**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.

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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...

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Suppose you need a buffer with a pH of 4.9. Which conjugate acid-base pair should you use? O sodium hydrogen carbonate (NaHCO3, pKa = 10.3) and sodium carbonate (Na2CO3) O hydrocyanic acid (HCN, pKa = 9.3) and potassium cyanide (LİCN) %3D O hypochlorous acid (HCIO, pKa = 7.5) and potassium hypochlorite (KCIO) O acetic acid (HC2H3O2, pKa = 4.8) and sodium acetate (NaC2H3O2)
A 100.0 mL buffer solution is constructed using 0.035 M HX, a weak acid, and 0.045 M NaX. Ka, HX = 4.7 x 10-6 a) Based on the Ka, what is the pH range where the buffer should be effective. b) From the given concentrations, what is the actual pH of the constructed buffer. c) What would the pH of the buffer if 0.0020 mol of HCl is added to the buffer solution. d) What would the pH be if 0.0020 mol of HCl was added to 100.0 mL of pure water without the presence of the buffer. Assume NaX and HCI completely dissociate.
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
An acetate buffer has a ph of 5, how much will be ionized? how much will be unionized? how much of drug P (kb = 7 x 10^-8) in solution at pH 8 will be: ionized? unionized?
A buffer is prepared from 60.0 mL of 0.100 M formic acid(HCOOH) and 40.0 mL of 0.100 M formate (HCOO --). What is thepH of the buffer solution ? K a of formic acid is 1.78 x 10 4
Is the following solution a buffer? Each solution was prepared by mixing and diluting appropriate quantities of the two solutes to yield the concentrations indicated. 0.10 M NaCN and 0.10 M NaCl a.yesb.no
Write a balanced molecular equation between the reactions of Buffer and NaOH
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
For a buffer containing HF (aq) and NaF (aq), what ratio of ([F ]/ [HF]) is needed to give a buffer of pH 2.35? 0.16 O 1.00 0.45 0.80 O 6.31
Which of the following solutions is a good buffer system? A) a solution thats is 0.10 M HNO2 and 0.10 M NaNO2 B) a solution that is 0.10 M NaOH and 0.10 M HNO3 C) a solution that is 0.10 M NaCl and 0.10 M HCI D) a solution that us 0.10 M HCN and 0.10 M HCI
Which pair of compounds will form a buffer in aqueous solution? HCNHCN and HClHCl NaCNNaCN and KCNKCN HClHCl and NaOHNaOH HCNHCN and NaCNNaCN NaCNNaCN and NaOHNaOH HClHCl and NaCl
Which of the following would destroy a buffer containing 0.134 moles of weak acid HA and 0.268 moles of conjugate base A -? 0.134 mol of HCl 0.186 mol of HCl 0.0670 mol of NaOH 0.0447 mol of NaOH 0.268 mol of HCl