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10. A 10.0 mL sample of 0.100 M KPO, is added to 20.0 mL of 0.300 M AgNO2. Silver The concentration of Ag ions in solution AFTER reaction phosphate precipitates. is, (A) 0.030 M (B) 0.100 MM (C) 0.200 M (D) 0.300 AM 11. The lattice energy of a salt is related to t he energy required to separate the ions. Which represents the correct order of the relative lattice energies for the ionic solids below? NaCl, CaO, KI, Mgo (A) KI < MgO < NaCl < Ca0 (B) KI < NaCl < CaO< Mgo (C) NaCl < KI< CaO < Mgo (D) NaCl < CaO < MgO< K

Answer 1

Approach: 1)Write balanced molecular equation

2)Determine moles of AgNO₃ and K₃PO₄

3)Calculate remaining moles of Ag⁺

4)Calculate molarity of Ag⁺

Write balanced molecular equation Determine moles of AgNO_3 and K_3 PO_4 Calculate remaining moles of Ag^+ Calculate molarity of Ag^+ 3 AgNO_3 + k_3 PO_4 rightarrow Ag_3 PO_4 + 3KNO_3 So 1 mole of K_3 PO_4 reacts with 3 moles of AgNO_3 Moles of AgNO_3 present = 20 times 0.300/1000 moles = 0.006 moles Moles of K_3 PO_4 added = 10 times 0.100/1000 moles = 0.001 moles Hence, 0.001 moles of K_3 PO_4 reacts with (3 times 0.001) or 0.003 moles of AgNO_3 So moles of AgNO_3 left after reaction = (0.006 - 0.003) moles = 0.003 moles. 1 moles of AgNO_3 produces 0.003 moles of Ag^+ Total volume of reaction mixture = (20 + 10)mL = 30 mL therefore concentration of Ag^+ after reaction = 0.003/30 times 1000(M) = 0.100 (M)