Determine the [H₃O⁺] and pH of a 0.200 M solution of formic acid.

검증된 단계별 안내

Identify the chemical formula for formic acid, which is HCOOH.

Write the dissociation equation for formic acid in water: \( \text{HCOOH} + \text{H}_2\text{O} \rightleftharpoons \text{H}_3\text{O}^+ + \text{HCOO}^- \).

Use the acid dissociation constant \( K_a \) for formic acid, which is typically given or can be found in a reference table.

Set up an ICE (Initial, Change, Equilibrium) table to determine the concentrations of the species at equilibrium.

Use the expression for \( K_a = \frac{[\text{H}_3\text{O}^+][\text{HCOO}^-]}{[\text{HCOOH}]} \) to solve for \([\text{H}_3\text{O}^+]\), and then calculate the pH using \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Acid-Base Chemistry

Acid-base chemistry involves the study of substances that can donate protons (H+) or accept protons. In this context, formic acid (HCOOH) is a weak acid that partially dissociates in water to produce H3O+ ions. Understanding the behavior of weak acids is crucial for calculating the concentration of hydronium ions in solution.

Dissociation Constant (Ka)

The dissociation constant (Ka) quantifies the strength of an acid in solution. For formic acid, Ka is used to determine the extent of its dissociation into H3O+ and its conjugate base (HCOO-). This constant is essential for calculating the equilibrium concentrations of the species in the solution.

pH Calculation

pH is a measure of the acidity of a solution, defined as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+]. To find the pH of the formic acid solution, one must first determine the concentration of H3O+ using the dissociation constant and then apply the pH formula. This relationship is fundamental in acid-base chemistry.

Determine the [H3O+] and pH of a 0.200 M solution of formic acid.

비슷한 문제에 대한 검증된 영상 답변:

주요 개념

Acid-Base Chemistry

Dissociation Constant (K<sub>a</sub>)

pH Calculation

Determine the [H₃O⁺] and pH of a 0.200 M solution of formic acid.