Magnesium bicarbonate → Calcium Carbonate

HRID 1753985

Reaction equation

HRID 1753985 reaction equation
[C:1](=[O:4])([OH:3])[O-:2].[Ca+2:5].[C:6](=[O:9])([OH:8])[O-:7].[Ca].[Mg:11].C(=O)(O)[O-].[Mg+2].C(=O)(O)[O-]>O>[C:1](=[O:2])([O-:4])[O-:3].[Ca+2:5].[C:6](=[O:7])([O-:9])[O-:8].[Mg+2:11]

Participants

7

Reactant 4

HCID 102204Magnesium bicarbonateHCID 5460341Calcium2×HCID 5462224MagnesiumHCID 10176262Calcium bicarbonate

Product 2

HCID 10112Calcium CarbonateHCID 11029Magnesium Carbonate

Reagents, catalysts & solvents 1

HCID 962WaterSolvent

Procedure

Mixing lime with the water will result in the lime preferentially reacting with carbon dioxide and bicarbonates to cause calcium carbonate to precipitate as calcium carbonate particles. This ordinarily occurs at a pH of approximately 10 to approximately 10.3. Once the carbon dioxide demand has been met, the lime is free to react with calcium bicarbonate, for example, which further results in the precipitation of calcium carbonate particles. Calcium bicarbonate is typically the most common calcium compound found in untreated water but other calcium-based hardness compounds have similar reactions. Magnesium compounds have a slightly different reaction. Generally, magnesium bicarbonate reacts with lime and produces calcium carbonate and magnesium carbonate. Then the magnesium carbonate reacts with lime and creates more calcium carbonate and magnesium hydroxide. Both of these compounds precipitate out of water.

Workup

  1. customa slightly different reaction

Sources & evidence

ORD record
ord-434a16b5a502449192df3f89547244f6
Source dataset
uspto-grants-2015_10
Patent number
US09169144B2

Linked notes

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