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tobyracine
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Determine the equilibrium pH of aqueous solutions for the following strong acids or bases: (a) 257mg/L of HSO4- ; (b) 10nM NaOH ; (c) 75ug/L of HNO3
A strong acid is a chemical compound that completely dissociates in water, producing a high concentration of hydrogen ions (H+) and a low concentration of hydroxide ions (OH-). This results in a low pH value (below 7) in aqueous solutions.
The equilibrium pH of a strong acid solution is determined by the concentration of the acid and its dissociation constant, which is a measure of the strength of the acid. It can be calculated using the Henderson-Hasselbalch equation: pH = -log([H+]), where [H+] is the concentration of hydrogen ions in the solution.
The equilibrium pH of a strong acid solution can be affected by the concentration of the acid, temperature, and the presence of other substances that can interact with the acid. Additionally, changes in pressure or dilution of the solution can also impact the equilibrium pH.
The equilibrium pH of a strong acid solution is lower than that of a weak acid solution, as strong acids dissociate completely in water while weak acids only partially dissociate. This means that strong acids have a higher concentration of hydrogen ions, resulting in a lower pH value.
No, the equilibrium pH of a strong acid solution cannot be lower than 0 or higher than 14. The pH scale ranges from 0 to 14, with 0 being the most acidic and 14 being the most basic. A strong acid solution can have a pH value close to 0, but it cannot go below 0. Similarly, it can have a pH value close to 14, but it cannot go above 14.