Which one of the following would make the best buffer? (Ac = acetate) O a solution of ammonia and ammonium chloride, NH3 and NH4Cl O a solution of hydrochloric acid and sodium chloride, HCl and NaCl a solution of acetic acid and ammonium chloride, HAC and NH4CI O a solution of acetic acid and ammonia, NaAc and NH3

Which one of the following would make the best buffer? (Ac = acetate) O a solution of ammonia and ammonium chloride, NH3 and NH4Cl O a solution of hydrochloric acid and sodium chloride, HCl and NaCl a solution of acetic acid and ammonium chloride, HAC and NH4CI O a solution of acetic acid and ammonia, NaAc and NH3

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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For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?
Which of the following would make the best buffer with the highest "buffer capacity"? 100 mM NH4+ and 5 mM NaOH 100 mM NH4+ and 10 mM NaOH 100 mM NH4+ and 25 mM NaOH 100 mM NH4+ and 50 mM NaOH 100 mM NH4+ and 100 mM NaOH
What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.10 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴)
Each graph below represents a titration involving solutions of two of the following substances: HC2H3O2, HNO3, CH3NH2 and NaOH. Which graph best represents HC2H3O2 being titrated using NaOH? Which graph best represents HC2H3O2 being titrated using CH3NH2? Which graph best represents HNO3 being titrated using NaOH? Which graph best represents HNO3 being titrated using CH3NH2? Which graph has the lowest pH at the equivalence point? Which graph has the equivalence point pH that is equal to 7?
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)
How many of the following three choices are not effective buffers?NaCHO 2/HCHO 2NaH 2PO 4/H 3PO 4NaF/NaOH
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH
Which pair could be a buffer? NaCl and KCl Weak base and its conjugate acid Strong base and a strong acid Strong base and its conjugate acid
What is the pH of an aqueous solution containing 75.0 mL of a 0.15M HNO2 solution and 45.0 mL of a .25M KNO2? What is the pH of this solution after 10.0 mL of a 0.20M solution of KOH is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)?