The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.400 moles of a monoprotic weak acid (K, = 4.0 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.400 moles of a monoprotic weak acid (K, = 4.0 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =

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 half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.580 moles of a monoprotic weak acid (K, = 2.5 x 10) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH about us careers privacy pollcy terms of use contact us help 10:23 P 3/12/202 ins t9 144
The half-equivalence point of a titration occurs halfway to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka-5.3x10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?
The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.280 moles of a monoprotic weak acid (Ka 4.8 x 10-) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
An undergraduate research student wishes to create a system that mimics human blood (pH = 7.4). The student chose as the model system to use a buffer solution of sodium dihydrogen phosphate (NaH2PO4, Ka = 6.2 × 10–8) and sodium hydrogen phosphate (Na2HPO4, Ka = 4.2 × 10-13). A) Which of the components of the buffer solution is the acid? B) Using the Henderson Hasselbalch equation, calculate the mole ratio of Na2HPO4/NaH2PO4 the student needs to use. C) To approximate the human condition of blood alkalosis (where the pH of blood rises to 7.6, which is usually lethal), how much base will the student need to add to the buffer?
Explain well with proper answer.
In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.31 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.98 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?
The curve for the titration of 25.0 mL of 0.100 M C5H5N(aq), pyridine, with 0.100 M HCI(aq) is given below. 12 10 8 4 2 5 10 15 20 25 30 35 Va(mL) (If the image above does not appear, click here.) Estimate the pH at the stoichiometric point. Your answer must contain only one decimal place. 8.8
The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.580 moles of a monoprotic weak acid (Ka = 2.5 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? PH =
The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka = 5.3 x 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?
I dont know how to do This question.
The pK, of hypochlorous acid is 7.530. A 59.0 mL solution of 0.134 M sodium hypochlorite (NaOCI) is titrated with 0.269 M HC1. Calculate the pH of the solution after the addition of 11.6 mL of 0.269 M HCI. pH = Calculate the pH of the solution after the addition of 30.7 mL of 0.269 M HCI. pH = Calculate the pH of the solution at the equivalence point with 0.269 M HCI. pH