Calculate the pH of a solution having the following ion concentrations at 298 K. [H+] = 4.6 × 10^-2 M

The pH of the solution is 1.34, being an acidic pH.

Explanation:

pH is a measure of acidity or alkalinity that indicates the amount of hydrogen ions present in a solution or substance.   The acronym pH stands for hydrogen potential.

The pH scale ranges from 0 to 14. Values less than 7 indicate the acidity range and those greater than 7 indicate alkalinity or basicity. Value 7 is considered neutral. Mathematically, pH is the negative logarithm of the molar concentration of hydrogen or proton ions (H⁺) or hydronium ions (H₃O⁺).

pH= - log [H⁺] = - log [H₃O⁺]

In this case, [H⁺]= 4.6*10⁻² M. Replacing:

pH= - log 4.6*10⁻²

Solving:

pH= 1.34

The pH of the solution is 1.34, being an acidic pH.

i would say b

explanation:

but i think i would need more information than that

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