8 ionic precipitation
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CHAPTER 8 : SALTS
IONICPRECIPITATION
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IONIC PRECIPITATE-An insoluble salt is prepared
through preipitate reation!
-In this reation" a#ueous solutionsontaining the ions o$ the insoluble
salt are %i&ed together to $or% the
salt!
-The insoluble salt $or%ed as apreipitate and an be obtained b'
$iltration!
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IONIC PRECIPITATE
-Che%ial and ioni
e#uations an be (ritten$or all reations
that are used to prepare
salts!
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E)A*PLE The $or%ation o$ preipitate o$ bariu% sulphate"
+aSO,!
Chemical reaction"
+aCl.a#/ 0 NaSO,.a#/ +aSO, .s/ 0 NaCl .a#/
+a00 Cl 0 Na00 SO,
-+aSO,
.s/ 0 Na0 0 Cl-
Ionic equations,
+a0 .a#/ 0 SO,-.a#/+aSO, .s/
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E)A*PLE -1hen a solution o$ sodiu% hloride reats
(ith sil2er nitrate!
Che%ial e#uations"NaCl .a#/ 0 AgNO3.a#/AgCl .s/ 0NaNO3.s/
Na00 Cl- 0 Ag0 0 NO-.a#/AgCl 0 Na0 0NO3-
Ioni e#uations"
Cl-.a#/ 0 Ag0 .a#/AgCl .s/
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E&eriseReactions can be represented using ionic equations.
Identify the two ionic equations that show the
neutralisation of an acid.
A. H+(aq + !H" (aq H#! (l
$. #H#! (l + !#(g +%e %!H"(aq
C. #H+ (aq + C!#"(aq H#! (l + C!#(g
&. '!#(g + H# (l #H+
(aq + #H+
(aq + '!)#"
(aq
*. H%+ (aq + !H"(aq H)(g + H#! (l
http://answer%20kimia.ppt/http://answer%20kimia.ppt/ -
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Constructing ionic equations
using the continuous ariation
method
- Can be used to onstrut ioni
e#uations $or the $or%ation
o$ insoluble salts!
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STEP.4/The nu%ber o$ %oles o$ ation and
anion that reat to $or% the salt is
deter%ined through ontinuous 2ariation
%ethod!
./The si%plest %ole ratio o$ ation to
anion that reat to $or% salt is
alulated!
.3/ The e%pirial $or%ula o$ the salt is
dedued!
.,/ +ased on the in$or%ation in ./" the
ioni e#uation $or the $or%ation an be
onstruted!
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E&a%ple
- cm)of .# mol dm")mercury solution
reacts completed with cm)of -. mol
dm")potassium iodide solution. A red
precipitate of mercury iodide is formed.
(aCalculate the simplest mole ratio of
mercury ions to iodide ions that reacts
with each other.
(b /hat is the empirical formula of
mercury iodide formed0
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./ 1rite do(n the ioni e#uations$or the preipitation o$ %erur'
iodide!
.d/ 1rite do(n the he%ial
e#uation $or the abo2e reation
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(aumber of moles of mercury ions in mercury
nitrate solution 1 23
1 .# ( - -
1 .# mol
umber of moles of iodide ions in potassium
iodide, 4I solution 1 23
1 -. ( -
1 . mol
Hence, the simplest mole ratio of mercury ion 5
iodide ion
1 .# 5 .1 .# 5 .
.# .#
1 - 5 #
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(b 6he empirical formula of mercury iodide is
Hg#
I.
(c 6he ionic equations for the precipitation
of mercury iodide is
Hg#+(aq + #I" HgI#(s
(d 6he chemical equation for the reaction is,
Hg(!)#(aq + #4I (aq HgI#(s +
#4!)(aq
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E&erise
cm)of -. mol dm")siler nitrate, Ag!)'olution was allowed to react completely
with magnesium chloride, 2gCl#solution to
form a siler salt.
(a /rite down the chemical and ionic
equations for the formation of siler
salt.
(b Calculate the mass of the siler saltprecipitated.
7Relatie atomic mass 5 Ag, -89 Cl, ).:
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