For 490.0 mL of a buffer solution that is 0.185 M in CH3CH₂NH₂ and 0.135 M inCH3CH₂NH3C1, calculate the initial pH and the final pH after adding 1.3×102 molof HCL. (Kb (CH3CH₂NH₂) = 5.6 x 10-4.)Express your answers using two decimal places separated by a comma.pHnitial, PHfinal =195] ΑΣΦ

This is an basic buffer solution with amonium ion salt and amonia base

For 490.0 mL of a buffer solution that is 0.185 M in CH3CH₂NH₂ and 0.135 Min CH3CH₂NH3C1, calculate the initial pH and the final pH after adding 1.3x102 mol of HCL. (Kb (CH3CH₂NH₂) = 5.6 x 10-4.) Express your answers using two decimal places separated by a comma. VE ΑΣΦ pHnitial PHfinal ?

For 490.0 mL of a buffer solution that is 0.185 M in CH3CH₂NH₂ and 0.135 Min CH3CH₂NH3C1, calculate the initial pH and the final pH after adding 1.3x102 mol of HCL. (Kb (CH3CH₂NH₂) = 5.6 x 10-4.) Express your answers using two decimal places separated by a comma. VE ΑΣΦ pHnitial PHfinal ?

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

Write the buffer equilibrium reaction, then write the neutralization reaction. What isthe pH of the 0.20M NH3/NH4CL buffer after the addition of 10.0 mL of 0.10 HCl to65.0 mL of buffer? The Ka for NH3 is 5.6 x 10-10
For 280.0 mL of a buffer solution that is 0.315 M in CH3CH2NH2 and 0.220 M in CH3CH2NH3Cl, calculate the initial pH and the final pHpH after adding 0.024 mol of NaOH. ( Kb(CH3CH2NH2)=5.6×10−4Kb(CH3CH2NH2)=5.6×10−4.)
A 25.0 mL sample of 0.450 M (CH3)2NH is titrated with HBr. What is the pH of the solution after 30.0 mL of 0.375 M HBr have been added to the methylamine solution? ((CH3)2NH; Kb Give answer to 2 decimal places. = 5.9×10-4)
For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)
What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.
A buffer solution is made that is 0.415 M in CH3COOH and 0.415 M in CH3COO- . (1) If Ka for CH3COOH is 1.80×10-5 , what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.103 mol HI is added to 1.00 L of the buffer solution. Use H3O+ instead of H+ .
What is the pH of a solution prepared by mixing 20.0 mL of 0.50 M NaOH and 35.0 mL of 0.50 benzoic acid solution? (Benzoic acid is monoprotic with a Ka of 6.5 x 10-5.)
the pKb values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.36. calculate the pH at all points in the titration of 50 mL of a .55 M B solution with 55 M HCI: before the addition of HCl, after the additon of 25 mL HCI, after addition of 50 mL HCl, after addition of 75 mL HCl, after addition of 75 mL HCl, after addition of 100 mL HCl
Part A A 440 mL sample of a 0.100 M formate buffer, pH 3.75, is treated with 4 mL of 1.00 M KOH. What is the pH following this addition? (pKa for formic acid is 3.75) Express your answer to two decimal places. VE ΑΣΦ pH = ?
What is the pH of a solution when 100.0 mL of a 0.1M HCN solution (Ka =6.2 x 10 -10) is titrated with 55.0 mL of a 0.075 M NaOH solution? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)? Where does this problem fall on the titration curve: (initial solution, buffer region, equivalence point, post-equivalence point) ? . Sketch the titration curve for this problem and indicate where the answer to this problem is located on this curve.
For 250.0 mL of a buffer solution that is 0.290 M in CH3CH2NH2 and 0.210 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 0.022 mol of NaOH . ( Kb(CH3CH2NH2)=5.6×10−4 .) What is the initial and final pH?
Determine the pH of a buffer formed by dissolving 21.5 g HC₇H₅O₂ and 37.7 g of NaC₇H₅O₂ in 200.0 mL of solution. The value of Ka for HC₇H₅O₂ is 6.3 × 10⁻⁵. Enter an answer with 2 significant figures.