The solubility product of $Ag _{2} CrO _{4}$ is $32 \times 10^{-12}$. What is the concentration of $CrO _{4}^{-}$ions in that solution?
- $2 \times 10^{-4} M$
- $16 \times 10^{-4} M$
- $8 \times 10^{-4} M$
- $8 \times 10^{-8} M$
The Correct Option is A
Approach Solution - 1
Approach Solution -2
The substance indicated is an inorganic salt called silver chromate, which has the molecular formula Ag2CrO4. When it dissolves, it can easily separate into silver and chromate ions. The silver ion is positively charged and is called a cation, while the chromate ion is negatively charged and is called an anion. The solubility product of silver chromate, which is called Ksp, has a value of 32×10-12.
We obtain the molecular formula of an inorganic salt, namely silver chromate with the formula Ag2CrO4. This salt is easily split into silver and chromate ions, where the silver ions are positively charged cations and the chromate ions are negatively charged anions. The solubility product of this salt is given as Ksp=32×10-12.
Dissociation of the salt produces two moles of silver ions and one mole of chromate ions, leading to the formation of the following equation Ag2CrO4 → 2Ag+ + CrO42-. Using this equation, the value of the solubility product can be determined: Ksp = (2s)2s = 4s3, where s is the solubility of the salt.
The value of s can be determined using the equation s = (Ksp1)1/3, substituting the value of Ksp into the equation. Thus, s = (32×10-121)1/3 = 2×10-4M. Thus, the concentration of the chromate ion CrO42- is 2×10-4M.
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Concepts Used:
Equilibrium
An equilibrium represents a state in a process when the observable properties such as color, temperature, pressure, concentration etc do not show any change.
The word equilibrium means ‘balance’ which indicates that a chemical reaction represents a balance between the reactants and products taking part in the reaction. The equilibrium state is also noticed in certain physical processes such as the melting point of ice at 0℃, both ice and water are present at equilibrium.
In the case of physical processes such as the melting of solid, dissolution of salt in water etc., the equilibrium is called physical equilibrium while the equilibrium associated with chemical reaction is known as chemical equilibrium.
Equilibrium in Chemical changes
The chemical equilibrium in a reversible reaction is the state at which both forward and backward reactions occur at the same speed.
The stage of the reversible reaction at which the concentration of the reactants and products do not change with time is called the equilibrium state.
Read More: Calculating Equilibrium Concentration
Types of Chemical Equilibrium
There are two types of chemical equilibrium:
- Homogeneous Equilibrium
- Heterogeneous Equilibrium
Homogenous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are all in the same phase. Homogenous equilibrium can be further divided into two types: Reactions in which the number of molecules of the products is equal to the number of molecules of the reactants. For example,
- H2 (g) + I2 (g) ⇌ 2HI (g)
- N2 (g) + O2 (g) ⇌ 2NO (g)
Reactions in which the number of molecules of the products is not equal to the total number of reactant molecules. For example,
- 2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
- COCl2 (g) ⇌ CO (g) + Cl2 (g)
Heterogeneous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are present in different phases. A few examples of heterogeneous equilibrium are listed below.
- CO2 (g) + C (s) ⇌ 2CO (g)
- CaCO3 (s) ⇌ CaO (s) + CO2 (g)
Thus, the different types of chemical equilibrium are based on the phase of the reactants and products.
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