This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Understand the term "equimolar solutions". "Equimolar solutions" means that the molar concentrations of Fe^3+(aq) and SCN^-(aq) are equal. Let this concentration be C mol/cm^3. Step 2: Calculate the moles of Fe^3+ ions used. Volume of Fe^3+ ions = 5 cm^3 Moles of Fe^3+ = Concentration × Volume = C × 5 mol Step 3: Calculate the moles of SCN^- ions used. Volume of SCN^- ions = 5 cm^3 Moles of SCN^- = Concentration × Volume = C × 5 mol Step 4: Determine the mole ratio of Fe^3+ to SCN^- at maximum colour intensity. Maximum colour intensity indicates the stoichiometric ratio at which the complex is formed. The ratio of moles of Fe^3+ to SCN^- is: Moles of Fe^3+Moles of SCN^- = C × 5 molC × 5 mol = (1)/(1) This means that one Fe^3+ ion combines with one SCN^- ion to form the complex. Step 5: Determine the formula and charge of the complex ion. The central metal ion is Fe^3+. The ligand is SCN^-. Since the ratio is 1:1, the complex will contain one Fe and one SCN. The charge of the complex is the sum of the charges of the metal ion and the ligand: Charge = (+3) + (-1) = +2 Therefore, the formula of the complex ion is [Fe(SCN)]^2+. The formula of the complex ion is: [Fe(SCN)]^2+ 3 done, 2 left today. You're making progress.