```
8.) Find the mass percent of $\mathrm{FeCl}_{3}$ in a solution whose density is $1.42 \mathrm{~g} / \mathrm{mL}$ and whose molarity is $1.19 \mathrm{M}$.
```

Sign in to unlock the answer

Answer from Sia

Posted 5 months ago

Solution

1

$ \text{Mass} = \text{Density} \times \text{Volume} = 1.42 \, \text{g/mL} \times 1000 \, \text{mL} = 1420 \, \text{g} $

2

$ \text{Moles of } \mathrm{FeCl}_{3} = 1.19 \, \text{M} = 1.19 \, \text{moles/L} $

$ \text{Mass of } \mathrm{FeCl}_{3} = \text{Moles} \times \text{Molar Mass} = 1.19 \, \text{moles} \times 162.204 \, \text{g/mol} = 193.02276 \, \text{g} $

3

$ \text{Mass percent} = \left( \frac{\text{Mass of } \mathrm{FeCl}_{3}}{\text{Mass of solution}} \right) \times 100 = \left( \frac{193.02276 \, \text{g}}{1420 \, \text{g}} \right) \times 100 $

Answer

13.59%

Key Concept

Mass percent of a solute in a solution

Explanation

The mass percent is calculated by dividing the mass of the solute by the total mass of the solution and multiplying by 100.

Not the question you are looking for? Ask here!

Enter question by text

Enter question by image

Upgrade to Asksia Pro

Join a AskSia's Pro Plan, and get 24/7 AI tutoring for your reviews, assignments, quizzes and exam preps.

Unlimited chat query usages

Strong algorithms that better know you

Early access to new release features

Study Other Question