Lime Dosing
Transcript of Lime Dosing
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Softening
cations mg/l eq.wt mg/l as CaCO3 Anions mg/l eq.wt
Ca2+
1073 20 2682.5 CO32-
0 30
Mg2+
574 12.2 2352.5 HCO3-
46 61
Na+
10165 23 22097.8 Cl-
16415 35.5
Fe2+
1.12 27.9225 2.0 SO42-
3750 48
Concentration
H+
1.94984E-08
HCO3-
0.0009
Ka 4.46684E-07
H2CO3 3.92864E-05
Therefore CO2 = H2CO3
Mol wt of CO2 44.0 g
CO2 1.728602696 1000.0 mg
CO2 3.92864249
Mg2+ Fe+
5038.9 27138.7
37.7
3.93 HCO3-
CO2 3.93
Ca carbonate
hardness 37.7
Mg Carbonate
hardness 0
excess lime 20
Amount of lime
(CaOH)2 required 61.63491803
Mg2+ Fe+
5001.2 27101.0
After the Carbonate Hardness is removed
CO2
Ca2+ Na+
2648.7 27099.0
1) Note: Ca & Mg g
2) first step to remove carbonate hardness
association with Ca & Mg.
alkalinity exist in the form of HCO3-& there w
the alkalinty exist as OH-
so either forms carbonic acid or HCo3- depen
precipitate calcicum and Magnesium carbonat
ness forms CaCO3 which precipitaes
MgCO3 which is soluble and does'nt get rem
convert MgCO3 to Mg(OH)2 which
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
Cl- SO42-
Amount of lime required = (CO2 + Ca carbonate hardness + Mg Carbonate hardness + excess Lime)
Na+
H2CO3 = [H+] x [HCO3
-]/[Ka1], mol/l
expressing CO2 in terms of mg/l
CO2 2686.4 27136.7
23157.4 27063.7
Availability of CO2 @ Ph 7.7
Assume all of H2CO3 forms CO2
expressing CO2 in terms of mg/l as CaCO3
mg/l as CaCO3
Ca2+
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3.93
Ca Non
carbonate
hardness 2648.7
Mg NonCarbonate
hardness 2352.5
Amount of Soda
Ash required 5001.2
Mg Non
Carbonate
hardness 2352.5
Lime 2414.093934
Soda Ash 4494.2
After Ca & Mg being removed
Fe+
24182.3
3.93 Cl- SO42-
CO2
Na+
34748.9
12584.5 17355.3
Cl- SO42-
Amount of Soda Ash required = (Ca Non carbonate hardness + Mg Non Carbonate hardness)
1)Calcium Non Carbonate Hardne2)CaCl2 Or CaSO4 reacts with Na2CO3 and for
dose
3)Mg Non Carbonate Hardness could
4)Firstly Mg Non Corbonate is added with
contributes har
5)secondly Lime is added which reacts with
leaves behind Nacl and Na2SO4 which is
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
23119.7 27026.0
mg/l as CaCO3
Amount of Lime required = ( Mg Non Carbonate hardness)
Total Amount of dosage required
mg/l as CaCO3
mg/l as CaCO3
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mg/l as CaCO3 pH 7.71
0.0 pKa 6.35 at 25C
37.7
23119.7
3906.3
26630.8616380354
27063.7
t to be precipitated to remove hardness.
hich is formed by (HCO3-,CO3
2-,OH
--Contributes to Alkalinity) in
3) At pH < 8.3
ould be presence of CO2 4) At pH > 8.3 all of
5) CO32-
is not stableing upon pH 6) Lime Ca(OH)2 is used to
e hardness 7) Lime + calcium Carbonate hard
8) Lime + Mg Carbonate Hardness forms
oved 9) So further addition of lime is required to
precipitaes 10) finally excess lime is added
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Note:
ss could be removed by addition of Soda Ash (Na2CO3)s CaCO3 which precipitaes and NaCl,Na2SO4 which dissolves and
nt contribute to hardness
be removed by addition of both Lime & Soda Ash (Na2CO3)
CaCO3 ,here MgCO3 is formed which is a soluble product and
dness along with this CaCl2 r CaSO4 .
gCO3 and forms Mg(OH)2 & CaCO3 a product that precipitaes .and
a soluble and non-hardness product, but contributes to TDS.
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Softening
cations mg/l eq.wt mg/l as CaCO3 Anions mg/l eq.wt
Ca2+
942 20 2355.0 CO32-
0 30
Mg2+
530 12.2 2172.1 HCO3-
45 61
Na+
5921 23 12871.7 Cl-
8935 35.5
Fe2+
0.1 27.9225 0.2 SO42-
4580 48
Concentration
H+
1.94984E-08
HCO3-
0.0009
Ka 4.46684E-07
H2CO3 3.92864E-05
Therefore CO2 = H2CO3
Mol wt of CO2 44.0 g
CO2 1.728602696 1000.0 mg
CO2 3.92864249
Mg2+ Fe+
4531.1 17403.0
36.9
3.93 HCO3-
CO2 3.93
Ca carbonate
hardness 36.9
Mg Carbonate
hardness 0
excess lime 20Amount of lime
(CaOH)2
required 60.8152459
Mg2+ Fe+
4494.2 17366.12322.0 17365.9
17392.2
Ca2+ Na+
1) Note: Ca & Mg g
2) first step to remove carbonate hardness
association with Ca & Mg.
alkalinity exist in the form of HCO3-& there w
the alkalinty exist as OH-
so either forms carbonic acid or HCo3- depen
precipitate calcicum and Magnesium carbonat
ness forms CaCO3 which precipitaes
forms MgCO3 which is soluble and does'nt get
to convert MgCO3 to Mg(OH)2 whic
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
Availability of CO2 @ Ph 7.7
H2CO3 = [H+] x [HCO3
-]/[Ka1], mol/l
Assume all of H2CO3 forms CO2
expressing CO2 in terms of mg/l
expressing CO2 in terms of mg/l as CaCO3
17402.8
mg/l as CaCO3
CO2
CO2
2358.9
mg/l as CaCO3
mg/l as CaCO3
SO42-
12621.4
Cl-
Amount of lime required = (CO2 + Ca carbonate hardness + Mg Carbonate hardness + excess Lime)
After the Carbonate Hardness is removed
Ca2+ Na+
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3.93
Ca Non
carbonate
hardness 2322.0Mg Non
Carbonate
hardness 2172.1
Amount of Soda
Ash required 4494.174544
Mg Non
Carbonate
hardness 2172.1
Lime 2232.946393
Soda Ash 4494.174544
After Ca & Mg being removed
Fe+
24182.3
3.93
mg/l as CaCO3
Amount of Soda Ash required = (Ca Non carbonate hardness + Mg Non Carbonate hardness)
1)Calcium Non Carbonate Hardne
2)CaCl2 Or CaSO4 reacts with Na2CO3 and for
dose
3)Mg Non Carbonate Hardness could
4)Firstly Mg Non Corbonate is added with
contributes ha
5)secondly Lime is added which reacts with
leaves behind Nacl and Na2SO4 which is
mg/l as CaCO3
mg/l as CaCO3
Amount of Lime required = ( Mg Non Carbonate hardness)
12584.5 17355.3
mg/l as CaCO3
Cl- SO42-
mg/l as CaCO3
Total Amount of dosage required
CO2
12584.5 17355.3Cl- SO42-
Na+
24182.1
mg/l as CaCO3
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mg/l as CaCO3 pH 7.71
0.0 pKa 6.35 at 25C
36.9
12584.5
4770.8
17402.9481974954
17392.2
t to be precipitated to remove hardness.
hich is formed by (HCO3-,CO3
2-,OH
--Contributes to Alkalinity) in
3) At pH < 8.3
uld be presence of CO2 4) At pH > 8.3 all of
5) CO3
2-is not stable
ing upon pH 6) Lime Ca(OH)2 is used to
e hardness 7) Lime + calcium Carbonate hard
8) Lime + Mg Carbonate Hardness
removed 9) So further addition of lime is required
precipitaes 10) finally excess lime is added
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Note:
ss could be removed by addition of Soda Ash (Na2CO3)
s CaCO3 which precipitaes and NaCl,Na2SO4 which dissolves and
nt contribute to hardness
e removed by addition of both Lime & Soda Ash (Na2CO3)
CaCO3 ,here MgCO3 is formed which is a soluble product and
dness along with this CaCl2 r CaSO4 .
gCO3 and forms Mg(OH)2 & CaCO3 a product that precipitaes .and
a soluble and non-hardness product, but contributes to TDS.
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Softening
cations mg/l eq.wt mg/l as CaCO3 Anions mg/l eq.wt
Ca2+
319 20 797.5 CO32-
0 30
Mg2+
177 12.2 725.4 HCO3-
65 61
Na+
7311 23 15893.5 Cl-
9928 35.5
Fe2+
0 27.9225 0.0 SO42-
3235 48
Concentration
H+
1.94984E-08
HCO3-
0.0013
Ka 4.46684E-07
H2CO3 5.67471E-05
Therefore CO2 = H2CO3
Mol wt of CO2 44.0 g
CO2 2.49687056 1000.0 mg
CO2 5.674705819
Mg2+ Fe+
1528.6 17422.1
53.3
5.67 HCO3-
CO2 5.67
Ca carbonate
hardness 53.3
Mg Carbonate
hardness 0
excess lime 20
Amount of lime
(CaOH)2 required 78.94868852
Mg2+ Fe+
1475.3 17368.8
5.67
mg/l as CaCO3
Availability of CO2 @ Ph 7.7
H2CO3 = [H+] x [HCO3
-]/[Ka1], mol/l
Assume all of H2CO3 forms CO2
expressing CO2 in terms of mg/l
expressing CO2 in terms of mg/l as CaCO3
CO2
Ca2+ Na+
803.2 17422.1
14036.4 17406.2
Cl- SO42-
Amount of lime required = (CO2 + Ca carbonate hardness + Mg Carbonate hardness + excess Lime)
1) Note: Ca & Mg g
2) first step to remove carbonate hardness
association with Ca & Mg.
alkalinity exist in the form of HCO3-& there w
the alkalinty exist as OH-
so either forms carbonic acid or HCo3- depen
precipitate calcicum and Magnesium carbonat
ness forms CaCO3 which precipitaes
MgCO3 which is soluble and does'nt get remconvert MgCO3 to Mg(OH)2 which
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
After the Carbonate Hardness is removed
CO2
Ca2+ Na+
749.9 17368.8
13983.1 17352.9
Cl- SO42-
Amount of Soda Ash required = (Ca Non carbonate hardness + Mg Non Carbonate hardness)
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Ca Non
carbonate
hardness 749.9
Mg Non
Carbonate
hardness 725.4
Amount of SodaAsh required 1475.3
Mg Non
Carbonate
hardness 725.4
Lime 804.3585246
Soda Ash 1475.3
After Ca & Mg being removed
Fe+
24182.3
3.93
Na+
19594.0
1)Calcium Non Carbonate Hardne
2)CaCl2 Or CaSO4 reacts with Na2CO3 and for
dose
3)Mg Non Carbonate Hardness could
4)Firstly Mg Non Corbonate is added withcontributes har
5)secondly Lime is added which reacts with
leaves behind Nacl and Na2SO4 which is
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
12584.5 17355.3
Cl- SO42-
Amount of Lime required = ( Mg Non Carbonate hardness)
mg/l as CaCO3
Total Amount of dosage required
mg/l as CaCO3
mg/l as CaCO3
CO2
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mg/l as CaCO3 pH 7.71
0.0 pKa 6.35 at 25C
53.3
13983.1
3369.8
t to be precipitated to remove hardness.
hich is formed by (HCO3-,CO3
2-,OH
--Contributes to Alkalinity) in
3) At pH < 8.3
ould be presence of CO2 4) At pH > 8.3 all of
5) CO32-
is not stable
ing upon pH 6) Lime Ca(OH)2 is used to
e hardness 7) Lime + calcium Carbonate hard
8) Lime + Mg Carbonate Hardness forms
oved 9) So further addition of lime is required toprecipitaes 10) finally excess lime is added
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Note:
ss could be removed by addition of Soda Ash (Na2CO3)
s CaCO3 which precipitaes and NaCl,Na2SO4 which dissolves and
nt contribute to hardness
be removed by addition of both Lime & Soda Ash (Na2CO3)
CaCO3 ,here MgCO3 is formed which is a soluble product anddness along with this CaCl2 r CaSO4 .
gCO3 and forms Mg(OH)2 & CaCO3 a product that precipitaes .and
a soluble and non-hardness product, but contributes to TDS.
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Softening
cations mg/l eq.wt mg/l as CaCO3 Anions mg/l eq.wt
Ca2+
699 20 1747.5 CO32-
0 30
Mg2+
367 12.2 1504.1 HCO3-
66 61
Na+
6204 23 13487.0 Cl-
9325 35.5
Fe2+
0 27.9225 0.0 SO42-
3400 48
Concentration
H+
1.94984E-08
HCO3-
0.00132
Ka 4.46684E-07
H2CO3 5.76201E-05
Therefore CO2 = H2CO3
Mol wt of CO2 44.0 g
CO2 2.535283954 1000.0 mg
CO2 5.762008986
Mg2+ Fe+
3257.3 16744.2
54.1
5.67 HCO3-
CO2 5.67
Ca carbonate
hardness 54.1
Mg Carbonate
hardness 0
excess lime 20Amount of lime
(CaOH)2
required 79.76836066
Mg2+ Fe+
3203.2 16690.1
After the Carbonate Hardness is removed
CO2
Ca2+ Na+
1699.1 16690.1
Cl-
SO42-
Amount of lime required = (CO2 + Ca carbonate hardness + Mg Carbonate hardness + excess Lime)
1) Note: Ca & Mg g
2) first step to remove carbonate hardness
association with Ca & Mg.
alkalinity exist in the form of HCO3-& there w
the alkalinty exist as OH-
so either forms carbonic acid or HCo3- depen
precipitate calcicum and Magnesium carbonat
ness forms CaCO3 which precipitaes
forms MgCO3 which is soluble and does'nt get
to convert MgCO3 to Mg(OH)2 whic
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
CO2
Ca2+ Na+
1753.2 16744.2
13187.9 16729.6
Availability of CO2 @ Ph 7.7
H2CO3 = [H+] x [HCO3
-]/[Ka1], mol/l
Assume all of H2CO3 forms CO2
expressing CO2 in terms of mg/l
expressing CO2 in terms of mg/l as CaCO3
mg/l as CaCO3
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5.67
Ca Non
carbonate
hardness 1699.1Mg Non
Carbonate
hardness 1504.1
Amount of Soda
Ash required 3203.2
Mg Non
Carbonate
hardness 1504.1
Lime 1583.866721
Soda Ash 3203.2
After Ca & Mg being removed
Fe+
24182.3
3.93 Cl- SO42-
Amount of Lime required = ( Mg Non Carbonate hardness)
mg/l as CaCO3
Total Amount of dosage required
mg/l as CaCO3
mg/l as CaCO3
CO2
Na+
21592.4
12584.5 17355.3
Cl- SO42-
Amount of Soda Ash required = (Ca Non carbonate hardness + Mg Non Carbonate hardness)
1)Calcium Non Carbonate Hardne
2)CaCl2 Or CaSO4 reacts with Na2CO3 and for
dose
3)Mg Non Carbonate Hardness could
4)Firstly Mg Non Corbonate is added with
contributes ha
5)secondly Lime is added which reacts with
leaves behind Nacl and Na2SO4 which is
mg/l as CaCO3
mg/l as CaCO3
mg/l as CaCO3
13133.8 16675.5
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mg/l as CaCO3 pH 7.71
0.0 pKa 6.35 at 25C
54.1
13133.8
3541.7
t to be precipitated to remove hardness.
hich is formed by (HCO3-,CO3
2-,OH
--Contributes to Alkalinity) in
3) At pH < 8.3
uld be presence of CO2 4) At pH > 8.3 all of
5) CO32-
is not stable
ing upon pH 6) Lime Ca(OH)2 is used to
e hardness 7) Lime + calcium Carbonate hard
8) Lime + Mg Carbonate Hardness
removed 9) So further addition of lime is required
precipitaes 10) finally excess lime is added
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Note:
ss could be removed by addition of Soda Ash (Na2CO3)
s CaCO3 which precipitaes and NaCl,Na2SO4 which dissolves and
nt contribute to hardness
e removed by addition of both Lime & Soda Ash (Na2CO3)
CaCO3 ,here MgCO3 is formed which is a soluble product and
dness along with this CaCl2 r CaSO4 .
gCO3 and forms Mg(OH)2 & CaCO3 a product that precipitaes .and
a soluble and non-hardness product, but contributes to TDS.