Which compound or compounds in each of the following groups...

Which compound or compounds in each of the following groups is (are) soluble in water? (a) $\mathrm{BaSO}_{4}, \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{BaCO}_{3}$ (b) $\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{NaClO}_{4}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}$ (c) $\mathrm{AgBr}, \mathrm{KBr}, \mathrm{Al}_{2} \mathrm{Br}_{6}$

Which compound or compounds in each of the following groups is (are) soluble in water?
(a) $\mathrm{BaSO}_{4}, \mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{BaCO}_{3}$
(b) $\mathrm{Na}_{2} \mathrm{SO}_{4}, \mathrm{NaClO}_{4}, \mathrm{NaCH}_{3} \mathrm{CO}_{2}$
(c) $\mathrm{AgBr}, \mathrm{KBr}, \mathrm{Al}_{2} \mathrm{Br}_{6}$

Key Concepts

Lattice Energy vs. Hydration Energy

The solubility of an ionic compound in water depends largely on the balance between its lattice energy (the energy holding the ionic lattice together) and the hydration energy (the energy released when water molecules surround and interact with the separated ions). When the hydration energy is greater than the lattice energy, the compound tends to dissolve; otherwise, it remains largely insoluble. This concept helps explain why some compounds expected to be soluble by charge considerations may still have low solubility due to strong lattice interactions.

General Solubility Rules

These are guidelines used to predict whether an ionic compound will dissolve in water. They state, for example, that all nitrate, acetate, and most alkali metal salts are soluble, while many sulfates, carbonates, and halides may be insoluble except when paired with cations from the alkali metals or ammonium. Understanding these rules helps in quickly assessing the solubility of various inorganic compounds without needing to perform complex calculations.

Ionic Nature and Polar Solvent Interactions

Most compounds discussed in solubility problems are ionic, meaning they are composed of positively and negatively charged ions. Water, being a polar solvent, interacts strongly with these ions through ion-dipole interactions, facilitating their separation and dissolution in the solvent. Understanding this interaction is crucial in predicting and rationalizing the solubility behavior of ionic compounds.

Transcript

00:01 Hello everyone, and thanks for joining me, ms.

00:03 Halsstrom, as we discuss and apply some solubility rules.

00:07 Okay, for this problem, we are going to have three sets of compounds, and we're going to look at each three set, each set individually, and determine what's soluble.

00:16 Set one.

00:19 Let's go a little darker color here.

00:21 For set one, our first compound is barium sulfate.

00:27 Our second compound is barium nitrate.

00:32 That's an n.

00:34 That a little nicer there in 03 and our third compound is barium carbonate you can look at a lot of different rules to figure these out the rules i'm looking at if you're using the same textbook as i'm referencing it's on page 133 chemistry and chemical reactivity okay let's look up first our sulfate rule most sulfates are soluble exceptions include oh one of them includes barium.

01:07 This is not soluble.

01:10 Next let's look up the rule for nitrates.

01:13 Here it is.

01:13 If it's got a nitrate, it's soluble.

01:15 I'm circling the substances that are soluble.

01:19 For insoluble compounds, most carbonates are insoluble, so they don't dissolve, and it is not on the exception list.

01:30 So this is not soluble.

01:32 Okay, that's set one...