Listen The pH of a solution of 0.04 M HCI is: 4 1.4 0.4 0.04 The pH cannot be determined Question 4 Listen In a titration of a weak acid by a strong base two equivalents of base are always needed to neutralize all the acid present the equivalence point cannot be defined exactly there is a region in which the pH changes slowly the equivalence point depends on the nature of the added base

Listen The pH of a solution of 0.04 M HCI is: 4 1.4 0.4 0.04 The pH cannot be determined Question 4 Listen In a titration of a weak acid by a strong base two equivalents of base are always needed to neutralize all the acid present the equivalence point cannot be defined exactly there is a region in which the pH changes slowly the equivalence point depends on the nature of the added base

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.84QE: Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink...

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Cacodylic acid, (CH3)2AsO2H, is a toxic compound that is a weak acid with pKa = 6.19. It is used to prepare buffered solutions. Calculate the masses of cacodylic acid and sodium cacodylate that should be used to prepare 500.0 mL of a pH = 6.60 buffer so that the buffer has a total of arsenic-containing species equal to 0.25 M, that is, so that: [(CH3)2AsO2H] + [(CH3)2AsO2] = 0.25 M
A particular buffer has been made up at 25 °C to give a pH of 8.00 and is then warmed to 35 °C. The pH of the solution changes because the pKa of the acid used to make the buffer has changed. What is the pH of the buffer solution at this new temperature if it is known that the pKa of the acid at 25 °C is 8.14 and ΔpKa/ ΔT = -0.018 °C-1?
1.Calculate the ratio of conjugate base to weak acid needed to make a buffer at pH 4.75 if the pKa of the acid is 5.32. 2.Calculate the pH of 0.055 M NH3 given Kb= 1.8x10^-5. 3.A solution at 25 °C that contains 1× 10-11 M OH− has what is the pH of the solution?
Calculate the pH of a buffered solution that is prepared by dissolving 0.3mol of NaHCO3 and 0.45mol of Na2CO3 in 1L of water at 298 K? (NaHCO3 pKa=10.27) 2. What change in pH would be obeserved upon the addition of 0.02 mol of HCl solution to (a) the buffered solution above and (b) 1L of pure water? (hint: which buffer component responds to the presence of the strong acid?)
Prepare 200.0ml of a 0.1M citrate buffer of pH 5.2 (pKa’s 3.128, 4.761, 6.396). What weight of each component is required? ( MW H3Cit=192, NaH2Cit=214 Na2HCit=236, Na3Cit=258)
The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.
what is the ph of a buffered sol'n having a 1:20 H2CO3 & HCO3- w/ 0.1 M concentration and dissociation constant of 7.9x10^-7. determine the pKa of the acid and ph of the buffer sol'n of a buffer mixed with 0.1 M tris and 0.5 M chloine salt having dissociation constant of 1.072x10^-6.
1: An unknown acid (0.596 g) was dissolved in approximately 50 mL of deionized water and titrated with a 0.250 M NaOH solution. When pH vs. Volume of NaOH (mL) added was plotted, the graph below was obtained. The unknown acid is: A) monoprotic B) diprotic C) triprotic 2: What is/are the pKa value(s) for this acid? A) 3.0 and 4.7 B) 4.0 and 7.7 C) 7.7 D) 4.0 E) 4.4 and 11.0 3: The volume of NaOH needed to reach the first equivalence point is: A) 30.0 mL B) 26.0 mL C) 15.0 mL D) 12.5 mL E) 19.5 mL 4: Calculate the number of moles of NaOH used to reach the first equivalence point. A) 0.00750 mol B) 0.00375 mol C) 0.00650 mol D) 0.00313 mol E) 0.00488 mol 5: The molar mass of the acid is: A) 86.9 g/mol B) 104 g/mol C) 66.8 g/mol D) 116 g/mol E) 159 g/mol
What is the lowest pH buffer that could effectively be made with a weak acid that has a pK a of 5.135? 6.135 8.135 3.135 7.135 4.135
A student needs to prepare a buffer solution with a pH of 4.80. Assuming a pKa of 4.73, how many mL of 0.1 M N a C2H3O2 would need to be added to 21.0 mL of 0.1 M HC2H3O2 to prepare this buffer?
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What amount of sodium formate must be added to a 1.00 L solution containing 1.28 moles of formic acid in order to make a buffer solution of pH = 4.10. The pKa of formic acid is 3.74.