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Key Question #4 - Lesson 4 Key Questions 16 a 2LiOH(aq...

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Lesson 4 Key Questions 16) a) 2LiOH (aq) + H 2 CO 3 (aq) Li 2 CO 3 (aq) + 2H 2 O (l) b) Cu(OH) 2 (aq) + 2HClO 3 (aq) Cu(ClO 3 ) 2 (aq) + 2H 2 O (l) c) 2Al(OH) 3 (aq) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 6H 2 O (l) d) HI (aq) + NH 3 (aq) + H 2 O (l) NH 4 I (aq) + H 2 O (l) 17) a) Cr (s) + 3Ag + (aq) Cr 3+ (aq) + 3Ag (s) b) No reaction c) No reaction d) 6H + (aq) + 3SO 4 2- (aq) Al 2 (SO 4 ) 3 (aq) e) Zn (s) + Pb 2+ (aq) Zn 2+ (aq) + Pb(s) 18) I would use phosphoric acid to precipitate the following salts: silver phosphate, barium metaphosphate and iron(III) phosphide. 9Ag (aq) + 2Ba (aq) + 3Fe (aq) + 6H 3 PO 4 (aq) 3Ag 3 PO 4 (s) + 2Ba(PO 3 ) 2 (s) + Fe 3 P (s) + 9H 2 (g) 19) molar mass BaF 2 = 175.3 g/mol n= CV n= ( 6.3 x 10 -3 mol/L x 0.2 L) n= 1.26 x 10 -3 mol m= (mol x g/mol) m= 1.204 mol x 10 -3 x 175.3 mol m=0.22 g Therefore 0.22 g of BaF 2 (s) is needed to produce 200 mL BaF 2 (aq) with a concentration of 6.3 x 10 -3 mol/L.
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20) In today’s age we have more industrial plants and car’s on the road then ever before. Although they are a necessity in today’s demand, they are also major contributors to acid rain. Acid rain is a form of precipitation which is much more acidic than usual. Clean or unpolluted rain usually has a
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