The plot below is for the titration of 30.00 mL CH3COOH with 0.150M KOH:CH3COOH (aq) + KOH(aq) → CH3COOK(aq) + H2O(l).->Titration of a weak acid with 0.150 M KOH solution14.0012.00Hd10.008.006.004.002.000.000.0010.0020.0030.0040.0050.0060.00Volume of KOH (mL)What is the approximate molar concentration of the weak acid solution? [mol acid/volume of acid]You can use MAVA-MBVB.Answer: 0. (3 significant figures). Do not include the unit, M.

Given: VCH3COOH = 30.0 ml , MKOH = 0.150 MVKOH = 38.2 ml (at the equivalence point from the given…

Answered: The plot below is for the titration of…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.103QE

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in the titration of 50.0 mL of 0.0200 M C6H5COOH(aq) with 0.100 M NaOH(aq), what is/are the major species in the solution after the addition of 5.0 mL of NaOH(aq)?
For the titration of 20.0 mL of 0.400 M HCl(aq) with 0.400 M NaOH(aq): 1. What is the initial pH of the HCl(aq)? HCl(aq) + NaOH(aq) NaCl(aq) + H₂O(l) pH = [Select] 2. What is the pH of the HCl(aq) after the addition of 10.00 mL of NaOH ? 3. What is the pH of the HCl(aq) after the addition of 20.0 mL of NaOH? pH = [Select] pH = [Select]
For the titration of 20.0 mL of 0.400 M HCI(aq) with 0.400 M NAOH(aq): HCI(ag) + NaOH(aq) NaC(aq) + H2O) 1. What is the initial pH of the HC(aq)? pH = |Select ] 2. What is the pH of the HCI(aq) after the addition of 10.00 mL of NaOH ? pH= [ Select] 3. What is the pH of the HCI(aq) after the addition of 20.0 mL of NaOH? pH [ Select]
(f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)
A titration is carried out for 50.00 mL of 0.100 M HNO3 (strong acid) with 0.200 M of a strong base NaOH (the titration curve is shown to the right). Calculate the pH at these volumes of added base solution: A B C D 0.200 M NaOH added 00.0 mL 15.0 mL 25.0 mL 40.0 mL HNO3(aq) + NaOH(aq) H₂O(9) + NaNO3(aq) pH of solution - Equivale point Midpoint HAlaq). Volume c
Che. 065: Acid -Base Titration: Part I: Standardization of NaOH(aq): Molarity of NaOH(aq) is determined by using the stoichiometry reaction with a strong acid such as HCl(aq). Part II: Molarity and mass % of acetic acid CH3COOH(aq) in a vinegar solution are determined by the reaction with NaOH(aq). Part I: Standardization of NaOH(aq): Use a 50.00 mL. Buret : wash it with tap H2O twice, with deionized H2O twice and twice with 0.100 M HCl (aq). Fill the buret with 0.100 M HCl(aq), remove the air bubble and adjust the initial buret reading to 0.00 mL. Get two 125 mL. Erlenmeyer. To each Erlenmeyer flask add 20.00 mL. HCl(aq) from the buret. Burette Holder 3P Burette Flask Support Stand Trail 2 Trial 1 Initial buret reading of HCl(aq): 0.00 mL. Final buret reading of HCl(aq): 20.00 mL. Volume of HCl(aq) : Initial buret reading of HCl(aq): 20.00 mL. Final buret reading of HCl(aq): 40.00 mL. Volume of HCl(aq) Add 3 drops of phenolphethaleine to each Erlenmeyer flask, the color of solution is…
A titration of 29.2 mL of a solution of the weak base aniline, C@HNH, ( K 4.0 x 10-10), requires 21.61 mL of 0.155 M HCl to reach the equivalence point. CH_NHz(aq) + HyO* (aq) + C,H,NH, (aq)+H,O(l) a What was the concentration of aniline in the original solution? Concentration 0115 ✔ M The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus, [C,HNH] [H₂O+] [OH-]- = 0.155 mol HC1 1.00 L 1 29.2 mL b What are the concentrations of H₂O¹, OH, and C6H5NHs at the equivalence point? M C = 0.115 M x 21.61 ml x M Correct 1 mol C, H, NH, 1 mol HCl Show Hint
ssume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 7.00 ✕ 102 mL of solution and then titrate the solution with 0.153 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(ℓ) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH-C6H5CO2- M Na+ M H3O+ M OH- M C6H5CO2-
Calculate the value of the equilibrium constant for the balanced net ionic equation for the weak acid- strong base titration. The beaker contains 0.1894 M CH3COOH and the buret contains 0.2006 M NaOH. 24 ml of NaOH is needed to titrate. lonic Equation: CH3COOH (aq.) + OH (aq.) = CH3 COO"(aq.) + H2O (1) Please help thank you.
The pkb values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.65. Calculate the pH at each of the points in the titration of 50.0 mL of a 0.60 M B(aq) solution with 0.60 M HCI(aq). What is the pH before addition of any HCI? pH = What is the pH after addition of 25.0 mL HCI? pH = What is the pH after addition of 50.0 mL HCI? pH What is the pH after addition of 75.0 mL HC1? pH = What is the pH after addition of 100.0 mL HC1? pH =
Molarity of the standard solution of sodium hydroxide 0.1037 mol/L Volumes of NaOH(aq): Rough titration First titration Second titration Third titration Final burette reading: mL) Initial burette reading: (mL) Velume of NaOII(aq) Titrated (added) (mL) 18.53 32.02 21.64 35.53 4.78 18.55 7.89 21.63 Fourth Finh titration titration Final burette reading: (ml) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (ml) 23.78 37.32 10.27 23.80 1. When HaSO<(aq) was reacted with NAOH(aq) in the titration, why was a precipitate not formed? 2. Why did the colour of the solution in the conical flask change at the end of the titration? 3. In this acid-base titration, what did we use to measure the volume of the Ha$O.(aq)? 4. What do we mean by stoichiometric point of a titration?
A volume of 500.0 mL of 0.100 M NaOH is added to 525 mL of 0.200 M weak acid (K, = 6.27 x 10), What is the pH of the resulting buffer? HA(aq) + OH (aq) H,O() + A (aq) pH = If a buffer solution is 0.190 M in a weak acid (K, = 5.7 x 10-) and 0.550 M in its conjugate base, what is the pH? pH =

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