Asample of hydrated tin (ii) chloride (sncl2) has a mass of 4.90 g. when it is dehydrated, it has a mass of 4.10 g. which is the correct chemical formula for the hydrate? sncl2•2h2o          sncl2•4h2o          sncl2•6h2o

SnCl₂·2 H₂O.

Explanation:

Relative atomic mass data from a modern periodic table:

How many moles of SnCl₂ formula units in this sample?

The first mass 4.90 grams contain both the SnCl₂ formula units and a number of water molecules. Luckily, the mass of the dehydrated salt 4.10 grams contains only SnCl₂.

Formula mass of tin (II) chloride SnCl₂:

.

Number of moles of tin (II) chloride SnCl₂ formula units in this sample:

.

How many moles of water molecules H₂O in this sample?

Water of crystallization exist as H₂O molecules in typical hydrated salts. The molar mass of these molecules will be:

.

The mass of water in the hydrated salt is the same as the mass that is lost when the water molecules are removed and the salt is dehydrated.

In other words,

.

.

What's the coefficient in front of water in the formula of this hydrated salt? In other words, how many water molecules are there in the compound for each SnCl₂ formula unit?

.

There are approximately two water molecules for each SnCl₂ formula unit. The formula of this compound shall thus be .

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

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