Which one of the following compounds will NOT be soluble in water?

A) NaOH
B) Na2S
C) K2SO4
D) LiNO3
E) PbO

To determine which compound will NOT be soluble in water, we need to refer to the solubility rules.

According to the solubility rules, compounds containing sodium (Na+), potassium (K+), and nitrate (NO3-) ions are generally soluble in water. Compounds containing hydroxide (OH-), sulfide (S2-), and oxide (O2-) ions are usually insoluble or only partially soluble in water.

Let's analyze each compound:

A) NaOH - Sodium hydroxide. It contains sodium (Na+) and hydroxide (OH-) ions. Sodium hydroxide is soluble in water.

B) Na2S - Sodium sulfide. It contains sodium (Na+) and sulfide (S2-) ions. Sodium sulfide is soluble in water.

C) K2SO4 - Potassium sulfate. It contains potassium (K+) and sulfate (SO4^2-) ions. Potassium sulfate is soluble in water.

D) LiNO3 - Lithium nitrate. It contains lithium (Li+) and nitrate (NO3-) ions. Lithium nitrate is soluble in water.

E) PbO - Lead(II) oxide. It contains lead (Pb2+) and oxide (O2-) ions. While most metal oxides are insoluble in water, lead(II) oxide is an exception and is slightly soluble in water.

Based on the solubility rules, the compound that will NOT be soluble in water is:

E) PbO - Lead(II) oxide.

To determine which compound will NOT be soluble in water, you need to consider the solubility rules for common ionic compounds.

There are several solubility rules that can help in predicting the solubility of different ionic compounds. One of the most commonly used rules is "like dissolves like," which states that compounds with similar polarities will dissolve in each other. In other words, polar compounds tend to dissolve in polar solvents, while nonpolar compounds tend to dissolve in nonpolar solvents.

For ionic compounds, another important rule is that salts containing alkali metal cations (Group 1 elements: Li+, Na+, K+, etc.) and the ammonium ion (NH4+) are generally soluble in water. The hydroxides (OH-) are also generally soluble, but there are exceptions such as with some transition metal hydroxides. On the other hand, some sulfides (S2-) and oxides (O2-) are generally insoluble in water.

Let's analyze each compound:

A) NaOH - This is a strong base consisting of Na+ cation and OH- anion. Both ions are soluble in water. Therefore, NaOH is soluble in water.

B) Na2S - This compound consists of Na+ cations and S2- anions. According to the solubility rules, most sulfides are insoluble in water. Therefore, Na2S is not soluble in water.

C) K2SO4 - This compound contains K+ cations and SO4^2- anions. According to the solubility rules, sulfates (SO4^2-) are generally soluble in water. Therefore, K2SO4 is soluble in water.

D) LiNO3 - This compound consists of Li+ cations and NO3- anions. According to the solubility rules, nitrates (NO3-) are generally soluble in water. Therefore, LiNO3 is soluble in water.

E) PbO - This compound contains Pb2+ cations and O2- anions. According to the solubility rules, oxides (O2-) are generally insoluble in water. Therefore, PbO is not soluble in water.

Based on the solubility rules, the compound that will NOT be soluble in water is:

E) PbO

e.

I'll bet you could google, solubility PbO and find the answer quicker than waiting on someone to answer here..