Question

A 25.0 mL sample of 0.15 M silver nitrate, AgNO3, is reacted with a 3.58 g sample of calcium chloride, CaCl2 (M = 111.0). Which of the following statements is true?

(A) Silver nitrate is the limiting reactant and calcium nitrate precipitates
(B) Silver nitrate is the limiting reactant and silver chloride precipitates.
(C) Calcium chloride is the limiting reactant and calcium nitrate precipitates.
(D) Calcium chloride is the limiting reactant and silver chloride precipitates.
Which aqueous solution exhibits the largest freezing point depression?
(A) 1.0 m KBr (C) 0.5 m MgCl2
(B) 0.75 m C6H12O6 (D) 0.25 m Ga2(SO4)3

Answer 1

The limiting reactant in the reaction between silver nitrate and calcium chloride is silver nitrate, and silver chloride precipitates.

Step-by-step explanation:

The balanced chemical equation for the reaction between silver nitrate, AgNO3, and calcium chloride, CaCl2, is:

AgNO3(aq) + CaCl2(aq) → AgCl(s) + Ca(NO3)2(aq)

To determine the limiting reactant, we need to compare the moles of each reactant to the stoichiometric ratio. In this case, we have:

Moles of AgNO3 = volume (L) × molarity (M) = 0.025 L × 0.15 M = 0.00375 mol

Moles of CaCl2 = mass (g) / molar mass (g/mol) = 3.58 g / 111.0 g/mol = 0.0323 mol

The smaller value is 0.00375 mol, which corresponds to the moles of AgNO3. Therefore, silver nitrate is the limiting reactant.

Since the stoichiometry of the reaction is one-to-one, we will form 0.00375 mol of AgCl.

The correct answer is (B) Silver nitrate is the limiting reactant and silver chloride precipitates.