How does KSP value affect solubility?
Ksp (Solubility product constant) is the equilibrium between a solid and its respective ions in a solution. The value of the constant identifies the degree of which the compound can dissociate in water. For example the higher the Ksp the more soluble the compound is.
How do you convert KSP to solubility?
Set up an ICE problem (Initial, Change, Equilibrium) in order to use the Ksp value to calculate the concentration of each of the ions. The concentration of the ions leads to the molar solubility of the compound. Use the molar mass to convert from molar solubility to solubility.
How does KSP compare to solubility?
The relative MOLAR solubility of salts (saturated solution) can be determined by comparing Ksp values. The greater the Ksp the more ions are in solution, hence the greater the molar solubility.
Is solubility product directly proportional to solubility?
A substance’s solubility product (Ksp) is the ratio of concentrations at equilibrium. Molar solubility, which is directly related to the solubility product, is the number of moles of the solute that can be dissolved per liter of solution before the solution becomes saturated.
How is Ksp calculated?
Let’s do an example: The solubility of Ag2CrO4 in water is 1.31 x 10-4 moles/L. Calculate the value of Ksp . Using mole ratios, the [Ag+] will go up by (2 x 1.31 x 10-4 moles/L) = 2.62 x 10-4 moles/L.
What 4 factors affect solubility?
Factors affecting solubility
- Temperature. Basically, solubility increases with temperature. …
- Polarity. In most cases solutes dissolve in solvents that have a similar polarity. …
- Pressure. Solid and liquid solutes. …
- Molecular size. …
- Stirring increases the speed of dissolving.
How do you solve solubility problems?
Solubility indicates the maximum amount of a substance that can be dissolved in a solvent at a given temperature. Such a solution is called saturated. Divide the mass of the compound by the mass of the solvent and then multiply by 100 g to calculate the solubility in g/100g .
How is solubility constant used?
To do this, simply use the concentration of the common ion as the initial concentration. Example: Estimate the solubility of barium sulfate in a 0.020 M sodium sulfate solution. The solubility product constant for barium sulfate is 1.1 x 10–10.
What is the solubility of Al OH 3 in the presence of 0.2 M NaOH?
The molar solubility of Al(OH)_(3) in 0.2 M NaOH solution is x xx 10^(-22)”mol/L”. Given that, solubility product of Al(OH)_(3)=2.4xx10^(-24).
What is the solubility of PbSO4 in 0.01 M Na2SO4?
The solubility of PbSO4 in 0.01M Na2SO4 solution is Ksp for PbSO4 = 1.25 × 10^-9 )
What will be the solubility of AgCl in 0.10 M NaCl?
What would be the solubility of silver chloride in 0.10 molar NaCl solution?( Ksp for AgCl solution = 1.20 × 10^-10 )