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An ionic compound is more soluble than a covalently bonded compound.
Intensive, as solubility is a chemical property having to do with whether a compound is ionic, covalent-polar, or covalent non-polar.
Lower solubility of an ionic compound, and an increased amount of precipitate formed
Precipitation titrations are based upon reactions that yield ionic compounds of limited solubility.
The ionic character increases for group 2 compounds as we go down the group. The metallic character also increases.
Ammonium sulfate precipitation is a method used to purify proteins by altering their solubility. It is a specific case of a more general technique known as salting out.Ammonium sulfate is commonly used as its solubility is so high that salt solutions with high ionic strength are allowed.The solubility of proteins varies according to the ionic strength of the solution, and hence according to the salt concentration. Two distinct effects are observed: at low salt concentrations, the solubility of the protein increases with increasing salt concentration (i.e. increasing ionic strength), an effect termed salting in. As the salt concentration (ionic strength) is increased further, the solubility of the protein begins to decrease. At sufficiently high ionic strength, the protein will be almost completely precipitated from the solution (salting out).
It increases.
Temperature is proportional to solubility for sodium bicarbonate in water. Generally, adding heat increases solubility, as this input of energy helps break bonds.
ionic product IP = [H2+]2[SO42-] SOLUBILITY PRODUCT = IP (mol3dm-9)
Solubility of covalent bonds is usually high to low. Solubility for Ionic compounds is usually high.
The volume solution in conical flask is very important in solubility ionic salt water. This is because it determines its solubility.
Since calcium chloride is an ionic salt, it becomes less soluble as the temperature lowers.
SSC buffer increases ionic strength so precipitation of DNA or RNA is increases.CHARUSAT UNIVERSITY.
Solubility is the ability of an ionic compound t dissociate in a solution.
True
solubility of an ionic compound decreases in the presence of a common ion. A common ion in the solution, that is common to the ionic compound being dissolved. for example the silver ion in silver nitrate solution is common to the silver in silver chloride. the presence of a common ion must be taken into accounts when determining the solubility of an ionic compounds.
Electrical conductivity, water solubility, crystalline structure