Please help! I have tried and still dont get how to do it. Thank you in advance!

Question

Please help! I have tried and still dont get how to do it. Thank you in advance!

To solve stoichiometry problems, you must always calculate numbers of moles. Recall that molarity, M, is equal to the concentration in moles per liter: M = mol/L. When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO_3(aq) + MgCl_2(aq) rightarrow 2AgCl(s) + Mg(NO_3)_2(aq) What mass of silver chloride can be produced from 1.92 L of a 0.101 M solution of silver nitrate? Express your answer with the appropriate units. The silver nitrate solution described in Part A required 3.99 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.

Explanation / Answer

V = 1.92 L iofM = 0.101 M of AGNO3

first, find mol of Ag+ possible to preciptate

mol = MV = 0.101*1.92 = 0.19392 mol of Ag+

since ratio is 1:1 with reapect of Ag+ and AgCl

expect 0.19392 mol of AgCl

mass = mol*MW= 0.19392*143.32 = 27.792 g of AgCl max

b)

V = 3.99 LK of MgCl2

find MgCl concnetration

0.19392 mol of Ag+ need 0.19392 mol of Ck-

since ratio is MgCl2 = 2Cl-

then

0.19392/2 = 0.09696 mol of MgCl2 are needed

M = mol/V = 0.09696/3.99 = 0.0243 M of MgCl2 solution

Related Questions

Navigate

• Browse (All)
• Browse P
• Subjects

---