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Chapter 8: Q80E. (page 298)

Which of the indicators in Fig. 8.8 could be used for doing the titrations in Exercises 64 and 66?

Short Answer

Expert verified

Bromothymol blue or phenol red can be used as an indicator for exercise 64.

Bromocresol green can be used as the indicator for exercise 66.

Step by step solution

01

Definition of indicators in titration

A substance that changes color in response to a chemical change is defined as an indicator in the process of titration.

02

Explanation

When choosing an indicator for an acid-base reaction, it is best if the indicator color change occurs near the pH of the equivalence point of the reaction.

In exercise 64, the titration is between a strong base and a strong acid HCl.

The pH at the equivalence point of the strong acid strong base titration is 7.00.An indicator that changes its color near pH 7.00 should be chosen. Bromothymol blue (6.0-7.6) or phenol red (6.8-8.4) can be used as indicators.

In exercise 66, the titration is between a weak base, hydrazine, and strong acid . ThepH at the equivalence point is 4.82. Bromocresol green (3.8-5.4) can be used as the indicator for this titration.

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Most popular questions from this chapter

Question: Indicators can be used to estimate the pH values of solutions. To determine the pH of a 0.01 M weak acid solution, a few drops of three different indicators are added to separate portions of 0.01 M HX. The resulting colors of the HX solution are summarized in the last column of the accompanying table. What is the approximate pH of the 0.01M HX solution? What is the approximate $K_{a}$ value for HX

Calculate the pH of each of the following solutions.
a. 0.100 M propanoic acid (HC₃H₅0₂ K_a = 1.3 x 10^-5)
b. 0.100 M sodium propanoate (NaC₃H₅O₂)
c. pure H₂O
d. 0.100 M HC₃H₅O₂ and 0.100 M NaC₃H₅O₂

Carbonate buffers are important in regulating the pH of the blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0012 M, determine the bicarbonate ion concentration required to buffer the pH of blood atpH = 7.40.
$H_{2} C O_{3} (a q) ⇌ H C {O_{3}}^{-} (a q) + H^{+} (a q) K_{a} = 4.3 \times 10^{- 7}$

Question:Consider 100.0 mL of a 0.100 M solution of H₃A (K_a1 = 1.5 x 10^-4, K_a2 = 3.0 x 10^-8, K_a3 = 5.0 x 10^-12).
a. Calculate the pH of this solution.
b. Calculate the pH of the solution after 10.0 mL of1.00 M NaOH has been added to the original solution.
c. Calculate the pH of the solution after 25.0 mL of1.00 M NaOH has been added to the original solution.

Calculate the solubility of each of the following compounds in moles per liter and grams per liter. (Ignore anyacid-base properties.)
a. Ag₃PO₄, K_sp= 1.8 X 10^-18
b. CaCO₃, K_sp = 8.7 x 10^-9
c. Hg₂Cl₂, Kp = 1.1 x 10^-18
(Hg₂²⁺ is the cation in solution.)

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