The pK, values for the dibasic base B are pKpi = 2.10 and pK2 = 7.62.%3D%3DCalculate the pH at each of the points in the titration of 50.0 mL of a 0.50 M B(aq) solution with 0.50M HCI(aq).What is the pH before addition of any HCI?pH =What is the pH after addition of 25.0 mL HC1?pH =What is the pH after addition of 50.0 mL HCI?pHWhat is the pH after addition of 75.0 mL HCI?pH =What is the pH after addition of 100,0 mL HCI?pH =

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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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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. 24.54 mL of 0.100M H2SO4(aq) is placed in a beaker. After 22.04 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution? Report your answer with 3 sig figs
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. 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.65 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?
When a 18.3 mL sample of a 0.460 M aqueous hydrocyanic acid solution is titrated with a 0.330 M aqueous barium hydroxide solution, (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 19.1 mL of barium hydroxide have been added?
in an acidbase titration, 10.0 mL (VB)of NH3 (Ka(NH+) = 5.8*10^ - 19) 0.18 M (CB) are titrated at the equivalence point (EP) with 10.0 ml (VA) of HCI 0.18 M (CA). Calculate (to two decimal places) the pH of the solution at the equivalence point.
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in mL, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 6.88. acid/base pairs to use: Ka pKa HCO2H/NaHCO2 1.8×10-4 3.74 H2CO3/NaHCO3 4.2×10-7 6.38 HBO3/NaH2BO3 7.3×10-10 9.14 NaHCO3/Na2CO3 4.8×10-11 10.32 HCO2H/NaHCO2 H2CO3/NaHCO3 H3BO3/NaH2BO3 NaHCO3/Na2CO3 ---------mL NaOH
Near the equivalence point in the titration of a strong acid with a strong base, one drop of base can cause the pH of the solution in the flask to change from 6.0 to 8.0. What is the relationship between the hydrogen ion concentrations at the two pH values? (A) The [H+] would be 100 times higher at pH 8.0 than 6.0. (B) The [H+] would be 200 times higher at pH 6.0 than 8.0. (C) The [H+] would be 2 times higher at pH 6.0 than 8.0. (D) The [H+] would be 2 times higher at pH 8.0 than 6.0. (E) The [H+] would be 100 times higher at pH 6.0 than 8.0.
A chemistry graduate student is given 250, ml, of a 1.30 M pyridine (C5H5N) solution, Pyridine is a weak base with Kg = 1.7 x10^-9. What mass of C5H5NHBr should the student dissolve in the C5H5N solution to turn it into a buffer with pH = 5.227 You may assume that the volume of the solution doesn't change when the C5H5NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.
A 400-mL buffer solution is 0.350 M in ammonia (NH3) and 0.350 M in ammonium chloride (NH4Cl).Kb(NH3)=1.76×10−5Part A:What is the initial pH of this solution? Express your answer using two decimal places.pH = 9.25 Part B:What is the pH after adding 125.0 mL of 0.100 M HBr to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 10.26) Part C:What is the pH after adding 150.0 mL of 0.100 M LiOH to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 8.33) --------------------------- Give the formula for tin(IV) hydroxide.
We have a titration for the titration of 50.0 mL of 0.425 M lactic acid, a monoprotic acid, (Ka = 1.38 x 10^-4) with 0.350 M NaOH. 1. Calculate the exact volume of the NaOH needed (to the correct numbers of sig figs) to reach the equivalence point. 2. Calculate the exact volume of NaOH needed (to the correct numbers of sig figs) to reach the mid point.
Consider the titration of a weak monoprotic acid with a strong base. The titration starts with 80mL of a weak acid solution with a concentration of 0.160 M. The Ka of the weak acid is 2.9*10^-8. The solution of the weak acid is titrated by adding a 0.290 M NaOH solution. (NaOH is a strong base) A. What is the pH of the solution after 15mL of the base is added?
5. You use a 0.1380 M HCI to standardize an NaOH solution. The burets below show initial and final volume readings for the titration to the perfect endpoint. Calculate the appropriate volume ratio (Va/Vb or Vb/Va ratio) and the [NaOH]. Acid Buret Reading (mL) initial final cumpasın INHI IN ||| Base Buret Reading (mL) initial final ייייייי |||||
A chemistry graduate student is given 100. mL of a 1.20M pyridine (CHN) solution. Pyridine is a weak base with K₁=1.7 × 10¯⁹. What mass of CH₂NHBr should the student dissolve in the CH₂N solution to turn it into a buffer with pH = 4.82? You may assume that the volume of the solution doesn't change when the C5H-NHBr is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 Ś

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