Sketch a qualitative titration curve (pH vs. mL of base) for the complete titration of a diprotic weak acid with NaOH.

A diprotic acid is titrated with a strong base. The pH at the first half-equivalence point is (3.69x10^0). The pH at the second half-equivalence point is (8.9000x10^0). What is the value of ka2? Enter your answer using 3 significant figures.

a saturated solution of M(OH)2 is prepared. 15 ml of the saturated solution was titrated with a .055 M HCL solution. Examination of the pH titration curve indicated that it took 8.15 ml of the HCL solution to reach the equivalence point. What is the [OH-] in the saturated solution

What information can be obtained by examining the titration curve of a weak acid the concentration of the base solution O the initial pH of the acid O the identity of the salt formed by the neutralization reaciton O the heat of formation of the acid

In a titration experiment discuss how the indicator (Phenolphthalein) works and how it helps identify the end point/equivalence point?

A solution of weak base is titrated to the equivalence point with a strong acid. a Which one of the following statements is most likely to be correct? The pH of the solution is greater than 13.0. The pH of the solution at the equivalence point is 7.0. The pH of the solution is between 2.0 and 7.0. The pH of the solution is between 7.0 and 13.0. The pH of the solution is less than 2.0. D The reason that best supports the answer above is OBecause the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. Whenever a solution is titrated with a strong acid, the solution will be very acidic. Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidie

What does the pKIn of an acid-base indicator mean and how does it help in choosing an appropriate indicator for a certain titration ?