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xxTIMURxx [149]
3 years ago
9

Complete the following paragraph to describe how the electrostatic forces in salt compounds can be overcome by interactions betw

een the solvent molecules and the salt compounds. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer.
(1) insoluble
(2) ionic bonds
(3) ion-dipole forces
(4) soluble
(5) hydrogen bonds
(6) dipole-dipole forces
(7) covalent bonds
(8) higher
(9) dispersion forces
(10) lower

Salts are composed of ions that form a tightly packed and ordered network, which is called a crystal lattice, and it is held together by ____.
When a salt is added to a polar solvent like water, the ions interact with the solvent molecules via ____, which overcome the forces originally holding the ions together.
The ions are then isolated and stabilized in solution via these interactions, and when this occurs for most of the salt compound, it is considered in ____ that solvent.
Due to the nature of the interaction between ions and solvent molecules, a concentration of ions can be dissolved ____in water than in alcohol.
Chemistry
1 answer:
motikmotik3 years ago
3 0

Answer:

The words are: (2) ionic bonds; (3) ion-dipole forces; (4) soluble; (8) higher

Explanation:

-Salts are composed of ions that form a tightly packed and ordered network, which is called a crystal lattice, and it is held together by <u>ionic bonds</u>.

<u><em>Explanation</em></u><em>: salts are ionic compounds, which are composed by oppositely charged ions (cations and anions) which are bonded each other by ionic bonds, in an ordered arrangement, often a crystalline solid.</em>

-When a salt is added to a polar solvent like water, the ions interact with the solvent molecules via <u>ion-dipole forces</u>, which overcome the forces originally holding the ions together.

<em>Explanation: the molecules of a polar solvent are dipoles because they have dipolar momentum (a difference in charge due to a electronegativiy difference). When a salt is dissolved in a polar solvent, it dissociates in ions. So, the resulting interactions between these species are ion-dipole forces.</em>

-The ions are then isolated and stabilized in solution via these interactions, and when this occurs for most of the salt compound, it is considered <u>soluble</u> in that solvent.

<em>Explanation: the ions in solution are surrounded by solvent molecules which stabilizes them. A salt which is enterely dissolved in a solvent is soluble in that solvent.</em>

-Due to the nature of the interaction between ions and solvent molecules, a concentration of ions can be dissolved <u>higher</u> in water than in alcohol.

<em>Explanation: water molecules have unique properties that make water an universal solvent. Due to these properties and its polarity, water can dissolve larger quantities of salt than other polar solvents such as alcohol. </em>

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6 0
3 years ago
The density of NaCl( s) is 2.165 g cm 3 at 25 C. How will the solubility of NaCl in water be affected by an increase in pressure
sammy [17]

The solubility of NaCl in water will not be affected by an increase in pressure.

We know that the density of NaCl(s) in 2.165 g/cm³ at 25 °C and we want to know how will its solubility in water be affected when the pressure is increased.

<h3>What is solubility?</h3>

Solubility is the maximum mass of a solute that can be dissolved in 100 grams of solvent at a determined temperature.

The solubility of a solid, such as NaCl, in a liquid, is mainly affected by the temperature. However, since solids are not compressible, an increase in pressure will not affect its solubility.

On the other hand, the solubility of gases in water will increase with an increase in pressure, as stated by Henry's law.

The solubility of NaCl in water will not be affected by an increase in pressure.

Learn more about solubility here: brainly.com/question/11963573

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6 0
3 years ago
The equilibrium constant Kc for the reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol
Ymorist [56]

Answer : The correct option is, (B) 0.11 M

Solution :

First we have to calculate the concentration PCl_3 and Cl_2.

\text{Concentration of }PCl_3=\frac{\text{Moles of }PCl_3}{\text{Volume of solution}}

\text{Concentration of }PCl_3=\frac{0.70moles}{1.0L}=0.70M

\text{Concentration of }Cl_2=\frac{\text{Moles of }Cl_2}{\text{Volume of solution}}

\text{Concentration of }Cl_2=\frac{0.70moles}{1.0L}=0.70M

The given equilibrium reaction is,

                            PCl_3(g)+Cl_2(g)\rightleftharpoons PCl_5(g)

Initially                 0.70        0.70              0

At equilibrium    (0.70-x)   (0.70-x)           x

The expression of K_c will be,

K_c=\frac{[PCl_5]}{[PCl_3][Cl_2]}

K_c=\frac{(x)}{(0.70-x)\times (0.70-x)}

Now put all the given values in the above expression, we get:

49=\frac{(x)}{(0.70-x)\times (0.70-x)}

By solving the term x, we get

x=0.59\text{ and }0.83

From the values of 'x' we conclude that, x = 0.83 can not more than initial concentration. So, the value of 'x' which is equal to 0.83 is not consider.

Thus, the concentration of PCl_3 at equilibrium = (0.70-x) = (0.70-0.59) = 0.11 M

The concentration of Cl_2 at equilibrium = (0.70-x) = (0.70-0.59) = 0.11 M

The concentration of PCl_5 at equilibrium = x = 0.59 M

Therefore, the concentration of PCl_3 at equilibrium is 0.11 M

3 0
3 years ago
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