10 public questions tagged with this topic.
In [Ni(NH₃)4Cl₂]Cl₂, the 2 Cl− ions outside the coordination sphere are ionizable and precipitate as AgCl, while the 2 inside are ligands. Thus, 2 moles form.
Ref: NCERT Class 12 Chemistry > Chapter 5: Coordination Compounds > Topic: Werner's Theory and Definitions - Ligands Coordination Number
In [Co(H₂O)4Cl₂]Cl, the 1 Cl− outside the coordination sphere is ionizable and forms AgCl, while the 2 inside are ligands. Thus, 1 mole precipitates.
Ref: NCERT Class 12 Chemistry > Chapter 5: Coordination Compounds > Topic: Werner's Theory and Definitions - Ligands Coordination Number
Molar mass of AgCl = 143.5 g/mol, Cl = 35.5 g/mol. Mass of Cl = (35.5/143.5) × 0.235 = 0.058 g. Percentage = (0.058/0.2) × 100 = 29%.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Qualitative and Quantitative Analysis - Lassaigne Test and Estimation
Molar mass of AgCl = 143.5 g/mol, Cl = 35.5 g/mol. Mass of Cl = (35.5/143.5) × 0.287 = 0.071 g. Percentage = (0.071/0.18) × 100 ≈ 39.44% ≈ 40%.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Qualitative and Quantitative Analysis - Lassaigne Test and Estimation
Mass of Cl = (35.5/143.5) × 0.287 = 0.071 g. Percentage = (0.071/0.15) × 100 = 47.33% ≈ 47%. Kjeldahl’s data is for nitrogen, irrelevant here.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Qualitative and Quantitative Analysis - Lassaigne Test and Estimation
Mass of Cl = (35.5/143.5) × 0.47 ≈ 0.116 g. Mass of S = (32/233) × 0.233 ≈ 0.032 g. Ratio = 0.116/0.032 ≈ 3.625:1, which rounds to 4:1 for practical purposes.
Ref: NCERT Class 11 Chemistry > Chapter 8: Organic Chemistry - Some Basic Principles and Techniques > Topic: Qualitative and Quantitative Analysis - Lassaigne Test and Estimation
Ksp = [Ag+][Cl-] = S² = 1.8 × 10⁻¹⁰ , so S = sqrt1.8 × 10⁻¹⁰ = 1.34 × 10⁻⁵ mol/L .
Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Buffer Solutions and Solubility Product and Common Ion Effect
Reaction: AgNO₃ + NaCl → AgCl + NaNO₃. Moles of AgNO₃ = 34/170 = 0.2 mol. 1 mol AgNO₃ produces 1 mol AgCl; mass = 0.2 × 143.5 = 28.7 g.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Stoichiometry and Stoichiometric Calculations and Limiting Reagent
Reaction: AgNO₃ + NaCl → AgCl + NaNO₃. Moles of AgNO₃ = 17/170 = 0.1 mol. 1 mol AgNO₃ produces 1 mol AgCl; mass = 0.1 × 143.5 = 14.35 g.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Importance and Nature of Chemistry and Properties of Matter
Reaction: AgNO₃ + NaCl → AgCl + NaNO₃. Moles of AgCl = 5.75/143.5 ≈ 0.04 mol. 1 mol AgCl from 1 mol AgNO₃; mass = 0.04 × 170 = 6.8 g.
Ref: NCERT Class 11 Chemistry > Chapter 1: Some Basic Concepts of Chemistry > Topic: Dalton's Atomic Theory and Atomic and Molecular Masses
