
The of HCN is 9.3. The pH of a solution prepared by mixing 2.5 moles of HCN and 0.25 moles of KCN in water and making of the total volume to 500 ml is:
A. 9.3
B. 7.3
C. 10.3
D. 8.3
Answer
489.9k+ views
Hint: There is a formula to calculate the pH of the solution by using and it is as follows.
pH = pH of the solution
= acid ionization constant
[salt] = concentration of the salt
[acid] = concentration of the acid
Complete step by step solution:
- In the question it is given that 2.5 moles of HCN and 0.25 moles of KCN in water and made the solution to 500 ml by using water.
- We have to calculate the pH of the resulting solution.
- It is given that Acid ionization constant = 9.3
- Concentration of the salt (KCN) = 0.25 moles
- Concentration of the acid (HCN) = 2.5moles
- Substitute all the known values in the below formula to get the pH of the resulting solution.
pH = pH of the solution
= acid ionization constant = 9.3
[salt] = concentration of the salt = 0.25 moles
[acid] = concentration of the acid = 2.5 moles
- Therefore the pH of the resulting mixture is 8.3.
So, the correct option is D.
Note: (hydrocyanic acid) is a weak acid and (potassium cyanide) is salt. By mixing these two we will get an acidic buffer.
is going to be formed by the reaction of with and it is as follows.
pH = pH of the solution
[salt] = concentration of the salt
[acid] = concentration of the acid
Complete step by step solution:
- In the question it is given that 2.5 moles of HCN and 0.25 moles of KCN in water and made the solution to 500 ml by using water.
- We have to calculate the pH of the resulting solution.
- It is given that Acid ionization constant
- Concentration of the salt (KCN) = 0.25 moles
- Concentration of the acid (HCN) = 2.5moles
- Substitute all the known values in the below formula to get the pH of the resulting solution.
pH = pH of the solution
[salt] = concentration of the salt = 0.25 moles
[acid] = concentration of the acid = 2.5 moles
- Therefore the pH of the resulting mixture is 8.3.
So, the correct option is D.
Note:
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