Concepts and reason
The solubility product for the reaction is equilibrium constant, where the solid ionic compound dissociates into its ions in a solution. The solubility product is denoted as Ksp. The solubility product value relates to the saturated solution and indicates the precipitate level of the compound. The formation precipitation starts when the ionic product exceeds the solubility product.
Fundamentals
The solubility product value of the compound depends on the concentrations of its ions in a solution. Example: AB is a solid ionic compound. Precipitation: If the solubility product value is lesser than the concentration of the ions present in the solution, the compound precipitates in the solution.
The given solid ionic compound is Ag2SO4 The equilibrium equation for the ionic compound is given below:
Therefore, the solubility product of the ionic compound is
Ksp=[Ag+]2[SO42−]=1.2×10−5
The equilibrium equation has been written for the given solid ionic compound (Ag2SO4), and the solubility product has been derived from the equilibrium equation.
The balanced equation for the reaction of AgNO3 and Na2SO4 :
The initial concentration of [Ag+] ions in AgNO3 is given below:
[Ag+]initial =1molAgNO35.0 mL× mL0.20mmolAgNO3×150.0+5.0)mL1molAg+=0.00645M
The initial concentration of [SO42−] ions in Na2SO4 is given below:
[SO42−]initial =(150.0+5.0)mL150.0 mL× mL0.10mmolNa2SO4×1molNa2SO41 molSO42−=0.0968M
The ionic product of Ag2SO3 is given below:
KIP==[Ag+]initial 2[SO42−]initial (0.00645)2(0.0968)=4.0×10−6
The ionic product (KIP) is less than the solubility product (Ksp), KIP<Ksp⇒ precipitation does not takes place.
For the mixture, 150.0mLof0.10MNa2SO4 (aq) and 5.0mL of 0.20M AgNO 3 (aq) precipitation does not take place.
The balanced equation for the reaction of AgNO3 and Na2SO4 is given in which the two moles of AgNO3 react with one mole of Na2SO4 to produce the Ag2SO4 precipitate. The concentration of silver ions [Ag+] and sulphate ions [SO42−] has been calculated to find the ionic product. The value of ionic product is less than that of the solubility product for which the precipitation does not takes place.
The balanced equation for the reaction of AgNO3 and Na2SO4 :
The initial concentration of [Ag+] ions in AgNO3 is given below:
[Ag+]initial =(150.0+5.0)mL5.0 mL× mL0.30mmolAgNO3×1molAg+31 molAgrO3=0.00968M
The initial concentration of [SO42−] ions in Na2SO4 is given below:
[SO42−]initial =(150.0+5.0)mL150.0 mL× mL0.10mmolNa2SO4×1 molSO42−41molNa2SO4=0.0968M
The ionic product of Ag2SO3 is given below:
KIP==[Ag+]initial 2[SO42−]initial (0.00968)2(0.0968)=9.1×10−6
The ionic product (KIP) is less than the solubility product (Ksp), KIP<Ksp⇒ precipitationdoesnottakesplace
For the mixture, 150.0mLof0.10MNa2SO4 (aq) and 5.0mL of 0.30M AgNO 3 (aq) precipitation does not take place.
The concentration of silver ions [Ag+] and sulphate ions [SO42−] has been calculated to find the ionic product. The ionic product's value is less than that of the solubility product for which precipitation does not occur.
The balanced equation for the reaction of AgNO3 and Na2SO4 :
The initial concentration of [Ag+] ions in AgNO3 is given below:
[Ag+]initial =(150.0+5.0)mL5.0 mL× mL0.40mmolAgNO3×150.0+5.0)mL1 molAg+molAgNO3=0.0129M
The initial concentration of [SO42−] ions in Na2SO4 is given below:
[SO42−]initial =(150.0+5.0)mL150.0 mL× mL0.10mmolNa2SO4×1 molSO42−41molNa2SO4=0.0968M
The ionic product of Ag2SO3 is given below:
KIP==[Ag+]initial 2[SO42−]initial (0.0129)2(0.0968)=1.6×10−5
The ionic product (KIP) is greater than the solubility product (Ksp), KIP>Ksp⇒ precipitationtakesplace
For the mixture, 150.0mLof0.10MNa2SO4 (aq) and 5.0mL of 0.40M AgNO 3 (aq) precipitation takes place.
The concentration of silver ions [Ag+] and sulphate ions [SO42−] has been calculated to find the ionic product. The value of ionic product is greater than that of the solubility product; therefore, the precipitation does take place.
The balanced equation for the reaction of AgNO3 and Na2SO4 :
The initial concentration of [Ag+] ions in AgNO3 is given below:
The initial concentration of [SO42−] ions in Na2SO4 is given below:
[SO42−]initial =(150.0+5.0)mL150.0 mL× mL0.10mmolNa2SO4×1molNa2SO41 molSO42−=0.0968M
The ionic product of Ag2SO3 is given below:
KIP==[Ag+]initial 2[SO42−]initial (0.0161)2(0.0968)=2.5×10−5
The ionic product (KIP) is greater than the solubility product (Ksp), KIP>Ksp⇒ precipitationtakesplace
For the mixture, 150.0 mL of 0.10MNa2SO4 (aq) and 5.0mL of 0.50M AgNO 3 (aq) precipitation takes place.
The balanced equation for the reaction of AgNO3 and Na2SO4 is given in which the two moles of AgNO3 react with one mole of Na2SO4 to produce the Ag2SO4 precipitate. The concentration of silver ions [Ag+] and sulphate ions [SO42−] has been calculated to find the ionic product. The value of ionic product is greater than that of the solubility product for which the precipitation does take place.