Consider the following solutions. In each case predict...

Consider the following solutions. In each case predict whether the solubility of the solute should be high or low. (a) $\mathrm{HCl}$ in $\mathrm{H}_{2} \mathrm{O} ;$ Justify your answers. ; (b) $\mathrm{HF}$ in $\mathrm{H}_{2} \mathrm{O} ;$ (c) $\mathrm{Al}_{2} \mathrm{O}_{3}$ in $\mathrm{H}_{2} \mathrm{O} ;$ (d) $\mathrm{SiO}_{2}$ in $\mathrm{H}_{2} \mathrm{O}$ (e) $\mathrm{Na}_{2}\left(\mathrm{SO}_{4}\right)$ in hexane, $\mathrm{C}_{6} \mathrm{H}_{14}$

Consider the following solutions. In each case predict whether the solubility of the solute should be high or low.
(a) $\mathrm{HCl}$ in $\mathrm{H}_{2} \mathrm{O} ;$
Justify your answers.
; (b) $\mathrm{HF}$ in $\mathrm{H}_{2} \mathrm{O} ;$
(c) $\mathrm{Al}_{2} \mathrm{O}_{3}$ in $\mathrm{H}_{2} \mathrm{O} ;$
(d) $\mathrm{SiO}_{2}$ in $\mathrm{H}_{2} \mathrm{O}$
(e) $\mathrm{Na}_{2}\left(\mathrm{SO}_{4}\right)$ in
hexane, $\mathrm{C}_{6} \mathrm{H}_{14}$

Key Concepts

Polarity and Solvent-Solute Interactions

This concept deals with the idea that substances with similar polarity tend to dissolve in each other. Polar solutes are more likely to dissolve in polar solvents because of favorable electrostatic interactions and hydrogen bonding. Conversely, nonpolar solutes dissolve well in nonpolar solvents, which is encapsulated in the principle 'like dissolves like'.

Acid Dissociation and Strength

Acid dissociation refers to the extent to which an acid ionizes in solution. Strong acids ionize completely, which typically contributes to high solubility in polar solvents like water. In contrast, weak acids do not ionize completely, resulting in different solubility behaviors despite both being acids.

Hydration Energy and Lattice Energy

For ionic compounds, solubility in a solvent like water depends on the balance between the lattice energy of the ionic solid and the hydration energy released when ions interact with water molecules. A high hydration energy compared to lattice energy results in greater solubility, while a high lattice energy can lead to low solubility.

Structural and Network Effects in Solubility

Some compounds, especially those with extensive covalent networks or strong intermolecular bonding, form rigid structures that are difficult for the solvent molecules to penetrate. This results in low solubility because the solvent cannot effectively interact with and break apart the solid structure.

Nonpolar Solvent and Ionic Compound Solubility

This concept highlights that ionic compounds, which are typically polar, are generally insoluble in nonpolar solvents. Nonpolar solvents lack the ability to stabilize charged species, leading to poor solubility of ionic substances due to unfavorable interactions.

Transcript

00:01 Good day.

00:02 Our topic is about solubility.

00:05 And when we say solubility, we say that it is the extent at which solute dissolves in solvent.

00:25 Now, solute and solvent are essential in the formation of solution.

00:29 Solute can be any compound and can be any face.

00:33 The same is true with solvent.

00:35 Now, the determining factor as to whether solute can really be.

00:39 Dissolved in solvent is governed by we commonly call the like dissolves like principle this principle tells us that the polarity or we say molecules with the same polarity when we say polarity it means whether it's polar or non polar so when we have molecules with the same polarity mix they definitely are insoluble each other.

01:19 So polar dissolves in polar while nonpolar dissolves in nonpolar.

01:31 So let us take a look at the following combination and let us say or let us comment about the solubility of this compound in each other.

01:42 So first is that we have hcl in water.

01:47 Let us note what type of polycules they are in terms of their polarity.

01:52 So what do we know about hcl and h2o is that they are composed of h atoms or are composed of a molecule of h bonded with electronegative atoms.

02:04 In the case of hcl, we have cl, that's the electronegative atom, and in the case of water, we have o...

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