Intermolecular forces: effect on solubility

Basic idea: “Like dissolves like.” The stronger the intermolecular forces between the solute molecule and the solvent molecule, the greater the solubility of the solute in the solvent.

What are the forces that affect solubility?

Solubility is the maximum of a substance that will dissolve in a given amount of solvent at a given temperature. There are two direct factors that affect solubility: temperature and pressure. Temperature affects the solubility of both solids and gases, but pressure affects only the solubility of gases.

And how are intermolecular forces and solubility related? Solubility depends on the solvent‘s ability to overcome the intermolecular forces in a solid. What happens when the molecule-to-molecule attractive forces in the solute are comparable to those in the solvent? -The material has limited solubility in the solvent.

Moreover, why does salt dissolve in water by intermolecular forces?

Water can dissolve salt because the positive part of water molecules attracts the negative one Chloride ions and the negative part of water molecules attract the positive sodium ions.

What 4 factors affect solubility?

Factors affecting solubility

  • Temperature. Basically, solubility increases with temperature.
  • Polarity. In most cases, solutes will dissolve in solvents of similar polarity.
  • Pressure. Solid and liquid solutes.
  • Molecule size.
  • Stirring increases the rate of dissolution.

What kind of reaction is NaCl ?

A combination reaction is a reaction in which two or more substances (the reactants) are combined directly to form a single product (the product). An example is the reaction where sodium (Na) combines with chlorine (Cl2) to form sodium chloride or common salt (NaCl).

What is the intermolecular force strongest?

The strongest intermolecular force is the hydrogen bond, which is the attractive force between an H atom covalently bonded to the lone pair of electrons of a strongly electronegative atom (oxygen, fluorine, and nitrogen).

Is h2o polar or non-polar?

A water molecule, abbreviated as H2O, is an example of a polar covalent bond. The electrons are distributed unequally, with the oxygen atom spending more time with electrons than the hydrogen atoms. Because electrons spend more time with the oxygen atom, it carries a partial negative charge.

What kind of intermolecular force causes NaCl to dissolve in water?

Ion-dipole forces

Ion-dipole forces

How is the solubility of a gas affected by temperature?

As temperature increases, solubility of a gas decreases, as shown by the Downtrend shown in the graph. An increased temperature causes an increase in kinetic energy. The higher kinetic energy causes more movement in molecules, which break intermolecular bonds and escape from solution.

Why is Caco3 insoluble in water?

Calcium carbonate has a relatively high lattice energy compared to let’s say NaCl. With calcium carbonate, the high lattice energy is the main reason. However, I should point out that it’s not completely insoluble in water, and it’s also strange that its solubility decreases as you increase the temperature.

How does structure affect solubility?

Solubility depends on the molecular structure. When a substance dissolves, its molecules or ions separate from each other and are evenly mixed with molecules of the solvent. Remember that water contains polar covalent bonds. Consequently, water molecules have a negative domain and a positive domain.

What types of intermolecular forces are there?

The three main types of intermolecular interactions are dipole-dipole interactions, London dispersion forces (these both are often collectively referred to as van der Waals forces) and hydrogen bonds.

Is solubility a chemical property?

Solubility. Solubility is a chemical property that refers to the ability of a specific substance, the solute, to dissolve in a solvent. It is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. The resulting solution is called a saturated solution.

Why is solubility important?

Solubility is the upper concentration that a compound will reach in a solution. Solubility is a very important property in drug discovery and development since concentration affects so many aspects of pharmacology (e.g. structure-activity relationships, efficacy, pharmacokinetics, toxicity).

What are examples of solubility?

So for some examples of solubility… meant are solvents that dissolve in a solute to form a solubility based on their solubility: salt or sugar in HOT water; in cold water it would form a mixture (and a small amount of solution).

How do you determine solubility?

Solubility is the maximum amount of a substance that can be dissolved in it can be a solvent at a given temperature. Such a solution is called saturated. Divide the mass of the compound by the mass of the solvent, then multiply by 100g to calculate the solubility in g/100g.

Is HCl dipole dipole?

For example, HCl molecules, z, have a dipole moment because the hydrogen atom has a slightly positive charge and the chlorine atom has a slightly negative charge. Due to the attraction between oppositely charged particles, there is a small dipole-dipole attraction between neighboring HCl molecules.

Which gas is the least soluble in water?

Water (H2O) is a polar molecule that exhibits hydrogen bonding, so the least soluble gas would be a non-polar compound.

What kind of intermolecular force is HCl?

Dipole Dipole

What is the intermolecular force of NaCl?

These intermolecular forces weaken the ionic bonds between the sodium and chloride ions, causing the sodium chloride to dissolve in the water (figure). Ion dipole forces in a sodium chloride solution. London Forces These intermolecular forces are sometimes referred to as “dipoline-induced dipole forces” or “instantaneous dipole forces“.

Why does solubility increase with temperature?

For many solids dissolved in liquid water , the solubility increases with temperature. The increase in kinetic energy that accompanies higher temperatures allows the solvent molecules to more effectively break apart the solute molecules that are held together by intermolecular attractions.