Equivalence point' in an acid base titration is defined as that point where equivalents of acid become equal to equivalents of base.In case of monoprotic acids and bases there is a single equivalence point, whereas in case of polyprotic acids and bases there may be multiple equivalnece points. Depending upon the type of suybstances present, pH of the soution can be calculated at nay equivalence point.
given that:
` Ka_(1),H_(3)PO_(4)=5xx10^(-4)`
`Ka_(2), H_(3)PO=5xx10^(-8)`
`Ka_(3),H_(3)PO_(4)=4.5xx10^(-11)
(Use: log 2 = 0.3, log 3 =0.4)`
What can be concluded abouyt the final soution obtained on mixing 200 ml of 0.2 `M H_(3)PO_(4)` with 50 ml of 0.3 M NaOH solution at 298 K?

Equivalence point' in an acid base titration is defined as that point where equivalents of acid become equal to equivalents of base.In case of monoprotic acids and bases there is a single equivalence point, whereas in case of polyprotic acids and bases there may be multiple equivalnece points. Depending upon the type of suybstances present, pH of the soution can be calculated at nay equivalence point. given that: Ka_(1),H_(3)PO_(4)=5xx10^(-4) Ka_(2), H_(3)PO=5xx10^(-8) Ka_(3),H_(3)PO_(4)=4.5xx10^(-11) (Use: log 2 = 0.3, log 3 =0.4) What can be concluded about nature of final solution obtained after mixing 50 ml of 0.1 M H_(3)PO_(4) with 0.1 M KOH at 298 K if volume of KOH solution added is less than or wequal to 50 mL?

Equivalence point' in an acid base titration is defined as that point where equivalents of acid become equal to equivalents of base.In case of monoprotic acids and bases there is a single equivalence point, whereas in case of polyprotic acids and bases there may be multiple equivalnece points. Depending upon the type of suybstances present, pH of the soution can be calculated at nay equivalence point. given that: Ka_(1),H_(3)PO_(4)=5xx10^(-4) Ka_(2), H_(3)PO=5xx10^(-8) Ka_(3),H_(3)PO_(4)=4.5xx10^(-11) (Use: log 2 = 0.3, log 3 =0.4) The pH of the solution when 100 ml of 0.1 M NaOH solution at 298 K Is:

When a strong acid is titrated using a weak base, the pH value at equivalence point is :

One gram equivalent of a weak acid is unable to completely neutralise one gram equivalent of a strong base.

A strong acid is titrated with weak base. At equivalence point, pH will be :

A strong acid is titrated with weak base. At equivalence point, pH will be :

In which of the following acid-base titration, the pH is greater than 8 at the equivalence point ?