The K, expression for the H, PO, /HPO buffer is given by the equation Ionic strength (u, M) 0.005 0.010 | 0.050| 0.10 0.933 0.914 0.86 0,83 [HPO | Yuro;- [H*] ru• K, = Yuro; - YH, PO; 0.740 0.660 0.445 0.355 = 10-720 (H,PO, | 74,0; 0.928 0.902 0.82 0.775 What is the pH of a 3:2 mixture of H, PO, to HPO - at an ionic strength of 0.050 M? Activity coefficients can be found in the table.

The K, expression for the H, PO, /HPO buffer is given by the equation Ionic strength (u, M) 0.005 0.010 | 0.050| 0.10 0.933 0.914 0.86 0,83 [HPO | Yuro;- [H*] ru• K, = Yuro; - YH, PO; 0.740 0.660 0.445 0.355 = 10-720 (H,PO, | 74,0; 0.928 0.902 0.82 0.775 What is the pH of a 3:2 mixture of H, PO, to HPO - at an ionic strength of 0.050 M? Activity coefficients can be found in the table.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 120IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

See similar textbooks

Similar questions

Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
The Ka expression for the H,PO,/HPO? - buffer is given by the equation Ionic strength (µ, M) 0.005 0.010 0.050 0.10 YH* 0.933 0.914 | 0.86 0.83 [HPO}-] Yuro; [H*] YH" Ка [H,PO] YH,PO, YHPO; 0.740 0.660| 0.445 0.355 = 10-7.20 YH, PO, 0.928 0.902 0.82 0.775 What is the pH of a 3:4 mixture of H, PO, to HPO- at an 2 ionic strength of 0.005 M? Activity coefficients can be found in the table. pH = 6.994
Calculate the pH of a buffer that is 0.012 M C6H;COOH ( Ka= 6.3x10-5) and 0.033 M NaC6HsCOO.
A 5.55-g sample of a weak acid with Ka = 1.3 * 10 - 4 was combined with 5.00 mL of 6.00 M NaOH, and the resulting solution was diluted to 750.0 mL. The measured pH of the solution was 4.25. What is the molar mass of the weak acid?
1: Cônsider the following buffer solution: 600.0 ml 0.550 M CH,COOH 0.325 M NACH,CO K - 1.76 x 10 Determine the pH of the buffering system after 170.0 ml of 2.00 M NaOH has been added. Part "A": Process the initial information and determine the buffer's initial pH and the initial moles of CH;COOH, NACH,CO0 and NAOH. Part "B": Analyze the in information above and determine if this is a Type I, Il or III Bothering the Buffer problem. Explain your decision (.a sentence or two should be sufficient) Part "C": Perform the necessary calculations and determine the pH of the buffer after the NAOH addition. Your answer should contain the correct number of S.F. Part "D": Compare your answer to the buffer's original pH and determine whether it is reasonable or not. Explain your rationale. O Focus 中

Please help me...... a. Do you expect the pH at the equivalence to be lowest when a 0.0500 M (CH3)3N(aq) solution or a C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution at 25.0 oC? Motivate your answer! (CH3)3N (Kb = 6.5 × 10-5) and C5H5N (Kb = 1.7×10-9) are weak monoprotic bases. Calculate the pH at the equivalence point and 25 oC when 1.00 L of a 0.0500 M C5H5N(aq) solution is titrated with a 0.0500 M HCl(aq) solution. Calculate the molar solubility for CaCO3 in a 0.060 M Ca(NO3)2(aq) solution. Ksp= 3.1 × 10-9 for CaCO3.
A chemistry graduate student is given 125. mL of a 1.50M diethylamine ((C,H, NH solution. Diethylamine is a weak base with K,=1.3 × 10 °. What mass (HIN %3D of (C,H5), NH,Br should the student dissolve in the (C,H,) NH solution to turn it into a buffer with pH =10.79? 2. You may assume that the volume of the solution doesn't change when the (C,H) NH, Br is dissolved in it. Be sure your answer has a unit symbol, and round 12 it to 2 significant digits. 10
Calculate the pH at the equivalence point in titrating 0.084 M solutions of each of the following with 0.078 M NAOH. (a) hydrobromic acid (HBr) pH = 2.52 (b) hydrosulfuric acid (H,S), K, = 9.5e-08 pH = 7.05 (c) phenol (HCsHş0), K, = 1.3e-10 pH =
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 Ka = 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 x 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
(f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)