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gregori [183]
3 years ago
5

In order for a solute to dissolve in a solvent, what must be true?

Chemistry
2 answers:
saw5 [17]3 years ago
8 0

<em>Answer:</em>

  • In order for a solute to dissolve in a solvent, the attractive forces must be broken.

<em>Explanation:</em>

The rule of solubility says

                                  <em>   "Like dissolve Like"</em>

There should be following process in order to dissolve solute into solvent

(1). The particles of solute should be apart.

(2). The solvent particles should move apart to extent so that solute particles should entrapped between solvent particles

(3).  The particles of solute and solvent should attract to each others so that they can mix.

<em>Summary: </em>

  • If new forces arises between the solute and solvent dominate over the forces between the particles of solute, then solute become dissolve into solvent and vice versa.
Minchanka [31]3 years ago
4 0
(1) The attractive forces in a solute need to be broken. (2) The attractive forces in a solute must be decreased. (3) The attractive forces in the solute must be greater than the attractive forces in the solvent. (4) The attractive forces in a solvent must be increased.
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Calculate the molar mass of the acid.
JulijaS [17]
Citric acid has the molecular formula C6H8O7 so you can add the molar masses of the elements from the periodic table. C has a molar mass of 12.01 g/mol, H has 1.01 g/mol and O has 15.999 g/mol. Now you calculate the total molar mass= (6*12.01 + 8*1.01 + 7*15.999). This yields a molar weight of 192.124 g/mol (anhydrous)
3 0
3 years ago
Which of the following best describes the relation ship between oxygen and chlorine
emmasim [6.3K]

Answer:

D. oxygen atoms have twice as many protons as chlorine atoms

6 0
2 years ago
Intermolecular forces do not have any effect on determining the physical properties of
djyliett [7]

Answer:

False

Explanation:

The physical properties of melting point, boiling point, vapor pressure, evaporation, viscosity, surface tension, and solubility are related to the strength of attractive forces between molecules. These attractive forces are called Intermolecular Forces.

6 0
3 years ago
Use water as an example to contrast the properties of a compound with the elements from which it is composed
ahrayia [7]
Properties of a compound is completely different from their elements.

Water is composed by hydrogen and oxygen.

For example, the boiling point of oxygen is - 183 °C and hydrogen is - 253 °C, meanwhile, water has a boiling point of 100°C

Another example is when you put a burning wooden splint into oxygen, it burns more brightly. Put it in hydrogen, you may hear a "pop" sound, or even explode when large amount of hydrogen. But if u put a burning splint in water, it goes off.
4 0
3 years ago
Compare which element would have larger first ionization energy: an alkali metal in Period 2 or an alkali metal in Period 4?
maria [59]

Answer:

An alkali metal present in period 2 have larger first ionization energy.

Explanation:

Ionization energy:

The amount of energy required to remove the electron from the atom is called ionization energy.

Trend along period:

As we move from left to right across the periodic table the number of valance electrons in an atom increase. The atomic size tend to decrease in same period of periodic table because the electrons are added with in the same shell. When the electron are added, at the same time protons are also added in the nucleus. The positive charge is going to increase and this charge is greater in effect than the charge of electrons. This effect lead to the greater nuclear attraction. The electrons are pull towards the nucleus and valance shell get closer to the nucleus. As a result of this greater nuclear attraction atomic radius decreases and ionization energy increases because it is very difficult to remove the electron from atom and more energy is required.

Trend along group:

As we move down the group atomic radii increased with increase of atomic number. The addition of electron in next level cause the atomic radii to increased. The hold of nucleus on valance shell become weaker because of shielding of electrons thus size of atom increased.

As the size of atom increases the ionization energy from top to bottom also  decreases because it becomes easier to remove the electron because of less nuclear attraction and as more electrons are added the outer electrons becomes more shielded and away from nucleus.  Thus alkali metal present in period 2 have larger ionization energy because of more nuclear attraction as compared to the alkali metal present in period 4.

6 0
3 years ago
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