A hydrate is a pure substance because it contains water molecules embedded in its crystal

structure that do not vary. Heating a hydrate "drives off" the water molecules, and the solid

that is left behind is called anhydrous $($which means "without water"$).$ The chemical formula of

the hydrate specifies the relative number of each kind of atom in a molecule, as well as the

number of water molecules bound to each molecule.

Calcium chloride dihydrate $($road salt$)$ is an example of a hydrate. The chemical formula for

calcium chloride dihydrate is $CaC{l}_2*2H_{2}O.$ The "dot" in the chemical formula indicates that

two water molecules $(2H_{2}O)$ are attached or bound to the calcium chloride $(CaC{l}_2)$ ions by

weak chemical bonds. The water molecules in calcium chloride dihydrate can be removed by

heating the hydrate. The number of water molecules in a typical hydrate is characteristic of

the particular salt and is usually a small whole number from $1$ to $10.$

The chemical formula of a hydrate can be determined by analyzing the percent water in the

hydrate, i$.$e$.$ the ratio of the mass of water lost upon heating divided by the mass of the

original hydrate. Use the hydrate manganese$($II$)$ chloride tetrahydrate to answer the following

questions. $($Round your answer to $2$ decimal places.$)$

What is the anhydrous mass of manganese$($II$)$ chloride tetrahydrate?

$\frac{g}{m}ol$

What is the mass of the water of manganese$($II$)$ chloride tetrahydrate?

$\frac{g}{m}ol$

What is the total mass of manganese$($II$)$ chloride tetrahydrate?

$\frac{g}{m}ol$

What is the $\%$ water inmanganese$($II$)$ chloride tetrahydrate?