Does the acid-base titration seem a suitable method for determining a solubility
ID: 1047373 • Letter: D
Question
Does the acid-base titration seem a suitable method for determining a solubility product constant? Answer this question briefly commenting on the differences observed between your experimental average Ksp value and the theoretical one obtained from literature [ 8.0 x 10^(-6) ]
Does the acid-base titration seem a suitable method for determining a solubility product constant? Answer this question briefly commenting on the differences observed between your experimental average Ksp value and the theoretical one obtained from literature [ 8.0 x 10^(-6) ]
Explanation / Answer
Ksp is known as the the solubility product usually used to find out the equilibrium constant of sparingly soluble salt such as AgCl or NaCl
As we know that the salt NaCl is formed by the reaction between NaOH and HCl which are acid and Base. NaCl is sparingly soluble in water along with many salts like AgCl ,CaCl2 and AlCl3 etc.
The salt NaCl is electrolyte it's dissociation occurs in solution hence dissociates in Na+ and Cl- ion
So at equilibrium undissolved salt and it's ion exist in equilibrium. And we calculate the solubility product from there
Since acid Base titration forms the salt during the reaction salt starts precipitating out as titration is proceed and we can easily find the Ksp by calculating the concentration of the salt and reactant.
Like NaOH+HCl-----> NaCl + H2O
Here salt of NaCl is formed due to the titration of acid and Base and Ksp = K [NaCl]= [Na+][Cl-]
Hence by doing acid Base titration we can determine the Ksp of the salt
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