CHEM 102 Lab 7 Acids and Bases

.docx

School

Drexel University *

*We aren’t endorsed by this school

Course

102

Subject

Chemistry

Date

Jan 9, 2024

Type

docx

Pages

Uploaded by DeanGerbil807

Chem Lab 102-102 02/22/2023 Acids and Bases

I. Photo of Experimental procedure II. Signed Data Page III. I n t r o d u c t i o n The purpose of this experiment is to determine the differences, relationships between acids and bases that were gotten from the experiment. We will use titration, also pH indicator and burette to observe and find the equivalence point.

In order to understand the topic, it is necessary to know the definition of acids and bases. By the Bronsted-Lowry theory, acids is a proton (H + ion) donor and the base is a proton acceptor. There are some examples for strong acids like HCL, HBr, and sulfuric acid. Also, there are some examples of strong bases like lithium hydroxide, or sodium hydroxide. When an acid and a base combine to generate water and salt, this process is known as neutralization, and the resultant solution has a pH of 7. An illustration of a neutralizing reaction is as follows: Hydrochloric acid (HCl) + Sodium hydroxide (NaOH) -> Sodium chloride(NaCl) + Water (H 2 O) In this reaction, the sodium ions (Na+) from the base and the chloride ions (Cl-) from the acid combine to make sodium chloride, which is a salt, while the hydrogen ions (H+) from the hydrochloric acid and the hydroxide ions (OH-) from the sodium hydroxide combine to generate water. The resultant mixture has a pH of 7, making it neutral. Titration is an analytical technique that uses a known quantity of one material to react with an unknown ingredient to determine its concentration in a solution. In a typical titration, a solution of the unknown substance is progressively mixed with a solution of a known concentration, or the titrant, until the reaction between the two is complete. The endpoint of the reaction is identified by an indicator that changes color to indicate completion of the reaction. The equivalence point is a point where pH is the acid with the stoichiometric amount of the base in the solution. It is necessary to indicate equivalence point as it helps to indicate the exact volume when the reaction was complete. Furthermore, titration curves shows us the relationship between the Volume of NaOH added and pH so that it the curves are visually seen, and equivalence point, greatest change in pH can be seen too. Acidic strength is measured using a standard called the dissociation constant, or K a . K a can be calculated by the help of the data observed, like a equivalence point and the corresponding pH. This can be determined by the following formula: K a =10 -pH at half volume IV. Calculations and Discussions

Your preview ends here

Eager to read complete document? Join bartleby learn and gain access to the full version

Access to all documents
Unlimited textbook solutions
24/7 expert homework help

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:9780534420123

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

Publisher:Cengage Learning

Principles of Modern Chemistry

Chemistry

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:Cengage Learning

Chemistry

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Cengage Learning

Chemistry

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Cengage Learning

SEE MORE TEXTBOOKS

Recommended textbooks for you

Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning