2. Fill in the following table to show the theoretical results for the titration of 1.0 L of 0.20 M acetic acid by adding the designated amount of solid (no volume change) potassium hydroxide, KOH. Show sample calculation of your work. Amount of NaOH added 0.0 mol 0.010 mol 0.020 mol 0.030 mol 0.040 mol Amount of acetic acid remaining pH [H+]

2. Fill in the following table to show the theoretical results for the titration of 1.0 L of 0.20 M acetic acid by adding the designated amount of solid (no volume change) potassium hydroxide, KOH. Show sample calculation of your work. Amount of NaOH added 0.0 mol 0.010 mol 0.020 mol 0.030 mol 0.040 mol Amount of acetic acid remaining pH [H+]

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.29QAP

See similar textbooks

Similar questions

I did an experiment called Potentiometric Analyses where we titrate NaOH with a solid unknown weak acid. Our group was told that our weak acid is diprotic. Mass of dry, solid acid = .155g Molar concentration of NaOH (mol/L)= 0.100 Buret reading of NaOH, initial (mL)= 50 mL Buret reading NaOH at stocichiometric point, final (mL)= 22.1 mL Volume of NaOH dispensed (mL) 27.9 mL Moles of NaOH to stoichiometric point (mol) : _____________ (I think the above answer would be 2.79 x 10-2? if yes then skip) Moles of acid (mol) _____________ Molar mass of acid (g/mol) __________ Note: In the book it says for a diprotic acid, 2 mol of OH-, neutralizes one mole of acid.
The next 11 questions are related to the titration of 30.00 mL of a 0.1000 M acetic acid solution with 0.0800 M KOH. Assume that the temperature is 25 oC.What is the initial pH of the analyte solution? What volume of KOH is required to reach the equivalence point of the titration? How many mmol of acetate are present at the equivalence point? Report the analytical amount, not the equilibrium amount of acetate at the equivalence point. What is the total volume of the solution at the equivalence point?
In the titration of 50.00mL of 0.2980M HCl, 71.93mL of 0.2173M NaOH was required to reach the phenolphthalien endpoint. Calculate the percent error between the predicted amount and the experimental amount
Calculate the pH of the solution for every 0.1 ml of the titrant (from 0 mL to 30 mL) and generate a titration curve using Excel. A 100.0-mL aliquot of 0.100 M diprotic acid H2A (pK1 = 4.00, pK2 = 8.00) was titrated with 1.00 M NaOH Highlight each stage in the titration and the equivalence point. Also, obtain the first derivative of the curve (that is ΔpH / Δvolume).
Consider the titration of 60.0 mL of 0.200 M pyridine with 0.400 M HCl. What is the pH at 0.00 mL, 15.00 mL, and 31.00 mL of the added acid?
A suitable target for the titration is 30.0 cm3 of 0.025 moldm-3 Br2(aq) Justify why a much smaller target titre would not be appropriate Calculate the amount in moles of bromine in the target titer Justification? calculate a suitable massof alive oil to transfer to the volumetric flask using your answer to of above question and the structure of Y Assume that the olive oil contains 85/- of Y by mass (If you were unable to calculate the amount of bromine in the target titer,you should assume it is 6.25×10^-8 mol .this in not the correct amount)
Why would an indicator end point not be very useful in the titration curve for pKa 10.00
please help!! Valentina titrated the 50.00 mL of 0.30 M formic acid to the equivalence point with 37.5 mL of 0.40 M LiOH. What is the concentration of the formate ion just after the strong reaction is completed?
Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.
The graph shows the titration of the aqueous solution containing 0.138 g of unknown monoprotic acid solution with 0.105M NaOH. Taking into account that the mass of the weak monoprotic acid used in the titration was 0.138 g, calculate the molar mass (MM), and identify the weak acid using the table from the lab manual
Calculate the pH at 0, 25, 50, 100 and 150.0mL titrant in the titration of 50.0mL of 0.500 M acetic acid with 0.25 M NaOH.
Consider the titration of 20 mL of 0.10 M base with 0.20 M HCl. The analyte is dibasic withpKb1 = 5.00 and pKb2 = 10.00. Calculate the pH at the following volumes of HCl0 mL, 5 mL, 10 mL, 15 mL, 20 mL