A buffer solution contains 0.50 mol of hydrazoic acid (HN3) and 0.62 mol of sodium hydrazoate (NaN3) in 7.00 L. The K, of hydrazoic acid (HN3) is K₂ = 1.9e-05. (a) What is the pH of this buffer? pH = 5.96 (b) What is the pH of the buffer after the addition of 0.35 mol of NaOH? (assume no volume change) pH = 5.86 pH x (c) What is the pH of the original buffer after the addition of 0.35 mol of HI? (assume no volume change) = x x

A buffer solution contains 0.50 mol of hydrazoic acid (HN3) and 0.62 mol of sodium hydrazoate (NaN3) in 7.00 L. The K, of hydrazoic acid (HN3) is K₂ = 1.9e-05. (a) What is the pH of this buffer? pH = 5.96 (b) What is the pH of the buffer after the addition of 0.35 mol of NaOH? (assume no volume change) pH = 5.86 pH x (c) What is the pH of the original buffer after the addition of 0.35 mol of HI? (assume no volume change) = x x

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 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) pH
The mixture of 100.0 mL of 0.100 M NaOH (aq) and 100.0 mL of 0.300 M CH3COOH (aq) will result in a buffer. (a) Explain why the resulting solution is a buffer. (b) What is the pH of this buffer?
A buffer solution contains 0.444 M NaHSO3 and 0.246 M K,SO3. If 0.0239 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 =
Q1 (a) How solubility and solubility products relate to each other? (b) The PH of a solution is 9.67. What is hydrogen ion concentration in the solution? (c) ClO3- and ClO4- ions have same number of electron pairs around central chlorine but their geometry is different. Give Comment about it. (d) Why a mixture of HCl and KCl does not function as a buffer where as a mixture of CH3COOH and CH3COONa does?
Acetic acid and a salt containing its conjugate base, such as sodium acetate, form buffer solutions that are effective in the pH range 3.7-5.7. (a) In resisting a pH change, which buffer component would react with NaOH? Explain. (b) What happens to the buffer activity when this component is exhausted?
1. Consider Ammonia, NH3, with Kb= 1.8x10-5 (a) What is the pH of a buffer solution prepared by adding 13.36g of ammonium chloride (NH4Cl) to .50 L of .400 M (b) What is the pH of the buffer after 100.0 mL of 1.50 M HCl are added to the solution from part (a)? (c) What is the pH of the buffer after 4.00g of NaOH are added to the solution from part (a)? (d) What is the pH of the buffer after 30.0g of NaOH are added to the solution from part (a)?
B ONLY (a)How many ml of 0.5 M HCl must be added to 100.0 ml of a 0.2 M Imidazole (C3H4N2 ; Kb=6.3x10-8) solution to obtain a pH of 5.52? (b)Is this solution a buffer?
Calculate the pH when 40.00 mL of 1.000 x 10 M HF is titrated (aq) 7a) -1with 1.150 x 10 M FrOH at the equivalence point. (aq) 7b) What is ONE best indicator for this titration? 7c) What is the best buffer pH for this titration?
A buffer solution contains 0.82 mol of hypobromous acid (HBrO) and 0.32 mol of sodium hypobromite (NaOBr) in 8.60 L.The Ka of hypobromous acid (HBrO) is Ka = 2.5e-09.(a) What is the pH of this buffer?pH = (b) What is the pH of the buffer after the addition of 0.20 mol of NaOH? (assume no volume change)pH = (c) What is the pH of the original buffer after the addition of 0.16 mol of HI? (assume no volume change)pH =
6. ( ) A 40 mL sample of a 0.2 M RNHz (kb = 3.7 x 10") is titrated with 0.2 M HC (eg). Calculate the pH after the addition of each of the following volume acids. a) Initial pH (b) Volume of HCI (ag): 20 mL (c) Volume of HCI (ag): 39.9 mL (d) Volume of HCI (ag): 40.0 mL (e) Volume of HCI (ag): 40.1 mL
Determine the pH during the titration of 58.9 mL of 0.341 M formic acid (Ka = 1.8×10-4) by 0.341 M NaOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any NaOH (b) After the addition of 14.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 88.4 mL of NaOH
Determine the pH during the titration of 69.1 mL of 0.366 M benzoic acid (Ka = 6.3×10-5) by 0.366 M NaOH at the following points. (Assume the titration is done at 25 °C.)(a) Before the addition of any NaOH (b) After the addition of 16.0 mL of NaOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 104 mL of NaOH