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Why are magnesium chloride and calcium chloride more soluble than sodium chloride?
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Mawerere Swaliki
Why are magnesium chloride and calcium chloride more soluble than sodium chloride?
$\ce{MgCl2}$ and $\ce{CaCl2}$ are more soluble than $\ce{NaCl}$ because In $\ce{MgCl2}$ and $\ce{CaCl2}$ the ionic charge is +2 hence it can interact with more number of $\ce{H2O}$ molecules, as the number of interactions increases more amount of energy is liberated which is a hydration energy which is sufficient enough to overcome the lattice energy of the compound.
Even solubility increases with increase in charge on ion.
$\ce{MgCl2}$ and $\ce{CaCl2}$ are more soluble than $\ce{NaCl}$ because In $\ce{MgCl2}$ and $\ce{CaCl2}$ the ionic charge is +2 hence it can interact with more number of $\ce{H2O}$ molecules, as the number of interactions increases more amount of energy is liberated which is a hydration energy which is sufficient enough to overcome the lattice energy of the compound.Even solubility increases with increase in charge on ion.
If only chemistry were so simple… A brief look at the More
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I don't think there is any simple answer.There are some rules of thumb, all of which have exceptions. Most chlorides are soluble. That includes both MgCl2 and CaCl2.
Solubility is the result of the balance between competing interactions: between the ions in the salt and between those ions and the water.
Many factors contribute to the solubility of a compound in water. In this case, the main difference between the compounds is the bonds’ strength.
The longer answer is to do with something called the "enthalpy of solvation".'
you can think it this way that the lattice enthalpy in MgCl2 and CaCl2 will be less and can be easily be overpowered by hydration enthalpy
I don't think there is any simple answer.There are some rules of thumb, all of which have exceptions. Most chlorides are soluble. That includes both MgCl2 and CaCl2.
Solubility is the result of the balance between competing interactions: between the ions in the salt and between those ions and the water.
Many factors contribute to the solubility of a compound in water. In this case, the main difference between the compounds is the bonds’ strength.
The longer answer is to do with something called the "enthalpy of solvation".'
you can think it this way that the lattice enthalpy in MgCl2 and CaCl2 will be less and can be easily be overpowered by hydration enthalpy
I am afraid solubility is one of the properties that cannot be properly explained yet. For example why is CaF2 absolutely insoluble ? By comparaison CaCl2, CaBr2 and CaI2 are all extremely soluble in water, as they can be dissolved in less than their weight of water.More
$\ce{MgCl2}$ and $\ce{CaCl2}$ are more soluble than $\ce{NaCl}$ because In $\ce{MgCl2}$ and $\ce{CaCl2}$ the ionic charge is +2 hence it can interact with more number of $\ce{H2O}$ molecules, as the number of interactions increases more amount of energy is liberated which is a hydration energy which is sufficient enough to overcome the lattice energy of the compound. Even solubility increases with increase in charge on ion.
$\ce{MgCl2}$ and $\ce{CaCl2}$ are more soluble than $\ce{NaCl}$ because In $\ce{MgCl2}$ and $\ce{CaCl2}$ the ionic charge is +2 hence it can interact with more number of $\ce{H2O}$ molecules, as the number of interactions increases more amount of energy is liberated which is a hydration energy which is sufficient enough to overcome the lattice energy of the compound.Even solubility increases with increase in charge on ion.
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I don't think there is any simple answer.There are some rules of thumb, all of which have exceptions. Most chlorides are soluble. That includes both MgCl2 and CaCl2.
Solubility is the result of the balance between competing interactions: between the ions in the salt and between those ions and the water.
Many factors contribute to the solubility of a compound in water. In this case, the main difference between the compounds is the bonds’ strength.
The longer answer is to do with something called the "enthalpy of solvation".'
you can think it this way that the lattice enthalpy in MgCl2 and CaCl2 will be less and can be easily be overpowered by hydration enthalpy
I don't think there is any simple answer.There are some rules of thumb, all of which have exceptions. Most chlorides are soluble. That includes both MgCl2 and CaCl2.
Solubility is the result of the balance between competing interactions: between the ions in the salt and between those ions and the water.
Many factors contribute to the solubility of a compound in water. In this case, the main difference between the compounds is the bonds’ strength.
The longer answer is to do with something called the "enthalpy of solvation".'
you can think it this way that the lattice enthalpy in MgCl2 and CaCl2 will be less and can be easily be overpowered by hydration enthalpy
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