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Biochemistry Laboratory

Laboratory lecture notes on acids, bases, and buffers
Course

Veterinary Medicine

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Academic year: 2022/2023
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Mariano Marcos State University

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BIOCHEMISTRY LABORATORY

Introduction

Definition of acid and base based on: 1. Arrhenius a. Acid  A substance that dissociates in water to form hydrogen ions or protons. In other words, it increases the number of H+ ions in the water.  Example: HCl b. Base  Dissociates in water to form hydroxide ions, OH-.  Example: NaOH 2. Bronsted- Lowry a. Acid  A chemical species capable of donating a proton. b. Base

A chemical species

capable of accepting a proton. In other words, it is a species that has a lone electron pair available to bond to H+. 3. Lewis a. Acid

Chemical species which

have empty orbitals and are able to accept electron pairs from Lewis bases.

b. Base

 Chemical species having a

highly localized HOMO (Highest Occupied Molecular Orbital). These chemical species have the ability to donate an electron pair to a given Lewis acid in order to form an adduct.  Example: Ammonia

 A quantitative measure of the acidity or basicity of aqueous or other liquid solutions.  The term "pH" was first described by Danish biochemist Søren Peter Lauritz Sorensen in 1909. pH is an abbreviation for "power of hydrogen" where "p" is short for the German word for power, potenz and H is the element symbol for hydrogen.  The pH scale runs from 0 to 14  pH < 7, basic; pH > 7, acidic, pH = 7, neutral

 pH = -log[H+] - where log is the base 10 logarithm and [H+] is the hydrogen ion concentration in moles per liter

Acids and Bases

What is pH?

Formula for pH

 The Henderson- hasselbalch equation provides a relationship between the pH of acids (in aqueous solutions) and their pKa (acid dissociation constant).  apH = pK + log ([A-]/[HA]) - [A-] = molar concentration of a conjugate base - [HA] = molar concentration of an undissociated weak acid (M) To solve for pOH:  pOH = pKb + log ([HB+]/[ B ])

  • [HB+] = molar concentration of the conjugate base (M)
  • [ B ] = molar concentration of a weak base (M)

BIOCHEMISTRY LABORATORY

Introduction

Definition of acid and base based on: 1. Arrhenius a. Acid  Gives off hydrogen ions  Turns litmus paper red  Taste: sour  Example: HCl b. Base  Gives off hydroxide ions  Turns litmus paper blue  Taste: bitter  Example: NaOH 2. Bronsted- Lowry

 It refers to the hydrogen ion concentration  How acidic or basic a liquid solution is  Tells you how much hydrogen ions are being given off  The pH scale runs from 0 to 14  pH < 7, acidic; pH > 7, basic, pH = 7, neutral

Henderson-hasselbalch Equation

Acids and Bases What is pH?

Notes

pH change is known as buffer action.

 Addition of salt  Slight increase or decrease in the pH (depending where the salt came from)  Stronger acid = decrease pH  Stronger base = increase pH  Addition of water  Also known as dilution  No effect; It does not affect the pH of the buffer  Increase Temperature  Lower pH  Increasing the temperature creates more hydrogen and hydroxide ions (ionize)

acetate

  • Dihydrogen phosphate and monohydrogen phosphate
  • Sodium dihydrogen phosphate and disodium hydrogen phosphate  Salt is a product of the reaction of acids and bases
  • HCl + NaOH  NaCl + H 2 O  The chemical process of producing salt is called neutralization  Water is a cleansing agent  Weak acids that are used in buffers have Ka values of not more than 10-  To obtain a buffer solution with a definite pH choose an acid with a pKa value that is approximate to the pH if the buffer solution.
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Biochemistry Laboratory

Course: Veterinary Medicine

5 Documents
Students shared 5 documents in this course

University: Mariano Marcos State University

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BIOCHEMISTRY LABORATORY
Introduction
Definition of acid and base based on:
1. Arrhenius
a. Acid
A substance that
dissociates in water to
form hydrogen ions or
protons. In other
words, it increases the
number of H+ ions in
the water.
Example: HCl
b. Base
Dissociates in water to
form hydroxide ions,
OH-.
Example: NaOH
2. Bronsted- Lowry
a. Acid
A chemical species
capable of donating a
proton.
b. Base
A chemical species
capable of accepting a
proton. In other words,
it is a species that has
a lone electron
pair available to bond to
H+.
3. Lewis
a. Acid
Chemical species which
have empty orbitals and
are able to accept
electron pairs from
Lewis bases.
b. Base
Chemical species having a
highly localized HOMO
(Highest Occupied
Molecular Orbital). These
chemical species have the
ability to donate an electron
pair to a given Lewis acid in
order to form an adduct.
Example: Ammonia
A quantitative measure of the
acidity or basicity of aqueous
or other liquid solutions.
The term "pH" was first
described by Danish
biochemist Søren Peter
Lauritz Sorensen in 1909. pH
is an abbreviation for "power
of hydrogen" where "p" is
short for the German word
for power, potenz and H is
the element symbol for
hydrogen.
The pH scale runs from 0 to
14
pH < 7, basic; pH > 7, acidic,
pH = 7, neutral
pH = -log[H+]
- where log is the base 10
logarithm and [H+] is the
hydrogen ion concentration
in moles per liter
Acids and Bases
What is pH?
Formula for pH

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