In acid-base titration one of the following is incorrect: A suitable indicator should have pH of color transition of pH = pka±1. O The equivalence point will be sharp when the both acid and base are weak. The end point will be sharper when more concentrated solutions are used. The end point will be sharper if the reaction is completed. If the equivalence point doesn't match with the end point the titration error will be high.

In acid-base titration one of the following is incorrect: A suitable indicator should have pH of color transition of pH = pka±1. O The equivalence point will be sharp when the both acid and base are weak. The end point will be sharper when more concentrated solutions are used. The end point will be sharper if the reaction is completed. If the equivalence point doesn't match with the end point the titration error will be high.

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...

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6
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HA+KOH → NaA + H₂O Nia titrates half of a weak acid solution with KOH until she observes the endpoint. She measures the pH of the half-titrated weak acid solution as 1.23. What is the Ka for the acid? K₂ = [? ] × 10¹²] a Coefficient (green) Exponent (yellow) Enter
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In acid-base titration one of the following is incorrect: The equivalence point will be sharp when the both acid and base are strong. A suitable indicator should have pH of color transition of pH = pKa±l. O The end point will be sharper when more diluted solutions are used. The end point will be sharper if the reaction is completed. If the equivalence point doesn't match with the end point the titroation error will be high.
Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.8 × 10-13). To find the pH of a buffer composed of H, PO, (aq) and HPO (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 pK22 = 7.21 O pKa3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 10.0 g of KH, PO,(s) and 25.0 g of Na, HPO,(s) in water and then diluting to 1.00 L. pH = II
If the pH at the 1/2 equivalence point is 4.19, what would be the Ka?