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3 years ago

Part G

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6 0

The molecule ammonium lauryl sulfate is a detergent because of its hydrophobic tail and a hydrophilic head which are responsible for its cleansing action.

<h3>Properties of ammonium lauryl sulfate</h3>

Though not shown, I presume that the property labelled as C must have to do with the cleasing action of the molecule ammonium lauryl sulfate.

The substance has a hydrophobic tail and a hydrophilic head which enables it to form miscles and these are the responsible for the cleansing action of the ammonium lauryl sulfate molecule.

Learn more about ammonium lauryl sulfate: brainly.com/question/16483020

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vampirchik [111]

Answer:

There are 0.0186 moles of formula units in 6.35 grams of aluminum sulfate $\rm Al_2(SO_4)_3$ .

Explanation:

What's the empirical formula of aluminum sulfate?

Sulfate is an anion with a charge of -2 per ion. When sulfate ions are bonded to metals, the compound is likely ionic.

Aluminum is a group III metal. Its ions tend to carry a charge of +3 per ion.

The empirical formula of an ionic compound shall balance the charge on ions with as few ions as possible.

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Three sulfate ions $\rm {SO_4}^{2-}$ will give a charge of -6.
Two aluminum ions $\rm Al^{3+}$ will give a charge of +6.

Pairing three $\rm {SO_4}^{2-}$ ions with two $\rm Al^{3+}$ will balance the charge. Hence the empirical formula: $\rm Al_2(SO_4)_3$ .

What's the mass of one mole of aluminum sulfate? In other words, what's the formula mass of $\rm Al_2(SO_4)_3$ ?

Refer to a modern periodic table for relative atomic mass data:

Al: 26.982;
S: 32.06;
O: 15.999.

There are

two Al,
three S, and
twelve O

in one formula unit of $\rm Al_2(SO_4)_3$ .

Hence the formula mass of $\rm Al_2(SO_4)_3$ :

$\underbrace{2\times 26.982}_{\rm Al} + \underbrace{3\times 32.06}_{\rm S} + \underbrace{12\times 15.999}_{\rm O} = \rm 342.132\;g\cdot mol^{-1}$ .

How many moles of formula units in 6.35 grams of $\rm Al_2(SO_4)_3$ ?

$\displaystyle n = \frac{m}{M} = \rm \frac{6.35\;g}{342.132\;g\cdot mol^{-1}} = 0.0186\;mol$ .

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