gageNOWI CX S Geometry w/Datax S Practice 10.10 | SexS Practice | SchoolcXG Sign in - Google/XLogins & Passwo X+t.cengagenow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator= assignment-takeOther E[Review Topics][References]Use the References to access important values if needed for this question.A buffer solution is 0.414 M in KHSO3 and 0.254 M in K₂SO3. If K₂ for HSO3 is 6.4 x 10-8, what is thepH of this buffer solution?pH =Submit AnswerRetry Entire GroupNo more group attempts remainVisitedDC

Acidic buffer : A mixture of weak acid and its salt with strong base is defined as acidic buffer…

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values if needed for this question. A buffer solution is 0.414 M in KHSO3 and 0.254 M in K₂SO3. If Ka for HSO3 is 6.4 x 10-8, what is the pH of this buffer solution? pH =

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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To prepare the buffer in the previous problem, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.99 M. (Remember the lesson on dilution: M1V1=M2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Write your answer in 3 decimal places without the unit). PREVIOUS PROBLEM:
Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the total vol. of buffer
What is the pH of a solution that contains a concentration of 1.35 x 10−5{"version":"1.1","math":"<math xmlns="http://www.w3.org/1998/Math/MathML"><mn>1</mn><mo>.</mo><mn>35</mn><mo> </mo><mi>x</mi><mo> </mo><msup><mn>10</mn><mrow><mo>-</mo><mn>5</mn></mrow></msup></math>"}M of H3O+{"version":"1.1","math":"<math xmlns="http://www.w3.org/1998/Math/MathML"><msub><mi>H</mi><mn>3</mn></msub><msup><mi>O</mi><mo>+</mo></msup></math>"}? Question 6 options: 0.99 - acid 4.9 - acid 0.99 - base 4.9 - base
to prepare the buffer in the previous problem, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: M1V1=M2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Write your answer in 2 decimal places without the unit).
In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
5. How would you prepare a liter of “carbonate buffer” at a pH of 10.10? H2CO3 ↔ H+ + HCO3- Ka = 4.2 x 10-7 HCO3-↔ H+ + CO3-2 Ka = 4.8 x 10-11 a 1stbuffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution b 2ndbuffer is preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution c 1stbuffer preferred to prepare at mole ratio of 0.60 to 1.0, dissolve in enough water to make up a 1-L solution d 2nd buffer is preferred to prepare at mole ratio of 0.40 to 1.0, dissolve in enough water to make up a 1-L solution
To prepare the buffer, a total volume of 600 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 1.5 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 2 decimal places)
(2). For the buffer system, what will be the pH when (a) 15.0 ml of 0.500 M HCl and (b) when 15.0 ml of 0.750 M NaOH is added to the buffer? Given: • 20.0 ml of 3.00 M sodium bicarbonate = conjugate base in molarity [? −] • 50.0 ML OF 2.00 M carbonic acid = weak acid in molarity [??] • 4.30 × 10−7 ?? of carbonic = ??? (acid-dissociation constant) • Base: (a) 15.0 ml of 0.500 M HCl (b) 15.0 ml of 0.750 M NaOH
enumerate the steps necessary to create a Phosphate Buffer NaH2PO4 - K2HPO4 with a final volume of 500 mL, a concentration of 0.10M, and a pH of 7.20 using 0.20 M NaH2PO4 and solid K2HPO4. Nota bene: Ka equals 6.3 x 10-8. (show computation as well) For solid K2HPO4, calculate for the mass (based from calculated moles of salt) rather than the volume since this is a solid substance.
Suppose you were designing a buffer system for imitationblood and wanted the buffer to maintain the blood at therealistic pH of 7.40. All other things being equal, whichbuffer system would be preferable: H2 CO3 / HCO3- orH2 PO-4 /HPO42- ? Explain.
A buffer system works to keep pH within a narrow range. Buffer systemsare critical in all living cells/tissues. If pH were to measurably shift in a cell,what category of biological molecules would be most impacted, andwhat term refers to the resulting loss of their functional shapes? A buffer is a substance that, when it ionizes in water, creates a buffersystem. The substance and one of its ions represent a weak acid and aweak base. These form a pH-controlled equilibrium. Based on thedefinitions of acid and base, if [H+] increases, which would combine withthe H+, preventing a pH shift? If [H+] decreases, whichwould release H+ to counter a pH change? Check the one characteristic below that is important in a buffer system. maintains a neutral pH prevents pH from dropping prevents pH from rising minimizes change in p
Calculate the volume (ml)of concentrated ammonia and the weight (gm) of ammonium chloride respectively to be taken to prepare 100 ml of buffer solution at a pH of 10 if the final concentration of the salt is 0.20 mol. Note that the molar concentration of concentrated ammonia is equal to 14.8 mol/liter, and that the pKb of ammonia is 4.76, and the molecular weight of ammonium :chloride 53.5 g/mole.lt is about