題目:
A solution contains 0.018 moles each of I-, Br-, and Cl-.When
the solution is mixed with 200mL of 0.24M AgNO3, how
much AgCl(s) precipitates out?
Ksp AgI=1.5*10-16(-16是指數,抱歉,沒辦法改成上標)
Ksp AgBr=5.0*10-13(-13是指數)
Ksp AgCl=1.6*10-10(-10是指數)
(A)0.0g (B)5.0g (C)3.3g (D)1.7g (E)2.6g
請會的人幫忙解答一下喔(希望可以給個詳解),感激不盡!!
普通化學 有關溶液的問題~
2009-07-03 7:56 pm
回答 (2)
2009-07-03 11:10 pm
✔ 最佳答案
The answer is D.
No. of moles of Ag+ added
= No of moles of AgNO3 added
= 0.24 x (200/1000)
= 0.048 mol
Ag+(aq) + I-(aq) → AgI(s)
Ag+(aq) + Br-(aq) → AgBr(s)
Ag+(aq) + Cl-(aq) → AgCl(s)
Ksp[KI(s)] >> Ksp[KBr(s)] >> Ksp[AgCl(s)]
Almost all I- ions are first precipitated.
No. of moles of Ag+ ions used = 0.018 mol
Amolst all Br- ions are then precipitated.
No. of moles of Ag+ ions used = 0.018 mol
No. of moles of Ag+ reacted with Cl- = 0.048 - (0.018 + 0.018) = 0.012 mol
No. of moles of AgCl formed = 0.012 mol
Molar mass of AgCl = 107.9 + 35.5 = 143.4 g/mol
Mass of AgCl formed = 0.012 x 143.4 = 1.7 g
=
2009-07-04 9:08 pm
收錄日期: 2021-04-29 18:23:14
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