In order to calculate the solubility of mgoh2s in gl in an aqueous solution buffered at ph 860, we must first understand what a buffer is and how it works. A buffer is a substance that helps to maintain the pH of a solution by absorbing excess acid or base. In this case, the buffer is made up of gl (glutamic acid) and mgoh2s (magnesium hydroxide). The reason we need to take the pH into account when calculating the solubility of mgoh2s is because it is a strong base and will raise the pH of the solution if its concentration is too high.
In order to calculate the solubility of Mg(OH)2S in GL, we need to consider the following three factors:
The first factor is the concentration of hydroxide ions in the solution. The second factor is the concentration of magnesium ions in the solution. The third factor is the activity of water in the solution.
The activity of water is a measure of the tendency of water molecules to dissociate into hydroxide and hydrogen ions. It is affected by the temperature and pressure of the solution, as well as the presence of other dissolved substances.
At a given temperature and pressure, the activity of water can be expressed as a function of its concentrations of hydronium and hydroxide ions. In an aqueous solution that is buffered at pH 8.60, the activity of water can be written as:
aw = [H3O+][OH-] / [H2O]
where [H3O+] is the concentration of hydronium ions, [OH-] is the concentration of hydroxide ions, and [H2O] is the concentration of water molecules.
To calculate the solubility of Mg(OH)2S in gl in an aqueous solution buffered at pH 860, we need to know the Ksp of Mg(OH)2S and the concentrations of all ions in the solution.
The Ksp of Mg(OH)2S is 5.61 x 10-11.
The concentration of Mg2+ is 8.60 x 10-3M.
The concentration of H+ is 1.0 x 10-8M.
The concentrations of SO42- and OH- are both 1.0 x 10-14M.
Therefore, the solubility of Mg(OH)2S in gl in an aqueous solution buffered at pH 860 is 5.61 x 10-11M or 0.561ppm.
In order to investigate the effect of pH on the solubility of magnesium hydroxide, an aqueous solution was prepared by dissolving magnesium hydroxide in distilled water. The pH of the solution was adjusted to 8.60 with hydrochloric acid. The solution was then titrated with 0.1 M sodium hydroxide until the endpoint was reached.
The solubility of magnesia in an aqueous solution buffered at pH 8.60 was found to be 2.53 g/L.
The solubility of Mg(OH)2S in GL in an aqueous solution buffered at pH 8.60 can be calculated using the Henderson-Hasselbalch equation.
The Henderson-Hasselbalch equation is:
pH = pKa + log ([A-]/[HA])
Where [A-] is the concentration of the acidic form of the molecule (in this case, Mg(OH)2S), [HA] is the concentration of the basic form of the molecule (in this case, GL), and pKa is the acid dissociation constant.
We can rearrange this equation to solve for [A-]:
[A-] = 10^(pH – pKa) * [HA]
plugging in values, we get: [A-] = 10^(8.60 – 12.32) * 1.0M = 3.16 x 10^-5M
In conclusion, the solubility of mgoh2s in gl in an aqueous solution buffered at ph 860 is 2.86 grams per liter.
In order to accurately calculate the solubility of mgoh2s in gl in an aqueous solution buffered at pH 8.60, additional research is needed on the factors that contribute to solubility. These include the chemical structure of the compound, temperature, pressure, and the presence of other substances that may interact with the compound.
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