All categories

3 years ago

A solution contains 0.140 mol KCl in 2.100 L water. What is the concentration of KCl in g/L?

Chemistry

1 answer:

viva [34]3 years ago

4 0

<h3><u>Answer</u>;</h3>

≈ 4.95 g/L

<h3><u>Explanation;</u></h3>

The molar mass of KCl = 74.5 g/mole

Therefore; 0.140 moles will be equivalent to ;

= 0.140 moles × 74.5 g/mole

= 10.43 g

Concentration in g/L

= mass in g/volume in L

= 10.43/2.1

= 4.9667

You might be interested in

What effect does atmospheric pressure and altitude have on the boiling point of water?

NeTakaya

The temperature change.

5 0

3 years ago

What do dipole-dipole forces do?

g100num [7]

An ion-dipole force is a type of intermolecular force in which forces of attraction or repulsion occur between neighboring ions, molecules or atoms.

3 0

3 years ago

Read 2 more answers

Types of atoms. The basic unit of matter. Pure substance is what?

ivanzaharov [21]

Solids, liquids, gases, and plasma are all matter. When all atoms that make up a substance are the same, then that substance is an element. Elements made of only one kind of atom. Because of this, elements are called "pure" substances.

hope this helps :)

7 0

2 years ago

Read 2 more answers

How is a simple cell constructed

ki77a [65]

Answer:

a simple voltaic cell is made by immersing one zinc plate and one copper plate inside water diluted sulfuric acid solution.

4 0

2 years ago

Read 2 more answers

What is the vapor pressure of the solution if 35.0 g of water is dissolved in 100.0 g of ethyl alcohol at 25 ∘C? The vapor press

masya89 [10]

<u>Answer:</u> The vapor pressure of the solution is 43.55 mmHg

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

<u>For water:</u>

Given mass of water = 35.0 g

Molar mass of water = 18 g/mol

Putting values in equation 1, we get:

$\text{Moles of water}=\frac{35.0g}{18g/mol}=1.944mol$

<u>For ethyl alcohol:</u>

Given mass of ethyl alcohol = 100.0 g

Molar mass of ethyl alcohol = 46 g/mol

Putting values in equation 1, we get:

$\text{Moles of ethyl alcohol}=\frac{100.0g}{46g/mol}=2.174mol$

Total moles of solution = [1.944 = 2.174] moles = 4.118 moles

Mole fraction of a substance is given by:

$\chi_A=\frac{n_A}{n_A+n_B}$

<u>For water:</u>

$\chi_{\text{water}}=\frac{n_{\text{water}}}{n_{\text{water}}+n_{\text{ethyl alcohol}}}$

$\chi_{water}=\frac{1.944}{4.118}=0.472$

<u>For ethyl alcohol:</u>

$\chi_{\text{ethyl alcohol}}=\frac{n_{\text{ethyl alcohol}}}{n_{\text{water}}+n_{\text{ethyl alcohol}}}$

$\chi_{\text{ethyl alcohol}}=\frac{2.174}{4.118}=0.528$

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the vapor pressure of the solution, we use the law given by Dalton, which is:

$P_T=\sum_{i=1}^n (p_i\times \chi_i)$