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

Nitrogen is discharged from wastewater treatment facilities into rivers and streams, usually as NH₃ and NH₄⁺: NH₃(aq)+H₂O(l) → NH₄⁺(aq)+OH⁻(aq) K(b)=1.76X10⁻⁵ One strategy for removing it is to raise the pH and “strip” the NH₃ from solution by bubbling air through the water. (a) AtpH 7.00, what fraction of the total nitrogen in solution is NH3,defined as [NH₃]/([NH₃] [NH₄⁺])? (b) What is the fraction at pH 10.00? (c) Explain the basis of ammonia stripping.
Given that Ka's for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 x 10-4 and 5.4 x 10-10, respectively, calculate the pH of the following solutions: (a) The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3). (b) The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.
PR: (a) Calculate the pH of a buffer solution prepared by dissolving 0.20 mole of sodium cyanate (NaCNO) and 1.0 mole of cyanic acid (HCNO) in enough water to make 800. mL of solution. (10). (b) Calculate the pH after 0.050 moles of NaOH are added to the buffer solution (assume no volume change) (10). Ka (HCNO) = 2.0 × 10-4
1. the temperature for each solution is carried out at approximately 297 K where Kw = 1.00 x 10 ^-14 (a) 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 4.5 L of solution. What is the pH of the resulting hydrochloric acid solution? (b) 0.70 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution ?
What is the pH of a solution made by adding 0.65 m of acetic acid (H3CO2H) and 0.30 mol of sodium acetate (H3CO2Na) to enough water to make a 1.0 L solution? (K, = 1.8 x 105) %3D CH3CO2H (aq) + H2O (1) CH3CO2° (aq) + H3O* (aq) 4.74 O 5.08 04.40 8.92
A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.
A common indicator ionizes in solution according to the equation: HA(aq) → H"(aq) + A (aq) reaction (1) red yellow When the indicator is dissolved in distilled water, the solution is yellow. If excess HCl is added to the solution, the solution turns (or stays) v as the v reaction predominates to establish equilibrium. We know that the dissociation of water takes place in the same solution: H2O(1) + H*(aq) + OH"(aq) reaction (2) If excess NaOH is added to the solution, the equilibrium in reaction (2) shifts to the v, thereby v H". The consequent effect on reaction (1) would be that the color is
The acetate ion, CH-COO", reacts with water as a weak base: CH,CO0 (aq) + H2O02 CH COOH(ag) + OH"(ag), with K-5.7x 10 10 at 25°C. If sodium acetate were dissolved in water to make a 0.35 M solution, what would be the resulting concentration of OH ? (M)
ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Ao
Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (non-ionized) acid form. If a patient takes an antacid that adjusts the pH of the stomach contents to 2.59 and then takes two 5-grain aspirin tablets (total 0.65 g), how many grams of aspirin are available for immediate absorption from the stomach, assuming immediate dissolution> Also assume that aspirin does not change the pH of the stomach contents. The pKa of aspirin is 3.5, and its formula weight is 180.2.
Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (non-ionized) acid form. If a patient takes an antacid that adjusts the pH of the stomach contents to 2.59 and then takes two 5-grain aspirin tablets (total 0.65 g), how many grams of aspirin are available for immediate absorption from the stomach, assuming immediate dissolution> Also assume that aspirin does not change the pH of the stomach contents. The pKa of aspirin is 3.5, and its formula weight is 180.2. _______ mg
5:50 1 Search Question 5 of 20 Submit Determine the mass of solid NaCH;COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH-COОH is 1.8 х 10-5. 1 2 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. CH3COOH+ H20(1) =H;O*(aq) +CH3COO-(a Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 × 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 х+ 5.00 x - 5.00 x + 1.0 × 10-9 х - 1.0 х 10-9 1.0 x 10-5 x - 1.0 × 10-5 x + 1.8 × 10-5 х - 1.8 х 10-5

SEE MORE QUESTIONS

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