Calculate [H^+] and pH in a solution in which lactic acid, HC3 H5 O3, is 0.250 M and the lactate

step 1 Okay, so we're being asked to find the H plus concentration and the pH of several buffer solutio

Calculate [H^+] and pH in a solution in which lactic acid,...

Calculate $\left[\mathrm{H}^{+}\right]$ and $\mathrm{pH}$ in a solution in which lactic acid, $\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3},$ is $0.250 \mathrm{M}$ and the lactate ion, $\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{3}-,$ is (a) $0.250 \mathrm{M}$ (b) $0.125 \mathrm{M}$ (c) $0.0800 \mathrm{M}$ (d) $0.0500 \mathrm{M}$

Calculate $\left[\mathrm{H}^{+}\right]$ and $\mathrm{pH}$ in a solution in which lactic acid, $\mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{3},$ is $0.250 \mathrm{M}$ and the lactate ion, $\mathrm{C}_{3} \mathrm{H}_{5} \mathrm{O}_{3}-,$ is
(a) $0.250 \mathrm{M}$
(b) $0.125 \mathrm{M}$
(c) $0.0800 \mathrm{M}$
(d) $0.0500 \mathrm{M}$

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Key Concepts

Acid-Base Equilibrium

This concept involves the balance between protons (H+) and their conjugate bases in solution. Weak acids, like lactic acid, do not fully dissociate in water but establish an equilibrium between the undissociated acid and the ions produced, which is fundamental to understanding and calculating pH.

Buffer Solutions

A buffer solution contains a weak acid and its conjugate base in appreciable amounts, allowing the solution to resist changes in pH upon the addition of small amounts of acid or base. The interplay between the acid and its conjugate base determines the pH of the buffer.

Henderson-Hasselbalch Equation

This equation provides a convenient way to calculate the pH of a buffer solution by relating the pH to the pKa of the acid and the ratio of the concentrations of the conjugate base to the weak acid. It is especially useful when the solution components are known and are in similar concentrations.

Acid Dissociation Constant (Ka) and pKa

Ka is a quantitative measure of the strength of a weak acid in solution, indicating the extent of its dissociation. The pKa, the negative logarithm of Ka, is used in conjunction with the Henderson-Hasselbalch equation to simplify the calculation of pH in acid-base equilibria.

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