Using the table of the weak base below, you have chosen Aniline as your weak base in thebuffer solution. You have already added enough of the conjugate acid salt to make the buffersolution concentration at 0.71 M in this salt. The desired pH of the buffer should be equal to3.8.Values of K₁ for Some Common Weak BasesConjugateAcidNameFormulaKbAmmoniaNH4+1.8 x 10-5NH3CH,NH,MethylamineCH3NH3 +4.38 x 10-4C₂H5NH₂C₂H5NH3+5.6 x 10-4EthylamineAnilineCH;NH,C6H5NH3 +3.8 x 10-10PyridineC,H,NCH;NH*1.7 x 10-⁹3. Compute the concentration of the weak base in Molarity (round off answer to 4decimal places).

Given: Buffer solution of weak base aniline (assuming B) and its conjugate acid HB+. pH of solution…

Using the table of the weak base below, you have chosen Aniline as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.71 M in this salt. The desired pH of the buffer should be equal to 3.8. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Kb Ammonia NH4+ 1.8 x 10-5 NH3 CH;NH, Methylamine CH3NH3+ 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3+ 3.8 x 10-10 Pyridine C,H,N CH;NH* 1.7 x 10-⁹ 3. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).

Using the table of the weak base below, you have chosen Aniline as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.71 M in this salt. The desired pH of the buffer should be equal to 3.8. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Kb Ammonia NH4+ 1.8 x 10-5 NH3 CH;NH, Methylamine CH3NH3+ 4.38 x 10-4 C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Ethylamine Aniline CH;NH, C6H5NH3+ 3.8 x 10-10 Pyridine C,H,N CH;NH* 1.7 x 10-⁹ 3. Compute the concentration of the weak base in Molarity (round off answer to 4 decimal places).

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

A buffered solution containing dissolved aniline, CH,NH,, and aniline hydrochloride, CH, NH, Cl, has a pH of 5.27. Determine the concentration of CH, NH in the solution if the concentration of CH, NH, is 0.275 M. The pK, of aniline is $ 9.13. [CH_NH] = = Calculate the change in pH of the solution, ApH, if 0.386 g NaOH is added to the buffer for a final volume of 1.35 L. Assume that any contribution of NaOH to the volume is negligible. ApH = M
A chemist titrates 230.0 mL of a 0.1072M ethylamine (C,H,NH,) solution with 0.5758M HCI solution at 25 °C. Calculate the pH at equivalence. The p K, of ethylamine is 3.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = Explanation Check 2021 McGraw-Hill Education All Rights sved T Le/Py 18 MacBook Air esc F7 FI F2 F3 F4 *
In Part A, a 15.00 mL aliquot of a 0.155 mol L-1 3-methylbutanoic acid solution was titrated to its equivalence point with 11.7 mL of 0.198 molL-1 NaOH solution. At the equivalence point, all of the weak acid, 3-methylbutanoic acid, is converted to its weak conjugate base, 3-methylbutanoate. What is the pH at this equivalence point? 6.957 4.770 8.855 5.145 O 9.230
Is it possible if u can get back to me asap when u see this??!~
You have 1.00 L of 0.10-M formic acid, HCOOH, whose Ka = 3.0 x 10-4. You want to bubble into the formic acid solution sufficient HCl gas to decrease the pH of the formic acid solution by 1.0 pH unit. Calculate the volume of HCl (liters) that must be used at STP to bring about the desired change in pH. Assume no volume change has occurred in the solution due to the addition of HCl gas.
A solution is prepared at 25 °C that is initially 0.14M in benzoic acid (HC, H, CO,), a weak acid with K=6.3 × 10 and 0.41M in potassium benzoate (KC H, CO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0
Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).
using the simultaneous equation method. please answer fully
A 12.0 mL sample of NH3 is titrated with 0.225 M HCI (aq). It takes 9.50 mL of HCI (aq) to reach the equivalence point. Answer the following questions to three significant figures. The pk, for ammonia (NH3) is 4.75. What is the concentration of NH3 in the original solution? Enter a value accurate to three significant figures. Number M What is the pH at the equivalence point? Enter a value accurate to three significant figures. Number
A solution is prepared at 25 °C that is initially 0.17M in trìmethylamine (CH,) N), a weak base with K = 7.4 × 10 *, and 0.20M in trimethylammonium ((CH,), NHCI). Calculate the pH of the solution. Round your answer to 2 decimal places. chloride pH =
An analytical chemist is titrating 106.5 mL of a 0.1100 M solution of methylamine (CH3NH₂) with a 0.8500M solution of HNO3. The p K₁ of methylamine is 3.36. Calculate the pH of the base solution after the chemist has added 11.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH 0 × S