Some automatic titrators measure the slope of a titration curve to determine the equivalence point. What happens to the slope that enables the instrument to recognize this point?

In order to determine the chloride concentration in a solution, a Mohr titration is perform. This involves adding a small amount of chromate to the solution and then slowly adding silver nitrate. Silver chloride is pale yellow solid while Silver chromate is a dark red. The appearance of the red silver chromate is the endpoint of the titration. Answer the questions below about this process. (Ksp of AgCl= 1.7x10^-10 and Ksp of Ag2CrO4= 1.12x10^-12) A 100 mL sample of water from a potentially contaminated stream is collected. A 0.0010 g of sodium chromate is dissolved in the sample. 1) if the solution had been 0.015 M in NaCl, what percent of the chloride is still in solution?  Given the answer to the question above, it should be clear that "all" of the chloride is removed before the silver chromate appears. This is why we can use it as an endpoint. 2) if it requires 21.4 mL of a 0.1 M solution of silver nitrate to reach the equivalence point with 100 mL of solution, what was the original…

A pH change of 0.2 units requires the addition of 1.50 mL of NaOH. You are probably at what point in the titration?     either before or after the equivalence point     very close to equivalence point     before equivalence point     after equivalence point

Explain the difference between an indicator endpoint for a titration analysis and the true equivalence point for the titration. Please simplify the answer so I can understand. Thanks

In an acid-base titration, a base or acid is gradually added to the other until they have completely neutralized each other. Since acids and bases are usually colorless (as are the water and salt produced in the neutralization reaction), pH is measured to monitor the reaction. Suppose that the equivalence point is reached after approximately 393 mL of a NaOH solution has been added (enough to react with all the acetic acid present) but that replicates are equally likely to indicate from 373 to 417 mL (exclusive), measured to the nearest mL. Assume that two technicians each conduct titrations independently. What is the probability that the average volume at equivalence from the technicians is 416 mL or 417? Select one: O a. 0.79069767 b. 0.00000000 c. 0.00054083 d. 1.00000000 e. 0.00049383 f. 0.02941176 O g. 0.04651163 O O

Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 pH 7 6 alizarin yellow R 5 O quinaldine red 4 3 O clayton yellow 2 1 metacresol purple 4 6 8 10 12 14 16 18 20 Volume of Titrant (mL) O methyl green 2.

Write the equation for the equilibirum that determines the pH at the following points in the titration curve of a weak acid (HA) being titrated with a strong base (OH) before any base has been added halfway to the equivalence point at the equivalence point

Use the following two titration curves to answer each of the following statements. Select the choice that completes the statement correctly. 14 pH 7 0 Graph A 25 volume of titrant added (mL) In graph A, the end point occurs at a In graph B, the equivalence point occurs at a + 141 pH 7 0 Graph B 25 volume of titrant added (mL)

3. Explain the weak acid/strong base titration curve Weak Acid/Strong Base Titration Curve 12 10 6 8 12 16 20 24 28 32 36 Volume Base Added (mL) Hd

The pH at the equivalence point of a strong acid-strong base titration cannot be determinined without more information is basic is acidic is exactly 7.00