Incorrect Question 3 0/ 0.5 pts Which statement best explains why the pH at the equivalence point of the titration of a strong acid with a strong base is 7.0 (at or near 25 °C)? A basic salt is formed, but it is neutralized by excess strong acid. All analyte has been consumed. An acidic salt is formed, but it is neutralized by excess strong base. There is no excess titrant. A neutral salt is the only chemical species present.

Incorrect Question 3 0/ 0.5 pts Which statement best explains why the pH at the equivalence point of the titration of a strong acid with a strong base is 7.0 (at or near 25 °C)? A basic salt is formed, but it is neutralized by excess strong acid. All analyte has been consumed. An acidic salt is formed, but it is neutralized by excess strong base. There is no excess titrant. A neutral salt is the only chemical species present.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The K of a certain indicator is 7× 107. The color of HIn is green and that of Inis red. A few drops of the indicator are added to an HC1 solution, which is then titrated against an NaOH solution. Over which pH range will the indicator change color? Select the single best answer. 7.2 to 9.2 ○ 4.2 to 6.2 O 6.2 to 8.2 O 5.2 to 7.2 O 3.2 to 5.2
Question 9 of 9 Šubmit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H,NNH, with 0.100 M HNO, after 10.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 x 10°. 1 2 NEXT> Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H,NNH,(aq) + H*(aq) H,NNH,"(aq) Before (mol) Change (mol) After (mol) CRESET 0.200 0.100 1.00 x 103 -1.00 x 103 2.00 x 103 -2.00 x 10* 6.00 x 103 -6.00 x 103 7.00 x 103 -7.00 x 103 8.00 x 103 -8.00 x 103
Consider the titration of 50.00 mL of a solution that is 0.0800 M oxalic acid. Calculate the pH after addition of 5.00 mL and 15.00 mL of 0.2000 M KOH (respectively). Find the value of salt and weak acid. Oxalic Acid Ka1 = 5.6 x 10-2 Oxalic Acid Ka2 = 5.4 x 10-5
Which of the following indicators would be most suitable for the titration of 0.10 M nitric acid and 0.10 M potassium hydroxide? bromothymol blue (pKIN = 7.1) methyl red (pKIN = 5.0) phenolphthalein (PKIN = 9.4) thymol blue (pKIN = 1.7) alizarin (pKIN = 11.7)
SOLVE STEP BY STEP DONT USE IA
Imagine you are working in the lab, and your labmate Jordan has challenged you to figure out which one of the following acetic acid/sodium acetate buffer solutions has the greatest buffering capacity at a pH above 4.74. pKa(acetic acid) = 4.74. Can you pick the solution with the highest buffering capacity at a pHabove 4.74? pKa(acetic acid) ? 0.36 M acetic acid and 0.12 M sodium acetate 0.16 M acetic acid and 0.12 M sodium acetate 0.36 M acetic acid and 0.22 M sodium acetate 0.16 M acetic acid and 0.22 M sodium acetate
11,The equivalence point of titrating of the weak base with the strong acid will be observed at Group of answer choices A, pH>7 B, pH<7 C, pH=pKb D, pH>pKb E, pH=7 12,The titration curve of titrating a diprotic acid with a strong base will have two distinct equivalence points Group of answer choices A, if Ka1<<Ka2 B, if Ka1=Ka2 C, always D, in case of ta strong acid E, if Ka1>>Ka2
Calculating the pH of a weak acid titrated with a strong base Try Again Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. 0/5 An analytical chemist is titrating 165.1 mL of a 1.100M solution of acetic acid (HCH3CO2) with a 1.200M solution of KOH. The pK of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 71.89 mL of the KOH solution to it. a Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. ? 00. 18 Ar pH ☑
If the pH at the 1/2 equivalence point is 4.19, what would be the Ka?