Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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A buffer solution contains 0.351 M KHSO3 and 0.344 M K2SO3.If 0.0252 moles of hydroiodic acid are added to 225 mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume change does not change upon adding hydroiodic acid)pH =
Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate (NaHCO 3) is always 0.20 M, but the concentration of sodium carbonate (Na 2CO 3) corresponds to each of the following values: (a) 0.20 M; (b) 0.40 M; (c) 0.10 M.
A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L
solution of propanoic acid (HPr, K«= 1.3 x 105). Assume the volume of the solution to
be 1.0 L.
a) Write the chemical equation for the acid hydrolysis reaction.
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b) What is the acid-base conjugate pair that governs the pH of the buffer?
c) Calculate the pH of the buffer. Be sure to justify and validate any
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Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardA buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.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 buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?arrow_forwardYou want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?arrow_forwardA buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of ammonia (NH3). What will the solution pH be if 0.239 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K₁ of ammonia is 1.8 x 10-5. (Two decimal places)arrow_forward
- An aqueous solution contains 0.18 M ammonium chloride. One liter of this solution could be converted into a buffer by the addition of: (Assume that the volume remains constant as each substance is added.) O 0.04 mol Ba(OH)2 O 0.08 mol HCIO4 O 0.18 mol HClO4 O 0.17 mol BaCl2 O 0.17 mol NH3arrow_forwardAt 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate.A) If the solution is to be buffered at pH = 5, what should be the molar ratio of sodium acetate to acetic acid?B) If the buffer is found to be 1.55M in acetic acid and 1.70M in sodium acetate, what will be the pH of the solution?C) If 0.15 mol of NaOH was added to the solution in B, what will be the pH of the solution?D) If the pH of the solution in B is 4.50, how many moles of HCl was added to the solution?arrow_forwardA buffer solution contains 0.345 M NAHSO3 and 0.436 M Na,SO3. If 0.0273 moles of perchloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding perchloric acid) pH =arrow_forward
- What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution consisting of 0.162 M NH3 and 0.181 M NH4Cl? (Assume that there is no change in total volume when the two solutions mix.) pKa = 9.25arrow_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_forwardA buffer solution contains 0.420 M NaHCO3 and 0.262 M Na2CO3. If 0.0303 moles of potassium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution ?arrow_forward
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