acid base titrations

question based on redox titration,acid base titration

acid base titration,iodometric titration

Which of the following are true for an acid- base titration?

The rapid change of pH near the stoichiometric point of an acid base titration is the basis of indicator detectio. pH of the solution is related to ratio of the concentrations of the conjugate acid (Hin) and base (In^(-)) forms of the indicator given by the expression

In an acid base titration, 0.1 M HCI solution was added to the NaOH solution of unknown strength. Which of the following correctly shows the change of pH of the titration mixture in this experiment?

In an acid base titration 50ml of 2N-NaOH solution is completely neutralised by 20ml of H_(2)SO_(4) . What is the molarity of sulphuric acid solution?

The following acid base titration graphs are given: (I) Which of the following graph represents titration of i. NH_(4)OH//HC1(W_(A)//S_(A)) ii. HNO_(3)//KOH(S_(A)//S_(B)) iii. C_(6)H_(5)COOH//KOH(W_(A)//S_(B))

Acidic solution is defined as a solution whose [H^(o+)] gt [overset(Theta)OH] . Base solution has [overset(Theta)OH] gt [H^(o+)] . During acid-base titrations, pH of the mixture will change depending on the amount base added. This variation is shown in the form of graph by making plot as titration curves 100mL of 1.0 M H_(3)A (K_(a_(1)) = 10^(-3), K_(a_(2)) = 10^(-5), K_(a_(3)) = 10^(-7)) is titrated against 0.1M NaOh . The titration curve is as follows. What would be the pH is more of NaH_(2)A is added to the titration mixture at point C ?