If you are titrating a sample of NaPH of unknown concentration with HCl and use 0.154 mol of HCl to get the equivalent point: How many mol of NaOH are in the sample?

In a particular titration experiment a 30.0 mL sample of an unknown monoprotic acid required 25.0 mL of 0.200 M NaOH for the end point to be reached. What is the concentration of the acid?

Consider a solution of a weak acid  being titrated with a solution of a strong base to beyond the equivalence point. Which of the following statements is incorrect?   a. The pH will increase intially and then change very little until the equivalence point is reached   b. Only a small percentage of the weak acid will react with the added base   c. The volume of the base solution required to reach the equivalence point can be less than, equal to, or more than the volume of the acid solution.   d. At the equivalence point, the solution will be basic   e. Beyond the equivalence point, the solution will be basic   f. None of the above   g. The pH of the solution in the tiration flask is affected by the total volume at any given point

Consider the titration of 25.00 mL of 0.100 M HCl with 0.050 M NaOH. At what volume of added NaOH is the solution a buffer solution?

It took 32.47 mL of 0.1424 M NaOH to reach the endpoint when titrating a sample containing 0.615g of unknown diprotic acid. What is the molar mass of this acid?

define the buffer capacity. a) buffer capacity is the amount of acid that can be added until all of the acid is used up b) buffer capacity is the amount of base that can be added until all of the base is used up c) buffer capacity is the amount of acid that can be added until all of the base is used up d) buffer capacity is the amount of acid ir base that can be added to a buffer without destroying its effectiveness e) buffer capacity is the amount of base that can be added until all of the acid is used up

At the equivalence point, all of the acid has been neutralized by the base. Why does the pH change so sharply around the equivalence point?

Use an example to discuss how a buffer solution resists changes in pH when small amounts of acid or base are added.

A 0.025M solution of hydrochloric acid is titrated with 0.020M of sodium hydroxide. If 250mL of the acid requires 30.0mL of the base for neutralization, calculate the initial concentration of hydrochloric acid.

It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form.  b) After the HCl was added, essentially all the indicator was in the HIn form.  Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.