A chemistry student is studying the effect of buffers. During his experiment, he collected the following data. However, is advisor informed him that his conclusions were incorrect. What are the likely conclusions the student provided that led to his advisor telling him this? (Select all that apply) Moles of pH of pH of buffer pH of buffer 2 HCI added water 1 (0.10 M HA/ (0.20 М НА/ Select 2 correct answer(s) 0.10 MA) 0.20 MA) | Buffer 2 is more concentrated, so its capacity to resist to changes in pH is higher than Buffer 1. 7.00 4.74 4.74 10-6 6.00 4.74 4.74 Any concentration of HCl will decrease the pH of water, while high concentrations of HCl is needed to change the pH of a buffer. 10-5 5.00 4.74 4.74 10-4 4.00 4.74 4.74 O Buffer 1 is less concentrated, so its capacity to resist changes in pH is higher than Buffer 2. 10-3 3.00 4.74 4.74 10-2 2.00 4.66 4.70 Adding HCl will increase the pH of water, but not the pH of the buffers 10-1 1.00 2.72 4.27

A chemistry student is studying the effect of buffers. During his experiment, he collected the following data. However, is advisor informed him that his conclusions were incorrect. What are the likely conclusions the student provided that led to his advisor telling him this? (Select all that apply) Moles of pH of pH of buffer pH of buffer 2 HCI added water 1 (0.10 M HA/ (0.20 М НА/ Select 2 correct answer(s) 0.10 MA) 0.20 MA) | Buffer 2 is more concentrated, so its capacity to resist to changes in pH is higher than Buffer 1. 7.00 4.74 4.74 10-6 6.00 4.74 4.74 Any concentration of HCl will decrease the pH of water, while high concentrations of HCl is needed to change the pH of a buffer. 10-5 5.00 4.74 4.74 10-4 4.00 4.74 4.74 O Buffer 1 is less concentrated, so its capacity to resist changes in pH is higher than Buffer 2. 10-3 3.00 4.74 4.74 10-2 2.00 4.66 4.70 Adding HCl will increase the pH of water, but not the pH of the buffers 10-1 1.00 2.72 4.27

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 32QAP: Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate...

See similar textbooks

Similar questions

Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
A chemist needs a buffer with pH 3.50. How many milliliters of pure formic acid (density = 1.220 g/mL) must be added to 375 mL of 0.0857 M NaOH solution to obtain such a buffer?
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.