If barium nitrate solution is added to sodium hydroxide solution does a precipitate form? Are there exceptions?

I have an assignment Q that asks about the precipitate, and I thought that Ba(OH)2 was soluble.

Barium hydroxide is moderately soluble, up to about .1M concentrations. So if the amount of barium hydroxide is on the order of or greater than .1M, there will be a precipate.

To determine if a precipitate will form when barium nitrate solution is added to sodium hydroxide solution, we will need to consider the solubility of the products.

First, let's examine the reaction between barium nitrate (Ba(NO3)2) and sodium hydroxide (NaOH):

Ba(NO3)2 + 2NaOH → Ba(OH)2 + 2NaNO3

As you correctly stated, barium hydroxide (Ba(OH)2) is generally considered moderately soluble. However, the solubility of Ba(OH)2 can vary depending on the concentration.

At low concentrations, barium hydroxide is indeed soluble. However, as the concentration of barium hydroxide increases, the solubility decreases, and a precipitate can form.

To determine whether a precipitate will form, you should consider the molar concentrations of the barium nitrate and sodium hydroxide solutions that you are mixing. If the concentration of barium hydroxide exceeds its solubility limit (approximately 0.1 M), a precipitate will likely form.

It's important to note that there can be exceptions and additional factors to consider. Factors such as temperature, presence of other ions, and pH can influence the solubility of the compounds and may result in different outcomes.

In summary, if the concentration of barium hydroxide exceeds its solubility limit (approximately 0.1 M), a precipitate is likely to form when barium nitrate solution is added to sodium hydroxide solution. However, considering any exceptions and the different factors that can affect solubility is essential for a more accurate prediction. You may need to consult additional references or experimental data to make a definitive conclusion for your specific situation.