Answer:
Explanation:
*Since the titration is between the strong acid HCl and the strong base Ca(OH)2, the pH at the equivalent point should be 7. On interpolation, we will obtain that 9.50mL and 9.82 mL of HCl is required to completely neutralized the given Ca(OH)2 solution.
*pH at the equivalence point =7
we know that pH + pOH = 14
Hence pOH= 14-7=7
pOH= -log(OH-)
The concentration of OH-= 10-pH= 1X10-7 M
One reason for the low solubility may be the higher reaction temperature, Another reason is the common ion effect.
The titration is between the strong acid HCl and the strong base Ca(OH)2, the pH at the equivalent point should be 7.
The process of determining the quantity of a substance A by adding measured increments of substance B, the titrant, with which it reacts until exact chemical equivalence is achieved (the equivalence point).
It is possible titrations are affected by temperature. The pH range for indicators can change with temperature. strong base
Since the titration is between the strong acid HCl and the strong base Ca(OH)2, the pH at the equivalent point should be 7.
On interpolation, we will obtain that 9.50mL and 9.82 mL of HCl is required to completely neutralized the given Ca(OH)2 solution.
*pH at the equivalence point =7
we know that pH + pOH = 14
Hence pOH= 14-7=7
pOH= -log(OH-)
The concentration of [tex]OH^-= 10^{-pH}= 1*10^{-7} M[/tex].
One reason for the low solubility may be the higher reaction temperature, Another reason is the common ion effect.
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