What is the percent by mass of 110.6 g of potassium fluoride (NaF) dissolved in 1500.0 g of

Chemistry

1 answer:

sveta [45]1 year ago

8 0

The percent by mass of 110.6 g of potassium fluoride (NaF) dissolved in 1500.0 g of water is 0.073733 %.

<h3>What is the mass percentage?</h3>

The mass percent of a solution is defined as the ratio of the mass of solute that is present in a solution, relative to the mass of the solution, as a whole.

$\rm\;Mass \;percentage =\frac{\;Mass \;of \;solute}{\;Mass \;of \;solution}$

Calculate the mass percent of potassium fluoride, using the formula:

$\rm\;Mass \;percentage =\frac{\;Potassium \;fluoride}{\;Mass \;of \;Water}$

$\rm\;Mass \;percentage =\frac{110.6}{1500.0}$

Mass percentage = 0.073733 %

Hence, the percent by mass of 110.6 g of potassium fluoride (NaF) dissolved in 1500.0 g of water is 0.073733 %.

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Which formula is an empirical formula?

poizon [28]

<h2>Hello!</h2>

The answer is:

The empirical formula is the option B. $NH_{3}$

The empirical formula of a compound is the simplest formula that can be written. On the opposite, the molecular formula involves a variant of the same compound, but it can be also simplified to an empirical formula.

$MolecularFormula=n(EmpiricalFormula)$

We are looking for a formula that cannot be simplified by dividing the number of molecules/atoms that conforms the compound.

Let's discard option by option in order to find which formula is an empirical formula (cannot be simplified)

A. $N_{2}O_{4}$

It's not an empirical formula, it's a molecular formula since it can be obtained by multiplying the empirical formula of the same compound.

$N_{2}O_{4}=2(NO_{2})$

B. $NH_{3}$

It's an empirical formula since it cannot be obtained by the multiplication of a whole number and the simplest formula. It's the simplest formula that we can find of the compound.

C. $C_{3}H_{6}$