9a.Phosphoric acid, H3PO4, is a trivalent acid with pKs1 = 2.12, pKs2 = 7.21, and pK $3 =12.37. Calculate how many milliliters of 1.50 M HCI should be added to 300 mL of 0.400 MNa₂HPO4 to obtain a buffer solution with pH = 6.85.9b.To the resulting buffer solution in question 9a, 16.0 mL of 0.500 M NaOH is added. Calculate thepH of the solution after this addition.9c.When ammonium hydrogen phosphate, (NH4)2HPO4, dissolves in water, the followingequilibrium is established:NH +HPO +NH3+H,POK = 10-2.04Based on the above equilibrium, calculate the concentrations of HPO and H₂PО in a 0.100M solution of (NH4)2HPO4.9d.Calculate the pH of the solution in question 9c.I

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Answered: 9a. Phosphoric acid, H3PO4, is a…

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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An analytical chemist is titrating 74.4 mL of a 0.3100 M solution of butanoic acid (HC,H,CO,) with a 0.3400 M solution of KOH, The p K_ of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 72.3 mL of the KOH solution to it. 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. do pH = 0 Pvacy Accessibilty Check 2021 McGraw-Hill Education All Rights Reserved Terms of Use Explanation V 11:16
A buffer solution is made that is 0.452 M in HC10 and 0.452 M in KC10. If K, for HC10 is 3.50 x 10-8, what is the pH of the buffer solution? pH : Write the net ionic equation for the reaction that occurs when 0.100 mol KOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.) +
4. A solution prepared to be initially 1 M in NH3 and 0.5 M in HCl is (Kb for NH3 = 1.8 x 10¯5): (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7
Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 145 mL of a buffer that is 0.300 M in both acetic acid (CH₂COOH) and its conjugate base (CH3COO-). Calculate the maximum volume of 0.170M HCl that can be added to the buffer before its buffering capacity is lost. volume: esc ! 1 ← 2 #3 с $ 4 G Search or type URL 27 20 % MacBook Pro 5 ^ 6 & 7 +00 8 ( 9 ) mL 0 1
The buffer was made by combining 0.220 M lactic acid (HC3H5O3) and 0.200 M sodium lactate ( NaC3H5O3). The Ka of HC3H5O3 is 1.4 x 10^-4. 1. write the equation describing the conjugate acid base relationship 2. Calculate the pH of the buffer 3. Calculate the pH of the buffer after the addition of 100.0 mL of 0.100 M potassium hydroxide to 0.9000 L of the buffer solution
Consider the reaction of a 20.0 mL of 0.220 M C;H;NHCI (Ka = 5.9 x 10) with 12.0 mL of 0.239 M CSOH. Write the net ionic equation for the reaction that takes place. What quantity in moles of C;H;NH" would be present at the start of the titration? What quantity in moles of OH" would be present if 12.0 mL of OH were added? -What species would be left in the beaker after the reaction goes to completion? d. What quantity in moles of C,H,NH would be left in the beaker after the reaction goes to completion?
A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 5.72) with 20.00 mL of 0.100 M NaOH. This buffer is then divided into 4 equal 15.00 mL parts. If 0.12 mL of a 1.0 M solution of hydrochloric acid is added to one of these 15.00 mL portions of the buffer, what is the pH of the resulting solution?
A buffer solution is made that is 0.432 M in H₂CO, and 0.432 M in KHCO3. If Kal for H₂CO, is 4.20 x 10-7, what is the pH of the buffer solution? PH = for this question. Write the net ionic equation for the reaction that occurs when 0.093 mol HBr is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H₂O instead of H*)
b A chemistry graduate student is given 300. mL of a 1.20M pyridine (CHN) solution. Pyridine is a weak base with K₂= 1.7 × 10 What mass of CH₂NHCl should the student dissolve in the C-H₂N solution to turn it into a buffer with pH = 5.20? You may assume that the volume of the solution doesn't change when the C5H₂NHCl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 I 5
A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 5.09) with 20.00 mL of 0.100 M NaOH. This buffer is then divided into 4 equal 15.00 mL parts. If 0.23 mL of a 10 M solution of sodium hydroxide is added to one of these 15.00 mL portions of the buffer, what is the pH of the resulting solution?
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0 The pK, values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.67. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.60 M B(aq) solution with 0.60 M HCl(aq). What is the pH before addition of any HCI? What is the pH after addition of 25.0 mL HC1? What is the pH after addition of 50.0 mL HC1? What is the pH after addition of 75.0 mL HC1? What is the pH after addition of 100.0 mL HC1? pH = pH pH = pH = pH = 12.76 11.9 9.2 6.33 1.4 Incorrect

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