3.00g of activated charcoal was added to 50 mL of acetic acid solution (0.4 mol/L) in a conical flask. After shaking for 5 minutes, it was filtered and 25 ml of the filtrate was titrated with 0.1 mol/L NaOH using 1% Phenolphthalein indicator and the equivalence point occurred after adding about 31.40 ml of NaOH. Calculate the amount (in mg) of acetic acid absorbed (per gram of charcoal).

3.00g of activated charcoal was added to 50 mL of acetic acid solution (0.4 mol/L) in a conical flask. After shaking for 5 minutes, it was filtered and 25 ml of the filtrate was titrated with 0.1 mol/L NaOH using 1% Phenolphthalein indicator and the equivalence point occurred after adding about 31.40 ml of NaOH. Calculate the amount (in mg) of acetic acid absorbed (per gram of charcoal).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

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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.
A 250.0-mg sample of an organic weak acid was dissolved in an appropriate solvent and titrated with 0.0556 M NaOH, requiring 32.58 mL to reach the end point. Determine the compound’s equivalent weight.
3 A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is titrated with 0.1062 M HCl by the double indicator method. It is found that 40.83 mL of the acid are required to reach the phenolphthalein end point. Methyl orange is then added to the solution and the titration continued using an additional 12.38 mL of the acid. Calculate the percentage of each component in the sample.
A 250.0-mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.0663 M NaOH, requiring 35.18 mL to reach the end point. Determine the compound’s equivalent weight
A 1.2 g sample of mixture of NaOH and Na:COs containing inert impurities s dissolved and titrated cold with 0.5N HCI. With phenolphthalein as indicator the solution turns colorless after the addition of 30.0 mL of the acid. Methyl orange is then added and 12 ml more of the acid is required before this indicator changes color. What is the percentage of NaOH and of Na:COs in the sample ?
(a) Sketch a pH vs base volume curve for a weak acid/strong base titration. (b) Identify which region of the curve is the equivalence point. (c) Assuming the titration is stopped exactly at the equivalence point, and that the acid's Ka value is 1.82 x 10-5, what is the pH at the equivalence point?
Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL of 0.0090 M NaOH was added to the collected H,SO4, and the excess base was then back titrated with 13.45 mL of 0.0100 M HCI. Calculate the sulfur content in the sample in parts per million. This problem involves back titration. Write the two chemical equations involved in the analysis. Identify the analyte, “bridging" reagent and titrant. Solve for the mole of the analyte using the titration values and the stoich relationships. One mole of H2SO4 is equal to one mole of sulfur in the sample. Solve for the mass of S then the ppm S.
A 1.2 g sample of mixture of NaOH and Na:CO. containing inert impurities s dissolved and titrated cold with 0.5N HCI. With phenolphthalein as indicator the solution turns colorless after the addition of 30.0 ml of the acid. Methyl orange is then added and 12 ml more of the acid is required before this indicator changes color. What is the percentage of NaOH and of Na:CO, in the sample ? 5.
What is a primary reason for needing to standardize strong base titrants like NaOH and KOH? 1)Standardization is the process of dissolving NaOH or KOH in aqueous solution.2)NaOH and KOH are both inexpensive, highly soluble, and easy-to-use bases.3)Standardization is the process of reacting a strong base like NaOH or KOH with an acid.4)NaOH and KOH both react with moisture in the air thereby making accurately-determined concentrations of their solutions difficult.5)NaOH and KOH are not very soluble in aqueous solutions making the concentrations difficult to determine.
b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.
A 0.4263 g solid sample containing NaCl and KBr only was dissolved in 50 mL of water and titrated to the Ag2CrO4 end point, requiring 36.85 mL of 0.1120 M AgNO3. A blank titration requires 0.71 mL of titrant to reach the same endpoint. Calculate the weight percentage of Cl in the solid sample.
10.) 0.085 g of an unknown diprotic acid is titrated with 0.115 M NaOH. The first equivalence point occurred in the titration at a volume of 9.00 mL of NaOH added; The second equivalence point occurred at a volume of 18.00 mL of NaOH added. How many moles of NaOH were used to reach the second equivalence point in this diprotic acid titration? mol NaOH mol