**Buffer System Analysis**The following buffer system is composed of HOCl and OCl⁻.**Equations:**1. HOCl + H₂O ⇌ OCl⁻ + H₃O⁺2. NaOCl → Na⁺ + OCl⁻ (in the presence of water)**Questions:**A) Is this buffer composed of a weak acid and its conjugate base or a weak base and its conjugate acid?B) What is the purpose of the NaOCl? What does it provide? Be specific.C) Which part of the buffer neutralizes base (OH⁻) that is added? Be specific.D) Which part of the buffer neutralizes acid (H⁺) that is added? Be specific.**Additional Task:**Identify and draw the correct structures for four isomers with the chemical formula C₆H₁₄.

"As you have posted multiple questions, so we will solve the first question posted and please post…

der the following buffer system, made up of HOCI and OCT HOCI+ H₂O OCI + H₂O' H₂O NaOCI- Na + oci A) Is this buffer composed of a weak acid and its conjugate base or a weak base and its conjugate acid? B) What is the purpose of the NaOCI? What does it provide? Be specific C) Which part of the buffer neutralizes base (OH) that is added? Be specific D) Which part of the buffer neutralizes acid (H) that is added? Be specific

der the following buffer system, made up of HOCI and OCT HOCI+ H₂O OCI + H₂O' H₂O NaOCI- Na + oci A) Is this buffer composed of a weak acid and its conjugate base or a weak base and its conjugate acid? B) What is the purpose of the NaOCI? What does it provide? Be specific C) Which part of the buffer neutralizes base (OH) that is added? Be specific D) Which part of the buffer neutralizes acid (H) that is added? Be specific

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

When titrating 125 mL of nitric acid HNO3 0.165 mol/L, with KOH 0.219 mol/L.a) What is the pH of the solution before starting the titration, and what volume of KOH (in mL) is required to reach the equivalence point?b) What is the pH of the solution after the addition of 44.5 mL of KOH solution?c) What is the pH of the solution at the equivalence point, and the pH of the solution after the addition of 200 mL of KOH solution?
nts) Consider the following buffer system, made up of HOCI and OCT HOCI + H₂O H₂0 OCI + H₂O NaOCI H₂O Na + OCI A) Is this buffer composed of a weak acid and its conjugate base or a weak base and its conjugate acid? B) What is the purpose of the NaOCI? What does it provide? Be specific C) Which part of the buffer neutralizes base (OH) that is added? Be specific D) Which part of the buffer neutralizes acid (H') that is added? Be specific There are many isomers that fit the chemical formula CH Draw the correct 6. structures for 4 of them.
Which of the following solutions is a buffer system?
0.50 M solutions of each weak acid in the table are available. Choose an acid solution and determine what volume, in mL, of a 1.00 M NaOH solution should be added to 1.00 L of the acid solution to create a buffer with pH = 6.88. acid/base pairs to use: Ka pKa HCO2H/NaHCO2 1.8×10-4 3.74 H2CO3/NaHCO3 4.2×10-7 6.38 HBO3/NaH2BO3 7.3×10-10 9.14 NaHCO3/Na2CO3 4.8×10-11 10.32 HCO2H/NaHCO2 H2CO3/NaHCO3 H3BO3/NaH2BO3 NaHCO3/Na2CO3 ---------mL NaOH
Which of the following does not represent the correct formula for a compound of sodium? A) NaCI B) Na20 C) Nas D) Na3N Which of the following can be constituents of a buffer solution? A) CH3COOH + CH3COONa B) HCI + CH3COONH4 C) CH3COOH + NH3CI D) NaOH + HCI NFIDENT Which of the following statement best describes the equation below and product formed? HCI(aq)+ NaOH(aq)→ NaCl(aq) +H,O (1) Sodium chloride (table salt) A) Salts contain a cation (a metal or ammonium ion) derived from the base and an anion excluding oxide or hydroxide ions) derived from the acid. B) Salts are ionic compounds C) Salts are generally crystalline compounds with high melting and boiling points. D) A, B and Care correct
Which statement describes the action of a buffer composed of propionic acid (CH, H, COOH) and sodium propionate (NaCH, CH,COO)? Propionic acid neutralizes added base, and sodium propionate neutralizes added acid. Sodium propionate neutralizes added base, and propionic acid neutralizes added acid. Both components, propionic acid and sodium propionate, neutralize added base. Both components, propionic acid and sodium propionate, neutralize added acid.
For each of the buffer systems below, determine the concentration of the acid and base components in the buffer: 1) An acetate buffer with a pH of 5.15 and a concentration of 3.5M. The (HC2H302] = Type your answer here M and the [NAC2H302] = Type your answer here M 2) A Carbonate buffer with a pH of 9.85 and a concentration of 0.50M. The [NAHCO3] = Type your answer here M and the Na2CO3] = Type your answer here M 3) A Phosphate buffer of pH 2.5 and a concentration of 1.0M. The [H3PO4] = Type your answer here Mand the [KH2PO4) Type your answer here
1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL pure water.
Write a balanced molecular equation between the reactions of Buffer and NaOH
Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1 mole HCL + 0.1 mole KCl 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4 0.1 mole NaCl + 0.1 mole KCl 0.1 mole of H3O+ + 0.1 mole OH- I am guessing option 2, but need clarification please!
Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base are mixed in equimolar proportions? Acid NH4* (from ammonia) HC₂H3O2 (acetic acid) HF (hydrofluoric acid) CH3CH₂NH3 (from ethylamine) acetic acid. b) ethylamine c) ammonia d) hydrofluoric acid e) none Ka 5.69 10-10 1.75 10-5 6.810-4 2.12 10-11
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).