 Okay, so first of all from here, we can find out the change.

00:32 In the mass should be corresponding to the water leaving the crystal.

00:41 So we can take the difference between the mass, and then we should be able to find out what would be the mass of water being removed.

00:53 So we have 0 .755 minus 0 .483, and then we should have 0 .272 gram, and it's corresponding of water being removed.

01:05 Okay, so the next step is we are going to set up an equation, and then we're going to determine x.

01:14 Okay, first of all, again, if we have mass, we're going to convert to lumber and moles.

01:17 So instead of using the mass of water, we're going to use a lumbermore water.

01:22 So we're going to convert the mass of water to lumber moles, and then we should be able to find it as equals to 0 .0151 -mode.

01:33 All right.

01:34 So the next step is we're going to calculate the number or more for copper sulfate, and then we can find out the more ratio between copper sulfate and water, and then we can find out x...

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