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Ch.16 - Acid-Base Equilibria
Brown - Chemistry: The Central Science 15th Edition
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 15th EditionCh.16 - Acid-Base Equilibria문제 100
16장, 문제 100

A solution is made by adding 0.300 g Ca1OH221s2, 50.0 mL of 1.40 M HNO3, and enough water to make a final volume of 75.0 mL. Assuming that all of the solid dissolves, what is the pH of the final solution?

검증된 단계별 안내
1
Calculate the moles of Ca(OH)_2 using its molar mass.
Determine the moles of HNO_3 using its concentration and volume.
Write the balanced chemical equation for the reaction: Ca(OH)_2 + 2HNO_3 -> Ca(NO_3)_2 + 2H_2O.
Calculate the moles of H^+ ions remaining after the reaction, considering the stoichiometry of the reaction.
Use the concentration of remaining H^+ ions in the final solution volume to find the pH using the formula: pH = -log[H^+].

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
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6m

주요 개념

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

Dissociation of Calcium Hydroxide

Calcium hydroxide, Ca(OH)2, is a strong base that dissociates completely in water to produce calcium ions (Ca²⁺) and hydroxide ions (OH⁻). The dissociation reaction can be represented as Ca(OH)2 → Ca²⁺ + 2OH⁻. Understanding this dissociation is crucial for determining the concentration of hydroxide ions in the solution, which directly affects the pH.
추천 영상:
가이드 코스
06:12
Hydroxide Ion Concentration Example

Strong Acid-Base Neutralization

In this scenario, nitric acid (HNO3) is a strong acid that also dissociates completely in solution to yield hydrogen ions (H⁺). The reaction between the hydroxide ions from calcium hydroxide and the hydrogen ions from nitric acid leads to neutralization, forming water. The stoichiometry of this reaction is essential for calculating the resulting concentrations of H⁺ and OH⁻ ions, which ultimately determines the pH of the solution.
추천 영상:
가이드 코스
01:09
Strong Acid-Strong Base Titration

pH Calculation

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration: pH = -log[H⁺]. In a neutralization reaction, the final pH depends on the relative amounts of H⁺ and OH⁻ ions present after the reaction. If there is an excess of H⁺, the solution will be acidic (pH < 7), while an excess of OH⁻ will result in a basic solution (pH > 7).
추천 영상:
가이드 코스
02:15
pH Calculation Example
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