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

Determine the mass of solid NaCH,COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH;COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH,COOH is 1.8 x 10. NEXT > Let x represent the original concentration of CH;COO in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq) + H2O(1) H,O (aq) CH;COO (aq) Initial (M) Change (M) Equilibrium (M)
Give a clear handwritten answer with explanation
(Please type answer note write by hand)
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