Please explain how to calculate the pH. In the next part of the experiment, you added successive quantities of HCl to the buffer solution, and measured the pH.Concentration of HCl solution (M)0.100Volume of aliquots of HCl solution2.00added before each measurement (mL)AMOUNT OF EACH SPECIES AFTER ADDITION OF HCINow, calculate the amount of each species present in the buffer after the addition of successive volumes of HCl, input yourexperimental pH value, and calculate the expected pH value.Amount present in buffer (mmol)Volume ofHCl (mL)NH4+NH3PHH3O+ExperimentalCalculated(Unrounded)Calculated(rounded)0.000.8000.4000.0009.2488.950788.9512.001.0000.2000.0008.8478.551808.5525.408044.001.2000.0000.0003.8439.25180 ×5.4086.001.2000.0000.2002.7129.251808.001.2000.0000.4002.4779.2518010.001.2000.0000.6002.34512.002000.0000.8002.2112.079186P222

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Answered: In the next part of the experiment, you…

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 8STP

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Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.
Explain why even though an aqueous acetic acid solution contains acetic acid and acetate ions, it cannot be a buffer.
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
Sulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.
Calculate the pH of these buffers.
What is meant by the capacity of a buffer? Describe a buffer with low capacity and the same buffer with greater capacity.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
what volume of acetic acid 0.1 M and what volume of sodium acetate 0.1 M should be added together to produce a solution (buffer) with a pH of 4.6?
How many moles of potassium hydroxide would have to be added to 250 mL of a 0.385 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.360? moles
Consider the buffer system composed of benzoic acid, HC, H,O,, and its conjugate base benzoate, C,H,0;. HC,H,0, + H,0 = H,0* +C,H,0, Using Le Châtelier's principle, predict how the concentration of each substance changes by the addition of H,O*. Does the concentration of HC, H,0, increase or decrease when H,0* is added? O increase decrease Does the concentration of C, H,0, increase or decrease when H,O* is added? O decrease O increase Does the concentration of H,O* change significantly when H,O* is added? O no Does the concentration of H,O* change significantly when H,Ot is added? по yes Does the pH change significantly when H,O is added? no O yes Using Le Châtclier's principle, predict how the concentration of cach substance changes by the addition of OH. Does the concentration of HC,H,O, increase or decrease when OH is added? increase O decrease Does the concentration of C,H,O, increase or decrease when OH" is added? O decrease

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