A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 × 10¬1º. ( PREV 1 2 3 Based on your ICE table and Kb expression, determine the original concentration of C6H5NH;*. [C,H$NH;*]; M %3D RESET 8.3 x 1010 0.86 1.2 10 2.1 0.50

A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 × 10¬1º. ( PREV 1 2 3 Based on your ICE table and Kb expression, determine the original concentration of C6H5NH;. [C,H$NH;]; M %3D RESET 8.3 x 1010 0.86 1.2 10 2.1 0.50

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

Macmillan Learning A buffered solution containing dissolved aniline, CH,NH2, and aniline hydrochloride, CH, NH, Cl, has a pH of 5.74. Determine the concentration of C6H5NH in the solution if the concentration of C6H5NH2 is 0.305 M. The pK, of aniline is 9.13. [CH_NH] = Calculate the change in pH of the solution, ApH, if 0.363 g NaOH is added to the buffer for a final volume of 1.70 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M
Design a buffer that has a pH of 6.70 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ką pKa HC,04 C,0,²- 6.4 x 10-5 4.19 H,PO4 HPO,2- 6.2 x 10-8 7.21 HCO3 co,?- 4.8 × 10-11| 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base =
So I have the correc answer
Determine the pH of a buffer that is 0.25 M NH3 and 0.15 M NH:CI. The value of pKb for NH3 is 4.75. 1 2 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH:(aq) H:O(1) ОН (аq) NH.*(aq) + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.25 0.15 4.75 +x -X +2x -2x 0.25 + x 0.25 - x 0.25 + 2x 0.25 - 2x 0.15 + x 0.15 - x 0.15 + 2x 0.15 - 2x
Calculate the pH of a solution that is 0.200 M in NH3 and 0.300 M in NH4Cl. Calculate the pH change that takes place when a 100-mL portion of (A) 0.0500 M NaOH and (B) 0.0500 M HCl is added to 400 mL of the buffer solution. Kb = 1.75 x 10-5 show your solution in picture
What is the effective pH range for a sodium acetate/acetic acid buffer? Ka = 1.80 x 105. %3D Enter your answer to three decimals. to
Determine the [H3O+H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2HCH3CO2H (HAc), is 4.745. You will also need this information in your post-lab. It is highly suggested you write these calculations down (both unrounded and rounded values) to use later. Solution 1.10 M Acetic Acid (mL) 0.900 M Sodium acetate (mL) [H3O+H3O+] (M) 1 8.00 2.00 Solution 1 Concentration 2 7.00 3.00 Solution 2 Concentration 3 6.00 4.00 Solution 3 Concentration 4 5.00 5.00 Solution 4 Concentration 5 4.00 6.00 Solution 5 Concentration 6 3.00 7.00 Solution 6 Concentration 7 2.00 8.00 Solution 7 Concentration 8 1.00 9.00 Solution 8 Concentration Solution 1 Concentration: M Solution 2 Concentration: M Solution 3 Concentration: M Solution 4 Concentration: M…
Please help explaining this one. For 270.0 mLmL of a buffer solution that is 0.270 MM in CH3CH2NH2 and 0.195 MM in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.030 mol of NaOH. Kb(CH3CH2NH2)=5.6×10^−4
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is the best choice for making a buffer solution with an optimum pH in the range of 3.1-3.5? O O O NaNO2/HNO2 (K₂ = 4.6 x 10-4) KCH3COO/CH3COOH (K₂ = 1.75 x 10-5) CH3NH2/CH3NH3CI (K₂ = 2.3 x 10-11) NaOCN/HOCN (K₂ = 2.0 x 10-4) NaNO3/HNO3 20