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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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 0.160 M NH3 and 0.182 M NH4Cl? (Assume that there is no change in total volume when the two solutions mix.)
pKa = 9.25
You are required to prepare a buffer (pH
sodium propionate. The concentration of the propionate
must the concentration of the acid be? K, = 1.3 × 105
5.30) using propionic acid and
0.6M. Which one
A buffer contains 0.035 mol of boric acid (pKa = 9.15) and 0.015 mol of sodium borate per liter.
(a) Calculate the pH of the buffer.(b) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of the buffer.(c) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of pure water.
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_forward(a) Calculate the pH of a solution that is 0.50 M acetic acid and 0.91 M sodium acetate. (b) How would you prepare 250.0 mL of this buffer solution if you have a stock solution of 3.0 M acetic acid and another stock solution of 1.5 M sodium acetate?arrow_forward1. A buffer is formed by mixing 65.0 mL of 0.82 M acetic acid (CH3CO2H) with 80.0 mL of 0.64 M sodium acetate (CH3CO2Na). (a) What is the pH of the solution? Assuming no change in volume, determine the pH of the buffer after (b) addition of 0.0050 mols NaOH; (c) addition of 0.0050 mols HCl. (Kp of NH3 = 1.8 x 10-5) а. b. с. 2 A 22 0O ml samnle of o 0 240 M HCI 0200 VK Oarrow_forward
- 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 =arrow_forwardWhat are the molar concentrations of acetic acid (CH, COOH) and sodium acetate (CH,COONA) in an aqueous solution buffered at a pH of 4.04 that has a freezing point of –3.45 °C? Assume complete dissociation of sodium acetate and a density of 1.02 g/mL for the solution. The pKa for CH,COOH is 4.75. [CH, COOH] = M [CH,COONA] Marrow_forwardA buffer solution contains 0.486 M hydrocyanic acid and 0.298 M potassium cyanide (K₂ (HCN) If 0.0309 moles of sodium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume does not change upon adding sodium hydroxide) pH = = 4.00 × 10-¹0).arrow_forward
- What is the pH change when 28.8 mL of 0.0540 M NaOH is added to 70.1 mL of a buffer solution consisting of 0.147 M NH3 and 0.183 M NH4C1? (K, for ammonium ion is 5.6 x 10-10. pH change =|arrow_forwardA buffer solution contains 0.405 M NaHSO3 and 0.332 M Na,SO3. If 0.0248 moles of potassium hydroxide are added to 150. mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide) pH =arrow_forwardA 35.00-mL solution of 0.2500 M HF is titrated with a standardized 0.1762 M solution of NaOH at 25 °C. (a) What is the pH of the HF solution before titrant is added? (b) How many milliliters of titrant are required to reach the equivalence point? mL (c) What is the pH at 0.50 mL before the equivalence point? (d) What is the pH at the equivalence point? (e) What is the pH at 0.50 mL after the equivalence point?arrow_forward
- When a 18.6 mL sample of a 0.490 M aqueous hydrofluoric acid solution is titrated with a 0.336 M aqueous potassium 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 40.7 mL of potassium hydroxide have been added?arrow_forwardA buffer is prepared by adding 5.0 g of ammonia, NH3, and 20.0 g of ammonium chloride, NH4Cl, to enough water to form 2.50 L of solution. (a) What is the pH of the buffer? (b) Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. (c) Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.arrow_forwardA buffer solution contains 0.476 M ammonium bromide and 0.339 M ammonia. If 0.0340 moles of potassium hydroxide are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding potassium hydroxide) pHarrow_forward
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