Skip to main content
Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 5th EditionCh.18 - Aqueous Ionic Equilibrium문제 90b
18장, 문제 90b

Use the given molar solubilities in pure water to calculate Ksp for each compound. b. Ag2SO3; molar solubility = 1.55⨉10-5 M c. Pd(SCN)2; molar solubility = 2.22⨉10-8 M

검증된 단계별 안내
1
Identify the dissolution equation for Ag_2SO_3: Ag_2SO_3(s) \(\rightleftharpoons\) 2Ag^+(aq) + SO_3^{2-}(aq).
Determine the relationship between molar solubility and ion concentrations: If the molar solubility of Ag_2SO_3 is s, then [Ag^+] = 2s and [SO_3^{2-}] = s.
Substitute the given molar solubility into the expressions for ion concentrations: [Ag^+] = 2(1.55 \(\times\) 10^{-5}) M and [SO_3^{2-}] = 1.55 \(\times\) 10^{-5} M.
Write the expression for the solubility product constant, K_{sp}: K_{sp} = [Ag^+]^2[SO_3^{2-}].
Substitute the ion concentrations into the K_{sp} expression and simplify: K_{sp} = (2 \(\times\) 1.55 \(\times\) 10^{-5})^2 \(\times\) (1.55 \(\times\) 10^{-5}).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m
도움이 되었나요?

주요 개념

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

Molar Solubility

Molar solubility is the number of moles of a solute that can dissolve in one liter of solution at a given temperature. It is a crucial measure in determining how much of a compound can be present in a saturated solution. In this context, the molar solubility of Ag₂SO₃ is given as 1.55×10⁻⁵ M, which indicates the maximum concentration of the compound that can dissolve in water.
추천 영상:
가이드 코스
04:13
Molar Solubility Example

Solubility Product Constant (Ksp)

The solubility product constant, Ksp, is an equilibrium constant that applies to the solubility of ionic compounds. It is defined as the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced equation. For Ag₂SO₃, Ksp can be calculated using the molar solubility to find the concentrations of Ag⁺ and SO₃²⁻ ions in a saturated solution.
추천 영상:
가이드 코스
01:47
Solubility Product Constant

Dissociation of Ionic Compounds

When ionic compounds dissolve in water, they dissociate into their constituent ions. For Ag₂SO₃, the dissociation can be represented as Ag₂SO₃(s) ⇌ 2Ag⁺(aq) + SO₃²⁻(aq). Understanding this dissociation is essential for calculating Ksp, as it allows us to relate the molar solubility to the concentrations of the ions produced in solution.
추천 영상:
가이드 코스
02:11
Ionic Compounds Naming
관련 실천
교과서 질문

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. BaCrO4; molar solubility = 1.08⨉10-5 M

1045
views
교과서 질문

Consider the compounds with the generic formulas listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp? a. AX; molar solubility = 1.35⨉10-4 M b. AX2; molar solubility = 2.25⨉10-4 M c. A2X; molar solubility = 1.75⨉10-4 M

924
views
교과서 질문

Use the given molar solubilities in pure water to calculate Ksp for each compound. a. MX; molar solubility = 3.27⨉10-11 M

479
views
교과서 질문

Two compounds with general formulas AX and AX2 have Ksp = 1.5⨉10-5. Which of the two compounds has the higher molar solubility?

1044
views
교과서 질문

The solubility of copper(I) chloride is 3.91 mg per 100.0 mL of solution. Calculate Ksp for CuCl.

1345
views
교과서 질문

Use the given molar solubilities in pure water to calculate Ksp for each compound. b. PbF2; molar solubility = 5.63⨉10-3 M c. MgF2; molar solubility = 2.65⨉10-4 M

2196
views
1
rank