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What is the pH of a solution containing 50.0g of (Na_3)(PO_4) in a liter of solution? We are given that (Na_3)(PO_4) is very basic.
You'll need to use the equilibrium constants, that's probably what your teacher/professor wants. I'll give you a general outline, although in most cases it's not the best way to learn the problem...What is the pH of a solution containing 50.0g of (Na_3)(PO_4) in a liter of solution? We are given that (Na_3)(PO_4) is very basic.
The pH of this solution would depend on the concentration of Na3PO4 and the equilibrium it forms in water. However, in general, the presence of a strong base like Na3PO4 would make the solution very basic, with a pH above 7.
To calculate the pH of a solution with a known amount of Na3PO4, you would need to determine the concentration of the solution, then use the concentration to calculate the concentration of the hydroxide ions present. From there, you can use the concentration of hydroxide ions to determine the pH using the equation pH = -log[OH-].
Yes, the pH of a solution containing Na3PO4 can change over time due to various factors such as the addition of other substances, changes in temperature, or the formation of new chemical equilibria.
The pH of a solution with Na3PO4 and a solution with NaOH can differ because they have different concentrations and form different equilibrium systems. Additionally, Na3PO4 is a weaker base compared to NaOH, so a solution with Na3PO4 would have a higher pH compared to a solution with the same molar concentration of NaOH.
Yes, the pH of a solution with Na3PO4 can be adjusted by adding an acid or base to the solution. This would change the concentration of the hydroxide ions and therefore affect the pH of the solution.