Interactions | Reactions | Processes

Classified as: Dissolution: With Ionisation

Water dissolves ionic compounds by independently solvating the anions and cations. Ions are surrounded by a sphere of hydration.
[H3O]+
  +  
[BF4]–
         
HBF4(aq)
  +  
H2O

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NaCl
         
Na+
  +  
Cl–

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SO3
  +  
H2O
         
H2SO4(aq)

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SO3
  +  
H2SO4(aq)
         
H2SO4

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CuO
  +  
H2SO4(aq)
         
CuSO4
  +  
H2O

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HBr
  +  
CH3COOH
         
HBr in CH3COOH
30% W/W

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NH3
  +  
H2O
         
NH3(aq)

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CH3COOH
  +  
H2O
         
CH3COOH(aq)

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HCl
  +  
H2O
         
HCl(aq)

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H2S
  +  
H2O
         
H2S(aq)

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N2O4
         
[NO]+
  +  
[NO3]–

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SeO2
  +  
H2O
         
H2SeO3

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Na2[B4O5(OH)4]
.8H2O
  +  
5
H2O
         
2
H3BO3
  +  
2
[B(OH)4]–
  +  
2
Na+
  +  
8
H2O

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CuSO4.5H2O
  +  
KNa Tartrate
.4H2O
  +  
NaOH
  +  
H2O
         
Fehling's
Solution

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Cu
  +  
HOOH
  +  
2
HCl(conc)
         
Cu2+
  +  
2
Cl–
  +  
2
H2O

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[Al(H2O)6]3+
  +  
4
NaOH(aq)
         
[Al(OH)4]–
  +  
4
Na+
  +  
6
H2O

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Al(H2O)3(OH)3
Al(OH)3
  +  
NaOH(aq)
         
[Al(OH)4]–
  +  
Na+
  +  
3
H2O

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Al(H2O)3(OH)3
Al(OH)3
  +  
3
H+
         
[Al(H2O)6]3+

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Fe(H2O)4(OH)2
Fe(OH)2
  +  
2
H+
         

[Fe(H2O)6]2+

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Co(H2O)4(OH)2
Co(OH)2
  +  
2
H+
         

[Co(H2O)6]2+

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Cu(H2O)4(OH)2
Cu(OH)2
  +  
2
H+
         

[Cu(H2O)6]2+

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Fe(H2O)3(OH)3
Fe(OH)3
  +  
3
H+
         

[Fe(H2O)6]3+

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Cr(H2O)3(OH)3
Cr(OH)3
  +  
3
H+
         

[Cr(H2O)6]2+

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AgBr
  +  
2
  +  
hν
         
[Ag(S2O3)2]3–
  +  
Br–

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AgCl
  +  
2
NH3(aq)
         
[Ag(NH3)2]+
  +  
Cl–

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Al(OH)3
  +  
NaOH
         
[Al(OH)4]–
  +  
Na+

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2
Al(OH)3
  +  
3
H2SO4(aq)
         
Al2(SO4)3
  +  
6
H2O

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2
Al(OH)3
  +  
3
H2SO4(aq)
         
2
Al3+
  +  
3
[SO4]2–
  +  
6
H2O

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CuCl2
  +  
2
HCl(conc)
         

[CuCl4]2–
  +  
2
H+

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MgO
  +  
2
HNO3(aq)
         
Mg2+
  +  
2
[NO3]–
  +  
H2O

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MgO
  +  
2
H+
  +  
H2O
         
Mg2+
  +  
H2O

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SiO2
  +  
2
NaOH
  +  
H2O
         
Na2SiO3
solution
  +  
H2O

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SiO2
  +  
2
[OH]–
         
[SiO3]2–
  +  
H2O

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AgCl
  +  
HCl(conc)
         
[AgCl2]–
  +  
H+

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FeSO4.7H2O
  +  
H2O
         

[Fe(H2O)6]2+
  +  
[SO4]2–
  +  
H2O

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Mg(OH)2
  +  
H2O
         
Mg2+
  +  
2
[OH]–

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Ca(OH)2
  +  
H2O
         
Ca(OH)2(aq)

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Ca(OH)2
  +  
H2O
         
Ca2+
  +  
2
[OH]–

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Sr(OH)2
  +  
H2O
         
Sr2+
  +  
2
[OH]–

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Ba(OH)2
  +  
H2O
         
Ba2+
  +  
2
[OH]–

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Be(OH)2
  +  
2
H+
  +  
H2O
         
Be2+
  +  
2
H2O

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Be(OH)2
  +  
2
HCl(aq)
         
Be2+
  +  
2
Cl–
  +  
2
H2O

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Be(OH)2
  +  
2
[OH]–
  +  
H2O
         
[Be(OH)4]2–

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Be(OH)2
  +  
2
NaOH(aq)
         
2
Na+
  +  
[Be(OH)4]2–

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Mg(OH)2
  +  
2
H+
  +  
H2O
         
Mg2+
  +  
2
H2O

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Mg(OH)2
  +  
2
HCl(aq)
         
Mg2+
  +  
2
Cl–
  +  
2
H2O

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BaCl2
  +  
2
NaOH(aq)
  +  
H2O
         
Ba(OH)2
  +  
2
NaCl

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BeCl2
  +  
4
NaOH(aq)
  +  
H2O
         
[Be(OH)4]2–
  +  
4
Na+
  +  
2
Cl–

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BaCl2
  +  
2
NaOH(aq)
  +  
H2O
         
Ba2+
  +  
2
Na+
  +  
2
Cl–
  +  
2
[OH]–

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K2CO3
  +  
2
HCl(aq)
         
2
K+
  +  
2
Cl–
  +  
H2O
  +  
CO2

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AgF
  +  
H2O
         
Ag+
  +  
F–

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AgBr
  +  
2
.880 NH3
         
[Ag(NH3)2]+
  +  
Br–

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Al2O3.2H2O
(+Fe, Ti oxides)
         
Al2O3

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AgF
  +  
NH3(aq)
         
Ag+
  +  
F–
  +  
NH3(aq)

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AgBr
  +  
NH3(aq)
         
Ag+
  +  
Br–

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HCl
  +  
H2O
         
HCl(conc)

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Au
  +  
Aqua Regia
  +  
Cl–
         
[AuCl4]–
  +  
NO
  +  
2
H2O

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NaCl
  +  
H2O
         
Brine

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© Mark R. Leach 1999 –

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