Calcule [H^+]de cada una de las disoluciones siguientes e...

Calcule $\left[\mathrm{H}^{+}\right]$de cada una de las disoluciones siguientes e indique si la disolución es ácida, básica oneutra: (a) $\left[\mathrm{OH}^{-}\right]$ $=0.00005 \mathrm{M}$; (b) $\left[\mathrm{OH}^{-}\right]=3.2 \times 10^{-9} \mathrm{M}$; (c) una disolución en la que $\left[\mathrm{OH}^{-}\right]$es 100 veces mayor que $\left[\mathrm{H}^{+}\right]$.

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Key Concepts

Ion Product of Water (Kw)

Kw is the equilibrium constant for the self-ionization of water, and at 25°C it has a value of 1.0×10?¹? M². This constant is crucial because it relates the concentrations of hydrogen ions [H?] and hydroxide ions [OH?] through the equation [H?][OH?] = Kw, allowing one to compute one ion concentration if the other is known.

Relationship between [H?] and [OH?]

Using the relation [H?] = Kw / [OH?], one can determine the concentration of hydrogen ions from the given concentration of hydroxide ions. This relationship is foundational in aqueous acid-base chemistry, providing a method to analyze and classify solutions based on their ion concentrations.

Acid-Base Classification

Solutions are classified as acidic when [H?] exceeds [OH?], basic when [OH?] is greater than [H?], and neutral when the concentrations are equal. This classification is essential for understanding the properties and behaviors of chemical solutions in various contexts.

pH and pOH Concepts

The pH of a solution is defined as the negative logarithm of the hydrogen ion concentration (pH = -log[H?]), while pOH is defined as -log[OH?]. At 25°C, these two scales are related by the equation pH + pOH = 14. These concepts provide a practical and intuitive way to express and compare the acidity or basicity of solutions.

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