Why is it not practical to titrate an acid or base that is too weak or too dilute?

Short Answer

Expert verified

It is not feasible to titrate an acid or a base that is too weak because the inflection point, which is so close to the corresponding point, shrinks and becomes more difficult to detect.

Step by step solution

01

Define titration curve.

  • The plot of the pH of the analyte solution versus the volume of the titrant added as the titration advances is known as a titration curve.

  • Titration curves demonstrate how the pH of a solution varies when a known chemical is added to it, therefore each point along the curve offers you information on the pH of the solution as the volume of the known chemical grows.

02

Reason for not titrating an acid or a base that is too dilute.

  • Inflection point and equivalence points are the two points that are easy to identify in a titration curve.

  • Weak acids are rarely titrated against weak bases because the color shift caused by the indicator is generally rapid, making it difficult for the viewer to perceive the change.

  • The titration can be completed with just one drop, which is far too tiny to rely on.

  • As the concentration and/or intensity of the acid/base drop, it becomes more difficult to detect the end of the titration.

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Most popular questions from this chapter

Titration on Diprotic Systems

11-30. This problem deals with the amino acid cysteine, which we will abbreviate H2C.

(a) A 0.0300Msolution was prepared by dissolving dipotassium cysteine, in water. Then of this solution were titrated with 0.0600MHCIO4. Calculate the pHat the first equivalence point.

(b) Calculate the quotient [C2-]/[HC-] in a solution of cysteinium bromide (the saltH3C+Br-).

Consider the titration of 50.0mL of 0.0500M malonic acid with 0.100MNaOH. Calculate the pH at each point listed and sketch the titration curve:Vb=0.0,8.0,12.5,19.3,25.0,37.5,50.0and 56.3 mL.

Finding the End Point with Indicators 11 - 37. Why does a properly chosen indicator change color near the equivalence point in a titration?

Spectrophotometric properties of a particular indicator are given below:

A solution with a volume of 20.0 mL containing 1.40 ×10-5 M indicator plus 0.050 0 M benzene-1,2,3-tricarboxylic acid was treated with 20.0 mL of aqueous KOH. The resulting solution had an absorbance at 604 nm of 0.118 in a 1.00-cm cell. Calculate the molarity of the KOH solution.

Constant-boiling aqueous HCl can be used as a primary standard for acid-base titrations. When,20 wt% HCl (FM 36.461) is distilled, the composition of the distillate varies in a regular manner with the barometric pressure:

(a) Make a graph of the data in the table to find the weight percent of HCl collected at 746 Torr.

(b) What mass of distillate (weighed in air, using weights whose density is 8.0 g/mL) should be dissolved in 1.000 0 L to give 0.100 00 M HCl? The density of distillate over the whole range in the table is close to 1.096

g/mL. You will need this density to change the mass measured in vacuum to mass measured in air. See Section 2-3 for buoyancy corrections.

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