A 25.0-mL volume of 0.040 0 M phosphoric acid was titrated with 0.050 0 M tetramethylammonium hydroxide. Write the series of titration reactions and find the pH at the following volumes of added base: Vb 0, 10.0, 20.0, 30.0, 40.0, and 42.0 mL. Sketch the titration curve and predict what the shape will be beyond 42.0 mL.

A 25.0-mL volume of 0.040 0 M phosphoric acid was titrated with 0.050 0 M tetramethylammonium hydroxide. Write the series of titration reactions and find the pH at the following volumes of added base: Vb 0, 10.0, 20.0, 30.0, 40.0, and 42.0 mL. Sketch the titration curve and predict what the shape will be beyond 42.0 mL.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 3.1ACP

See similar textbooks

Similar questions

Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid:(a) 0 mL(b) 15.00 mL(c) 29.00 mL(d) 29.90 mL(e) 30.00 mL(f ) 30.10 mL(g) 40.00 mL
You are going to titrate 29.0 mL of 0.294 M cyanic acid (HCNO) with 0.15 M NaOH. What is the pH of the solution after 5.684 mL of the NaOH has been added? The Ka of cyanic acid at the temperature of the experiment is 2.3 x 10-4. Report your answer to the hundredths place and do not include units
Find the pH during the titration of 20.00 mL of 0.2850 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.2850 M NaOH solution after the following additions of titrant. (a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 20.00 mL(e) 25.00 mL
Generate a curve for the titration of 50.00 mL of a solution in which the analytical concentration of HClO4 is 0.1000 M and that of formic acid is 0.0800 M. Calculate the pH after the addition of 0.00,10.00, 20.00, 24.00, 25.00, 26.00, 35.00, 44.00, 45.00, 46.00 and 50,00 ml of KOH 0,2000 M.
Construct a curve for the titration of 50.0 mL of 0.100 M hydrazoic acid, HN3 (Ka = 2.2 x 10-5) with 0.200 M solution of KOH. Calculate the pH after the addition of 0.00,12.50, 20.00, 24.00, 25.00, 26.00, 37.50, 45, and 50.00 mL of titrant. Identify the specie/species present at the following regions of the curve:a. Start of the titrationb. Before equivalence pointc. At equivalence pointd. Past the equivalence point.
if 15.00mL of 0.0500 M HCl is used to titrate 30.00mL saturated Ca(OH)2, calculate the molar concentration. Then, Based on the molar concentration of Ca(OH)2 from this question, calculate the Ksp of Ca(OH)2.
Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus:  250-mL conical flasks  Clamp  Burette  Graduated cylinder  Pipette Reagents / Materials:  Vinegar  Phenolphthalein indicator  0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid  The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…
Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH₃CH₂CH₂COOH (Kₐ=1.54X10⁻⁵), with0.1000 M NaOH solution after the following additions of titrant:(a) 0 mL(b) 10.00 mL(c) 15.00 mL(d) 19.00 mL(e) 19.95 mL(f ) 20.00 mL(g) 20.05 mL(h) 25.00 mL
What is the pH in the titration of 15.0 mL of 0.40 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 25.0 mL of 0.45 M NaOH?
1Upon the addition of 30.00 mL of 0.350 M HCl to a 80.00-mL of the weak base amine (Kb = 4.95 x 10-10) whose concentration is 0.530M, the resulting pH is then equal to 8.80. True or False? 2.When 100 mL of a 1.0M strong acid is 50% titrated with 1.0M strong base, the volume of the base should be added is 50mL and this corresponds the equivalence point. True or False? 3. The pH of a buffer can be calculated using the formula: 14-pOH = pKb + log of [proton acceptor]/[acid component]. True or False?
Use the following experimental titration data to calculate the concentration of the acid being analysed. Observations: The initial solution of acetic acid (HC2H3O2) is clear and colourless. A few drops of phenolphthalein indicator are added to each sample. A dilute solution of sodium hydroxide (concentration 2.50 x 10-4 mol/L) is used as the titrant. As the mixture reaches the endpoint, flashes of pink colour are seen and the titrant is added drop by drop. The endpoint is reached when one drop of titrant turns the mixture a pale pink colour that does not fade.
Calculate the pH during the titration of 40.00 mL of 0.0250 M KOH with 0.0500 M HCl after addition of the following volumes of titrant reagent (HCl): a) 0.00 mL b) 10.00 mL c) 15.00 mL d) 18.00 mL e) 20.00 mL f) 25.00 mL