10. (12 pts) Formic acid, HCCOH, ionizes according to the following equation:HCOOH(aq)+H,O(l)=HCOO (aq)+H,O* (aq)You have 500.0 mL of 0.200 M forming acid. Calculate the volume of NaOH, 0.0500 M, thatshould be added to formic acid to form a buffer that has a pH of 4.00. Ka = 4.0 × 104.14. (12 pts) Calculate the pH of 0.200 M Barium acetate, Ba(CH3COO)2. Ka for aceticacid, CH3COOH, is 1.8 × 10-5.

Answered: Image /qna-images/answer/d47584c6-c23f-4a9e-8bd3-9b7e9c68c972.jpg

Answered: 10. (12 pts) Formic acid, HCCOH,…

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

What is the pH of 0.33 M acetic acid to 1.00 L of which 1.44 g of sodium acetate, NaCH3 CO2, has been added? (Ka for acetic acid is 1.8 x 10-) pH =
Ff.33.
For which of the following mixtures will Ag2SO4(s) precipitate? 150.0 mL of 0.10 M Na₂SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) 150.0 mL of 0.10 M Na₂SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq) 150.0 mL of 0.10 M Na₂SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)
A buffer is prepared by mixing a hypothetical weak acid, HA (pKa = 6.06) with its sodium salt. If 0.10 moles of HA and 0.50 moles of NaA are mixed with enough water to make 250.0 mL of solution, what is the pH of the buffer? Report your answer to 2 decimal places (e.g. 1.23 or 12.34) Your Answer: Answer
9:26 A buffer solution contains 0.274 M C,HgNH3Br and 0.386 M C,H5NH2 (aniline). Determine the pH change when 0.093 mol HBr is added to 1.00 L of the buffer. pH after addition – pH before addition = pH change =
10. A buffer solution is made of mixture of aqueous methanolic acid, HCOOH. With aqueous sodium methanolate acid NaHCO. The equilibrium reaction takes place in buffer solution is: НСООН < НСОО + Н Small amount of NaOH is then added to that buffer solution. What reaction take places at the buffer solution to resist change of pH caused by addition of base? а. НСООН +H* b. HCOO+H* НСООН НСООН с. НСООН +ОН" d. HCOOH +ОН" НСОО +Н2О НСООН
You have a 5.0% formic acid (HCOOH) solution and a 5.0% vinegar (acetic acid, CH3COOH3) solution. You titrate 5.0 mL of each with 0.1868 M NaOH. Which would need more NaOH to reach the end point? How much more? Show calculations.
Comparing the two quantities based on the given condition, which is greater I or II? or are they equal? Can the quantities be compared? Ten (10) mL of solution X contains 0.100 M HCl and 0.100 M HA (pKa = 5) Ten (10) mL of solution Y contains 0.100 M HCl and 0.100 M HB (pKa = 7) Both solutions are titrated with 0.100 M NaOH. I. Volume of titrant required to reach the 2nd equivalence point in solution X II. Volume of titrant required to reach the 2nd equivalence point in solution Y.
A4. For an unknown acid lab, titrating with 0.1 M NaOH, what is an acid that is slightly brown solid and has a molar pass of 74-76 g/mol?
For different enzymes, there is an optimum pH at which the enzyme is most active. For example, for enzymes of gastric juice optimum pH 1-2, for duodenal enzymes pH 7.7, for liver enzymes pH 9.5, etc. Determine which medium (a or b) is most favorable for each of the enzymes mentioned above if the following substances are added to 1.0 liter of water: a) 0.040 mol KOH and 0.030 mol HBr; b) 4.0 10-9 mol HNO3. Neglect the change in the volume of the solution. Confirm your answer with calculations.
A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K = 4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 5.00 mL of NaOH are added to the analyte? Question 4 A 10.00 mL sample of 1.20 M HNO2 (analyte) (pK, = 3.34 and K, -4.57x104) is titrated with 1.20 M NaOH (titrant), what is the pH when 10.00 mL of NaOH are added to the analyte? Assume Ku = 1.0 x 10-14 Using the titration curve below for the titration of 10.00 mL of the analyte NH3 with HCl(aq) (titrant) to estimate pKa for NH3 Titration of 10.00 mL Ammonia (ag) with Hydrochloric Acid (ag) 12.0 11.0 10.0 9.0 8.0 7.0 5.0 4.0 3.0 2.0 1.0 0.0 0.0 2.0 4.0 10.0 12.0 140 16.0 180 20.0 6.0 Volume of HCI Added (mL) 8.0
After the neutralization reaction of 42% 0.5 mL nitric acid and 0.28M 18 mL sodium hydroxide, a temperature increase of 15 ° C was observed and the temperature value was determined as 825 cal. According to these results; What is the number of moles of neutralized base? (d(HNO3) = 1,51 g/mL; M(HNO3)=63,01 g/mol)

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS