The hydronium ion concentration in an aqueous solution of H2 SO4 is 2.0 ×10^-4 M at 25^∘ C. The

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The hydronium ion concentration in an aqueous solution of H2...

The hydronium ion concentration in an aqueous solution of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is $2.0 \times 10^{-4} \mathrm{M}$ at $25^{\circ} \mathrm{C}$. The hydroxide ion concentration in the solution is (a) 0 (b) $2.0 \times 10^{-4} \mathrm{M}$ (c) $5 \times 10^{3} \mathrm{M}$ (d) $5 \times 10^{-11} \mathrm{M}$

The hydronium ion concentration in an aqueous solution of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is $2.0 \times 10^{-4} \mathrm{M}$
at $25^{\circ} \mathrm{C}$. The hydroxide ion concentration in the solution is
(a) 0
(b) $2.0 \times 10^{-4} \mathrm{M}$
(c) $5 \times 10^{3} \mathrm{M}$
(d) $5 \times 10^{-11} \mathrm{M}$

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Key Concepts

Water Ion-Product Constant (Kw)

This concept refers to the equilibrium constant for the autoionization of water, where water molecules dissociate into hydronium and hydroxide ions. At a given temperature, typically 25°C, the product of the concentrations of these ions remains constant. This relationship is crucial for determining one ion concentration when the other is known in aqueous solutions.

Acid-Base Equilibrium

Acid-base equilibrium involves the balance between acids and bases in a solution, where the concentration of hydronium ions (from acids) and hydroxide ions (from bases) are interrelated through the water ion-product constant. This concept helps in understanding how the addition of an acid or base affects the overall pH of the solution.

Strong Acid Dissociation

A strong acid, such as those that fully dissociate in water, releases a high concentration of hydronium ions upon dissolution. This complete dissociation simplifies calculations in aqueous solutions since the acid is assumed to contribute all of its protons, making it easier to use equilibrium constants to determine ion concentrations.

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