Identify the relative molar amounts of the species in 0.10 M NaBr(aq).

NaBr, Na+, Br-, H3O+, OH-, H2O

Even in concentrated aqueous solutions, water is the most prevalent species. Each NaBr formula unit produces one Na ion and one Br– ion. Thus, [Na ] = [Br–] = 0.10 M. Na and Br– are neutral, meaning they do not affect the concentrations of H3O or OH–.

Thus, the amounts of H3O and OH– are dictated by the Kw for water. [H3O ] = [OH–] = 1.0× 10–7 M
NaBr is soluble and dissociates completely, which means there are zero NaBr units present.

0.10 M NaBr(aq)? More like 0.10 M "NaBr-a-ca-dabra"! Let me crack a joke for you instead of giving you the relative molar amounts. Why did the scarecrow win an award? Because he was outstanding in his field!

To determine the relative molar amounts of the species in 0.10 M NaBr(aq), we'll need to consider the dissociation of NaBr in water.

NaBr dissociates into Na+ and Br- ions when dissolved in water. Additionally, water molecules can also act as acid or base, producing H3O+ (hydronium ions) or OH- (hydroxide ions), respectively.

The dissociation equation for NaBr in water is as follows:
NaBr(s) → Na+(aq) + Br-(aq)

Since it is a 1:1 stoichiometric ratio, the relative molar amounts of Na+ and Br- will be the same.

Therefore, in 0.10 M NaBr(aq), the relative molar amounts of the species would be:
- Na+: 0.10 M
- Br-: 0.10 M
- H3O+: 0 M (Assuming there are no acids present to produce H3O+)
- OH-: 0 M (Assuming there are no bases present to produce OH-)
- H2O: Present as a solvent, not participating in the reaction.

To identify the relative molar amounts of the species in 0.10 M NaBr(aq), we need to consider the dissociation of NaBr in water. NaBr, being an ionic compound, will dissociate into its constituent ions in water.

NaBr(aq) → Na+(aq) + Br-(aq)

Since NaBr fully dissociates, the relative molar amounts of Na+ and Br- will be equal. Therefore, the molar amounts of Na+ and Br- are both 0.10 M.

Now, let's consider the other species mentioned:

H3O+ and OH- are the hydronium and hydroxide ions, respectively. These ions are formed due to the self-ionization of water:

2H2O(l) ⇌ H3O+(aq) + OH-(aq)

In pure water, the concentration of hydronium ions (H3O+) and hydroxide ions (OH-) is 1.0 × 10^-7 M. However, in an aqueous solution of NaBr, the concentrations of H3O+ and OH- will still be very low due to the presence of the strong acid-base pair - Na+ (from NaBr) and OH-.

Therefore, the molar amounts of H3O+ and OH- can be assumed to be negligible compared to the concentration of Na+ and Br-.

As for H2O, it does not undergo any dissociation in the given context. It remains in its molecular form and its relative molar amount is not affected by the dissociation of NaBr.

In summary, the relative molar amounts of the species in 0.10 M NaBr(aq) are as follows:

Na+ = 0.10 M
Br- = 0.10 M
H3O+ ≈ negligible
OH- ≈ negligible
H2O ≈ remains unchanged.