Logout Open In App
Open In App
Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

Chapter 11: Q35P (page 261)

Prepare a second derivative graph to find the end point from the following titration data.

Short Answer

Expert verified

The graph is shown below

Step by step solution

01

Excel sheet regarding calculation

The calculation in excel sheet for determining the 2nd derivative is shown below

02

Graph

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

When22.63mlof aqueousNaOHwere added to1.214gof cyclohexylaminoethanesulfonic acid(FM207.29 structure in Table 9-2)dissolved in41.37ml of water, the pH was 9.24. Calculate the molarity of theNaOH

Why does an acid-base titration curve (pH versus volume of titrant) have an abrupt change at the equivalence point?

Titration on Diprotic Systems

11-28 . A solution containing 0.100M glutamic acid (the molecule with no net charge) was titrated to its first equivalence point with0.0250MRbOH.

(a) Draw the structures of reactants and products.

(b) Calculate the at the first equivalence point.

The balance says that you have weighed out 1.023 g of tris to

standardize a solution of HCl. Use the buoyancy correction in Section 2-3 and the density in Table 11-4 to determine how many grams you have really weighed out. The volume of HCl required to react with the tris was 28.37 mL. Does the buoyancy correction introduce a random or a systematic error into the calculated molarity of HCl? What is the magnitude of the error expressed as a percentage? Is the calculated molarity of HCl higher or lower than the true molarity?

Question:Titrating weak acid with weak base.

(a) Prepare a family of graphs for the titration of 50.0 mL of 0.020 0 M HA (pKa = 4.00) with 0.100 M B (pKb = 3.00, 6.00, and 9.00).

(b) Write the acid-base reaction that occurs when acetic acid and sodium benzoate (the salt of benzoic acid) are mixed, and find the equilibrium constant for the reaction. Find the pH of a solution prepared by mixing 212 mL of 0.200 M acetic acid with 325 mL of 0.050 0 M sodium benzoate.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free