QI/ One of the student wanted to calculate the exact of HCl concentration.He made standardization of 10 ml NaOH with 0.1M H,C,0,2H,0according to the table:Titration-H2C204 (Burette)Run. NoV in. mlV final ml End point12512Then, he made titration of 10 ml HCl with standard solution of NaOHaccording to the table:Titration-NAOH (Burette)Run. NoV in. mlV final mlEnd point110.221020.3Was the student successful in the titration ? why? So what is theconcentration of HCI?

The question is based on the concept of acid base titrations. we need to calculate concentration of…

QI/ One of the student wanted to calculate the exact of HCl concentration. He made standardization of 10 ml NaOH with 0.IM H;C,O4.2H,0 according to the table: Titration- H2C204 (Burette) Run. No V in. ml V final ml End point 1 5 5 12 Then, he made titration of 10 ml HCI with standard solution of NaOH according to the table: Titration- NaOH (Burette) Run. No V in. ml V final ml End point 1 10.2 10 20.3 Was the student successful in the titration ? why? So what is the

QI/ One of the student wanted to calculate the exact of HCl concentration. He made standardization of 10 ml NaOH with 0.IM H;C,O4.2H,0 according to the table: Titration- H2C204 (Burette) Run. No V in. ml V final ml End point 1 5 5 12 Then, he made titration of 10 ml HCI with standard solution of NaOH according to the table: Titration- NaOH (Burette) Run. No V in. ml V final ml End point 1 10.2 10 20.3 Was the student successful in the titration ? why? So what is the

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.14QAP

See similar textbooks

Similar questions

A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
please stop rejecting. we pay for this service, so we deserve getting our answer! I do not want to have to put a claim in and report Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10