The number of hydronium ions in 1 ml of an aqueous solution of pH 12.0 at 25^∘ C is (a) 0.01 (b)

step 1 So in this question number of H3O positive ions, that is 1 into 10 x2 power minus 12 divided by

The number of hydronium ions in 1 ml of an aqueous solution...

The number of hydronium ions in $1 \mathrm{ml}$ of an aqueous solution of $\mathrm{pH} 12.0$ at $25^{\circ} \mathrm{C}$ is
(a) $0.01$
(b) $10^{-12}$
(c) $6.02 \times 10^{8}$
(d) $6.02 \times 10^{11}$

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Key Concepts

Avogadro's Number

Avogadro's number (approximately 6.02 x 10^23) defines the number of particles (atoms, molecules, ions) in one mole of substance. This concept enables the conversion of a substance’s amount in moles to the actual number of individual particles, allowing for quantitative analysis at the molecular or ionic level.

Hydronium Ion Concentration

Hydronium ion concentration represents the molar concentration of H3O+ ions in the solution. It is directly calculated from the pH value using the relationship [H3O+] = 10^(-pH) mol/L, which is essential for determining the number of hydrogen ions present in any given volume.

pH Scale

The pH scale is a logarithmic measure of the hydronium ion concentration in a solution, where each unit change corresponds to a tenfold change in concentration. It is defined as the negative logarithm (base 10) of the hydronium ion concentration, providing a convenient way to express the acidity or basicity of a solution.

Unit Conversion between Milliliters and Liters

Converting between milliliters and liters is crucial when working with molar concentrations, as concentration is typically expressed in moles per liter. Understanding that 1 mL is equivalent to 0.001 L helps accurately calculate the total number of moles present in a given volume.

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