Skip to main content
Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145당신이 사용하는 게 아니라요?교과서 변경
모든 교과서McMurry 8th EditionCh.16 - Aqueous Equilibria: Acids & Bases문제 112
16장, 문제 112

Write a balanced net ionic equation and the corresponding equilibrium equation for the reaction of the following weak bases with water. (c) Cyanide ion, CN

검증된 단계별 안내
1
Step 1: Write the reaction of the cyanide ion with water. The cyanide ion (CN-) acts as a base and accepts a proton (H+) from water, which acts as an acid. This results in the formation of hydrocyanic acid (HCN) and hydroxide ion (OH-). The reaction is: CN- + H2O -> HCN + OH-
Step 2: Since cyanide ion is a weak base, it does not completely ionize in water. Therefore, the reaction is reversible and we can write the equilibrium expression for the reaction. The equilibrium constant for the reaction of a base with water is known as the base ionization constant (Kb).
Step 3: Write the equilibrium equation. The equilibrium equation is the ratio of the product of the concentrations of the products to the product of the concentrations of the reactants, each raised to the power of their stoichiometric coefficients. For the reaction, the equilibrium equation is: Kb = [HCN][OH-] / [CN-]
Step 4: Note that the concentration of water is not included in the equilibrium expression. This is because water is a pure liquid and its concentration remains essentially constant during the reaction.
Step 5: The balanced net ionic equation and the corresponding equilibrium equation for the reaction of cyanide ion with water are: CN- + H2O <=> HCN + OH- and Kb = [HCN][OH-] / [CN-]

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
1m
도움이 되었나요?

주요 개념

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

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions. It focuses on the actual chemical change occurring in the solution. For weak bases, the net ionic equation typically shows the base accepting a proton from water, resulting in the formation of hydroxide ions and the conjugate acid of the base.
추천 영상:
가이드 코스
00:51
Net Ionic Equations

Weak Bases

Weak bases are substances that partially dissociate in water to produce hydroxide ions (OH⁻) and their conjugate acids. Unlike strong bases, which completely dissociate, weak bases establish an equilibrium between the undissociated base and its ions in solution. Understanding the behavior of weak bases is crucial for writing accurate chemical equations.
추천 영상:
가이드 코스
00:51
ICE Charts of Weak Bases

Equilibrium Constant (K)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a reversible reaction. For weak bases, the equilibrium expression is derived from the dissociation of the base in water. This concept is essential for understanding the extent of the reaction and predicting the direction in which the reaction will proceed.
추천 영상:
가이드 코스
01:14
Equilibrium Constant K
관련 실천
교과서 질문
Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) AgBr
463
views
교과서 질문
Oxycodone 1C18H21NO42, a narcotic analgesic, is a weak base with pKb = 5.47. Calculate the pH and the concentrations of all species present (C18H21NO4, HC18H21NO4 + , H3O+ , and OH-) in a 0.002 50 M oxycodone solution.
747
views
2
comments
교과서 질문
Calculate the concentrations of H3O+ and SO4 2- in a solution prepared by mixing equal volumes of 0.2 M HCl and 0.6 M H2SO41Ka2 for H2SO4 is 1.2 * 10-22.
537
views
교과서 질문
Strychnine 1C21H22N2O22, a deadly poison used for killing rodents, is a weak base having Kb = 1.8 * 10-6. Calculate the pH of a saturated solution of strychnine (16 mg/100 mL).
553
views