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Chapter 11: Q50P (page 261)

Why is it more accurate to use a primary standard with a

high equivalent mass (the mass required to provide or consume 1

mol of H1) than one with a low equivalent mass?

Short Answer

Expert verified

When we weigh a high equivalent mass of a primary standard there is less chance of an error as opposed to a primary standard with a lower mass.

Step by step solution

01

Define Primary standard

The primary standard is a chemical substance used as a reference to determine the unknown concentration of a substance in a solution or any mixture. When we weigh a certain quantity of primary standard the weight of it correlates to the actual number of moles of the substance. The primary standard is supposed to agree with the following criteria -

  • Must be available with high purity
  • Must be stable under the conditions of proper storage.
  • It should have a higher molecular weight so as to minimize the effects caused by errors in weighing.
02

 Determine the primary standard with a high equivalent mass

A compound having high molar mass gives high equivalent weight. It is not tedious to be weighed. It can be weighed accurately and easily on a balance with minimal error since weighing such large samples minimizes the errors. Suppose that the weighing balance shows an error of 0.001 grams. Weighing 0.100 grams of the primary standard causes1%error. Instead, if we take a compound of high equivalent weight that provides more than 0.001 grams such as 1.000 grams the error will be minimized as0.1%

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Most popular questions from this chapter

Question:Titrating weak acid with weak base.

(a) Prepare a family of graphs for the titration of 50.0 mL of 0.020 0 M HA (pKa = 4.00) with 0.100 M B (pKb = 3.00, 6.00, and 9.00).

(b) Write the acid-base reaction that occurs when acetic acid and sodium benzoate (the salt of benzoic acid) are mixed, and find the equilibrium constant for the reaction. Find the pH of a solution prepared by mixing 212 mL of 0.200 M acetic acid with 325 mL of 0.050 0 M sodium benzoate.

In-1Spectrophotometry with indicators.* Acid-base indicators arc themselves acids or bases. Consider an indicator. HIn. which dissociates according to the equation

HIn鈬�KaH++In-

The molar absorptivity,. is role="math" localid="1654932356442" 2080M-1cm-1for HIn and 14200M-1cm-1for In-1. at a wavelength of 440 nm.

(a) Write an expression for the absorbance of a solution containing HIn at a concentration [HIn] and role="math" localid="1654932619574" In-1at a concentration role="math" localid="1654932655635" In-in a cell of pathlength 1.00 cm. The total absorbance is the sum of absorbances of each component.

(b) A solution containing indicator at a formal concentration of role="math" localid="1654931801074" 1.84脳104-Mis adjusted to pH 6.23and found to exhibit an absorbance of 0.868 at 440 nm. Calculate pKa for this indicator.

Sketch the general appearance of the curve for the titration of a weak base with a strong acid. What chemistry governs the pHin each of the four distinct regions of the curve?

11-19. Sketch the general appearance of the curve for the titration of a weak diprotic acid withNaOH. What chemistry governs the pHin each distinct region of the curve?

11-21. The baseNa+A-, whose anion is dibasic, was titrated withHCI to give curveb in Figures 11-4. Is the first equivalence point Hthe isoelectric point or the isoionic point?
See all solutions

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