Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (a) \(0.75 \mathrm{~L}\) of \(1.5 \times 10^{-2} M \mathrm{KBr},\) (b) \(125 \mathrm{~g}\) of \(0.180 \mathrm{~m} \mathrm{KBr},\) (c) \(1.85 \mathrm{~L}\) of a solution that is \(12.0 \% \mathrm{KBr}\) by mass (the density of the solution is \(1.10 \mathrm{~g} / \mathrm{mL}\) ), (d) a \(0.150 \mathrm{M}\) solution of \(\mathrm{KBr}\) that contains just enough KBr to precipitate \(16.0 \mathrm{~g}\) of AgBr from a solution containing \(0.480 \mathrm{~mol}\) of \(\mathrm{AgNO}_{3}\)

(a) Calculate moles of KBr needed: moles of KBr = (1.5 × 10⁻² M) * (0.75 L). Convert moles to grams: mass of KBr = (moles of KBr) * (119 g/mol). Preparation: Weigh out the mass of KBr, dissolve in a 0.75 L volumetric flask, and fill with water. (b) Calculate molality: mass of solvent = (125 g) / (0.180 m). Calculate moles of KBr: moles of KBr = (0.180 m) * (mass of solvent in kg). Convert moles to grams: mass of KBr = (moles of KBr) * (119 g/mol). Preparation: Weigh out the mass of KBr, dissolve in the calculated mass of the solvent. (c) Calculate mass of KBr: mass of KBr = 0.12 * (1.10 g/mL) * (1.85 L * 1000 mL/L). Preparation: Weigh out the mass of KBr, dissolve in a 1.85 L volumetric flask, and fill with water. (d) Determine moles of AgBr: moles of AgBr = (16.0 g) / (187.8 g/mol). Calculate moles of KBr (equal to moles of AgBr). Convert moles to grams: mass of KBr = (moles of KBr) * (119 g/mol). Find volume: volume = moles of KBr / (0.150 M). Preparation: Weigh out the mass of KBr, dissolve in a volumetric flask of the calculated volume, and fill with water.