Calculate the pH of each of the following solutions...

Calculate the $\mathrm{pH}$ of each of the following solutions containing
a strong acid in water.
a. $2.0 \times 10^{-2} \mathrm{M} \mathrm{HNO}_{3}$
c. $6.2 \times 10^{-12} \mathrm{MHNO}_{3}$
b. $4.0 \mathrm{M} \mathrm{HNO}_{3}$

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Key Concepts

pH Calculation

The pH of a solution is defined as the negative base-10 logarithm of the hydrogen ion concentration. This definition is central to measuring and understanding the acidity of aqueous solutions, where lower pH values indicate higher acidity.

Strong Acid Ionization

Strong acids, such as HNO3, dissociate completely in water, meaning that they provide an amount of hydrogen ions equal to their initial concentration. This property simplifies pH calculations because the acid does not establish an equilibrium in solution.

Water Autoionization

Water autoionizes to produce hydrogen and hydroxide ions, typically at concentrations around 1.0×10?? M under standard conditions. In solutions where the acid concentration is extremely low, the contribution of these ions from water must be considered to accurately determine the pH.

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