Concept explainers
A sample of 0.220 M triethylamine, (CH3CH2)3 N, is titrated with 0.544 M HCl.
(a) Write a balanced net ionic equation for the titration.
(b) How many milliliters of HCl are required to reach the equivalence point?
(c) Calculate [(CH3CH2)3N], [(CH3CH2)3NH+], [H+], and [Cl-] at the equivalence point. (Assume that volumes are additive.)
(d) What is the pH at the equivalence point?
Trending nowThis is a popular solution!
Chapter 14 Solutions
Chemistry: Principles and Reactions
- Calculate the mass of sodium acetate, NaCH3COO, you should add to 500. mL of a 0.150-M solution of acetic acid, CH3COOH, to buffer a solution at a pH of 4.57.arrow_forwardKa for formic acid is 1.7 104 at 25C. A buffer is made by mixing 529 mL of 0.465 M formic acid, HCHO2, and 494 mL of 0.524 M sodium formate, NaCHO2. Calculate the pH of this solution at 25C after 110 mL of 0.152 M HCl has been added to this buffer.arrow_forward(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after the addition of 0.030 mol HCl? note: Ka (NH4+) = 5.6 x 10 -10 NH3 (aq) + H+ (aq) → NH4+ (aq) (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.arrow_forward
- Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.arrow_forwardDuring a titration, 10.0 ml of 0.135 M NaOH is added to 25.0 ml of 0.123 M CH3COOH. What is the pH at this point in the titration? ka for CH3COOH is 1.8x10^-5 at 25 C.arrow_forwardA chemist titrates 20.00 mL of 0.2000 M HBrO (Ka = 2.3x10-9) with 0.1000 M NaOH. What is the pH: (a) before any base is added? (b) when [HBrO] = [BrO2]? (c) at the equivalence point?(d) when the amount (mol) of OH2 added is twice the amount of HBrO present initially?arrow_forward
- (a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of ha IS 5.66 X 10-7. Express the pH numericall to three decimal places (b) What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Express the pH numerically to three decimal places. (c) What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base. Express the pH numerically to three decimal placesarrow_forwardFor the titration of 25.00 mL of 0.100M CH CO,H with 0.100 M NAOH. The reaction can be represented as: CH,CO,H + OH- → CH,CO, + H,0 (a) What is the initial pH before any amount of the NaOH solution has been added?K: 1.8 x 10 for CH,CO,H. (b) Find the pH after 12.50 mL of the NaOH solution have been added. (c) Find the pH after 25.00 mL of the NAOH solution has been added. (d) Find the pH after 3750 mL of the NaOH solution has beern added.arrow_forwardCalculate the pH at the following points in a titration of 40. mL (0.040 L) of 0.145 M 4-chlorobenzoic acid (Ka = 1.0 ✕ 10−4) with 0.145 M KOH. (Assume Kw = 1.01 ✕ 10−14.) (a no KOH added???? (b)20. mL of KOH solution added???? (c)39 mL of KOH solution added???? (d)40. mL of KOH solution added???? (e)41 mL of KOH solution added????arrow_forward
- A buffer contains 0.010 mol of lactic acid (pKa = 3.86) and 0.050 mol of sodium lactate per liter. (a) Calculate the pH of the buffer. (b) Calculate thechange in pH when 5 mL of 0.5 M HCl is added to 1 L of the buffer. (c) What pH change would you expect if you added the same quantity of HCl to 1 L of pure water?arrow_forwardConsider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d pleasearrow_forwardA buffer is prepared by adding 10.0 g of ammonium chloride(NH4Cl) to 250 mL of 1.00 M NH3 solution. (a) Whatis the pH of this buffer? (b) Write the complete ionic equationfor the reaction that occurs when a few drops of nitricacid are added to the buffer. (c) Write the complete ionicequation for the reaction that occurs when a few drops ofpotassium hydroxide solution are added to the buffer.arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning