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Mercury(I) ions (Hg22+) can be removed from solution by
Chapter 4, Problem 81E(choose chapter or problem)
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl-. Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
Questions & Answers
QUESTION:
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl-. Suppose that a solution contains aqueous Hg2(NO3)2. Write complete ionic and net ionic equations to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
ANSWER:Solution: Step1: a) In order to calculate the volume of 0.115 M HClO , we will use the 4utralization equation, i.e., M V1 M1V , 2e2 M and V are1 e molar1y and volume of the acid and M , V are the molarity and volume of the base. 2 2 Substituting the values of molarity and volume of the acid and base in the above equation, we get, 0.115 M X V = 0.0875 M X 50 mL 1 0.115 M X V = 4.31 (M X mL) V1 4.375 / 0.115 [(M X mL)/ mL] V1 38.04 mL Thus, required volume of HClO is 38.04 mL4 Step2: b) Mass of Mg(OH) = 2.87 g 2 Molar mass of Mg(OH) = 58.32 g/mol 2 Therefore, number of moles of Mg(OH) = 2.87 / 58.322 = 0.049 mol The reaction between HCl and Mg(OH) takes place in 2e following manner: 2HCl(aq) + Mg(OH) -----------> MgCl (aq) + 2H O 2 2 2 In the above equation, it is seen that, 1 mole of Mg(OH) requires 2 mole2of HCl for complete neutralization. Therefore, 0.049 moles of Mg