4 1. wite a balanced equation for each of the following neutralization reactionsa.HSO, and RbOHH2 Soy Caa)b. Ca(OH), and HCIO.C HPO. and Mg(OH);2. Predict whether the following pairs of substances could function as a buffer system is aqueoussolution. (indicate yes or no)2. HNO; and KNO,b. H,SO. and NaHSo.C. NANO, and HNO,d. NAHCO, and K;CO,

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Answered: 1. Write a balanced equation for each…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 57P

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What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
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The pH of a buffer solution that is made by mixing 124 mL of 0.156 M of acetic acids (pls=4.74) with 56.8 mL of 0.106 M sodium acetate is ?
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Two buffers are prepared by adding an equal numberof moles of formic acid (HCOOH) and sodium formate(HCOONa) to enough water to make 1.00 L of solution.Buffer A is prepared using 1.00 mol each of formic acid andsodium formate. Buffer B is prepared by using 0.010 mol ofeach. (a) Calculate the pH of each buffer. (b) Which bufferwill have the greater buffer capacity? (c) Calculate thechange in pH for each buffer upon the addition of 1.0 mLof 1.00 M HCl. (d) Calculate the change in pH for each bufferupon the addition of 10 mL of 1.00 M HCl.
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