B? The concentrations of acid and base in buffer B are twice the concentrations of buffer A (buffer B is twice as strong as buffer A). Show that the ratio of the volume of titrant required to raise the pH of each buffer 1 unit (VB/VA) is directly related to the ratio of the buffer strengths (strengthB/strengtha) be Buffer capaaty ldefined uuhnn hu 1 unuf/ hy the H change and votume of huffer ucd in hbres cun ar Hhe nuolet ofaud or han needed to clane the

B? The concentrations of acid and base in buffer B are twice the concentrations of buffer A (buffer B is twice as strong as buffer A). Show that the ratio of the volume of titrant required to raise the pH of each buffer 1 unit (VB/VA) is directly related to the ratio of the buffer strengths (strengthB/strengtha) be Buffer capaaty ldefined uuhnn hu 1 unuf/ hy the H change and votume of huffer ucd in hbres cun ar Hhe nuolet ofaud or han needed to clane the

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 10P

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Similar questions

A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
A titration curve is constructed by plotting the pH of the analyte solution versus the volume ofthe reagent added as the titration progresses. As the equivalence point is approached, there is arapid change in the pH. Titration curves enable us to explain how end points are detected andtheir relationship to equivalence points. They can also serve as guides for choosing the properindicators for a particular acid-base titration. Explain how each plot can be used to interpret the acid-base titration.
What species are in the buffer region of a weak acid–strong base titration? How are they different from the species at the equivalence point? How are they different from the species inthe buffer region of a weak base–strong acid titration?
The graph below, which is related to a titration curve, shows the fraction (f) of the stoichiometric amount of acetic acid present as non-ionized CH3COOH and as acetate ion, CH3COO-, as a function of the pH of the solution containing these species. (Graph piture attached) Explain the significance of the point at which the two curves cross. What are the fractions and the pH at that point?
Draw the titration curve, when 40.00 mL of 0.22 M ammonia solution is titrated with 0.50 M HCl. As with this does not need to be 100% perfect, but should correctly represent the important characteristics such as shape of the curve and pH values at the 4 distinct locations: Beginning, buffer region, equivalence point, beyond plateau.
For each of the statements, identify the appropriate key point(s) (I, II, III, IV, V) in the titration.
The titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? Given that the chemical reaction is 2MnO4- + 5C2O42- + 16H+ -----> 2Mn2+ + 10CO2 + 8H2O Provide a detailed solution.
Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Let x represent the original concentration of CH3COO- in the water. based on the given values, set up the ICE table in order to determine the unknown
Build a titration curve for the following scenarios. Make sure to label your accesses and anyother appropriate pieces of data. Each curve should have a minimum of 4 data points, but youcan use the following to help structure your curvea) Initial pHb) pH at Veqc) pH=pka (if applicable)d) pH when excess titrant is addede) Additional pH point near Veq for Strong Acid/Strong Base titrations (in order to see thesteepness of the slope) OR additional pH point in buffer zone for titrations with a Weakcompound.