The molar concentration of the original HF solution : 0.342 M
Further explanation
Given
31.2 ml of 0.200 M NaOH
18.2 ml of HF
Required
The molar concentration of HF
Solution
Titration formula
M₁V₁n₁=M₂V₂n₂
n=acid/base valence (amount of H⁺/OH⁻, for NaOH and HF n =1)
Titrant = NaOH(1)
Titrate = HF(2)
Input the value :
Answer:
The pH of the solution is 2.56.
Explanation:
Given :
Concentration (c) = 0.40 M
Acid dissociation constant =
The equilibrium reaction for dissociation of (weak acid) is,
initially conc. c 0 0
At eqm.
Dissociation constant is given as:
By solving the terms, we get value of
No we have to calculate the concentration of hydronium ion or hydrogen ion.
Now we have to calculate the pH.
Therefore, the pH of the solution is, 2.56.