Nuetralization reaction
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The document discusses classifying solutions as acidic, basic, or neutral based on their properties. It defines acids as having more H3O+ ions than OH- ions and bases as having more OH- ions than H3O+ ions. A solution with equal amounts is neutral. It then classifies a bitter liquid with a pH of 8.0 as basic and a sour liquid with a pH of 2.0 as acidic. The rest of the document discusses acid-base reactions and examples of neutralization reactions forming salts and water.
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This document provides an overview of acids and bases. It begins with a brief history of acids and bases according to Arrhenius' theory. Key points include that acids produce H+ ions and bases produce OH- ions in water. The document then discusses the properties, uses, and pH scale of acids and bases. It explains that acids have a pH below 7 while bases have a pH above 7. The document concludes by noting that the reaction between an acid and base is called neutralization.
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1. The document discusses solutions and solubility. A solution has two parts - a solute that dissolves and a solvent like water that the solute dissolves into.
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Acids and bases p pt
This document defines acids and bases according to the Arrhenius model and discusses their properties in aqueous solutions. It also explains acid-base titrations for determining concentrations and defines pH. Buffers are formed from a weak acid and its conjugate base or weak base and conjugate acid and do not experience large pH changes upon addition of acids or bases.
Acid Base Notes (H)
This document provides information about acids and bases including:
1) Common acids and their names, acid-base definitions using Arrhenius and Brønsted-Lowry models, and properties of acids and bases.
2) Conjugate acid-base pairs, acid and base strength, pH and pOH calculations.
3) Buffers, neutralization reactions, and examples of pH indicators.
Unit 3
This document discusses acids and bases, including their properties and reactions. It defines acids as substances that release hydrogen ions in water and bases as those that release hydroxide ions. Acids and bases neutralize one another in a reaction that produces salt and water. The document also discusses acid-base theories, strong vs. weak acids/bases, pH, electrolytes, self-ionization of water, and acid-base indicators. Buffers are introduced as solutions that resist changes in pH when small amounts of acid or base are added.
Chemistry unit 7 notes
This document provides information about acids and bases including:
- Acids produce H+ ions in water and bases produce OH- ions. The strength depends on how completely they ionize.
- Examples of acids include vinegar and lemon juice. Examples of bases include soap and ammonia. Neutral substances have equal concentrations of H+ and OH- ions.
- Acids have a sour taste and low pH while bases have a bitter taste, slippery feel and high pH.
- The names and formulas of acids can be determined based on their ionic parts. Neutralization reactions between acids and bases produce salt and water. pH indicators are used to determine if a solution is acidic or basic.
Chemistry GCSE Chapter 8 Acid bases and Salts .pptx
This document discusses acids, bases, and salts. It defines acids as substances that produce hydrogen ions in aqueous solution and bases as substances that produce hydroxide ions in aqueous solution. Examples of strong acids and weak acids are provided. The document also discusses the properties of acids and bases, including their reactions with metals, metal hydroxides, metal carbonates to form salts. It introduces the pH scale for measuring acidity and alkalinity and discusses acid-base indicators. Various types of oxides such as basic, acidic, amphoteric, and neutral oxides are also defined.
Acids and Bses
This document provides an overview of acid-base theories and properties. It covers the Bronsted-Lowry and Lewis theories of acids and bases. It defines strong and weak acids and bases, and how their strength affects properties like conductivity and reaction rate. It also introduces the pH scale and explains how pH is determined by the concentration of hydrogen ions in solution.
Acids-bases-salts-VG.ppt
The document discusses acids, bases, and salts. It provides information on the Arrhenius and Bronsted-Lowry theories of acids and bases. Key points include: Arrhenius acids contain H+ ions and bases contain OH- ions. Bronsted-Lowry defined acids as proton donors and bases as proton acceptors. Acids have a pH below 7 while bases are above 7. Neutralization reactions involve acids and bases reacting to form water and a salt. Titration can be used to determine the concentration of an unknown acid or base solution.
Acid,Bases And Salt(s) (ScienCe)
This document discusses acids, bases, and salts. It defines acids as sour tasting substances that increase the hydronium ion concentration in water. Bases are defined as bitter tasting and slippery substances that increase the hydroxide ion concentration in water. Strong acids and bases are completely ionized in water while weak acids and bases are only partially ionized. The document also discusses pH, the logarithmic scale used to measure acidity and alkalinity, and how pH and pOH are related through their sum being equal to 14.
acids-and-bases-lecture.ppt
1. There are three classes of strong electrolytes: strong acids, strong bases, and most water soluble salts. Weak acids and bases only partially dissociate in water.
2. pH is a measure of the concentration of hydrogen ions [H+] in a solution. Low pH indicates high [H+] and an acidic solution, while high pH indicates low [H+] and a basic solution. Household substances like coffee, milk, and baking soda have different pH values.
3. The acid dissociation constant Ka and base dissociation constant Kb are equilibrium constants that indicate the strength of an acid or base. Strong acids and bases fully dissociate while weak acids and bases only partially dissociate,
1. acid base
In the pharmaceutical inorganic chemistry as per PCI for B-pharm FY students easy to understand the topic is Acid and base
Acids and bases
1. The document discusses acids and bases, including their definitions and properties.
2. An acid is defined as a proton donor, donating hydrogen ions (H+) in water. A base is a proton acceptor, accepting hydrogen ions.
3. Common strong acids include hydrochloric acid (HCl), nitric acid (HNO3), and sulfuric acid (H2SO4) which fully ionize in water.
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
Acids, Bases are defined by Four main theories,
1.Traditional theory / concept
2.Arrhenius theory
3.Bronsted and Lowry theory
4.Lewis theory
Importance of acids and bases in pharmacy
Buffers: Buffer action
Buffer capacity Buffers system
Types of Buffers : Generally buffers are of two types:
1. Acidic buffers
2. Basic buffers
There are some other buffer system:
3. Two salts acts as acid-base pair. Ex- Potassium hydrogen phosphate and potassium dihydrogen phosphate.
4. Amphoteric electrolyte. Ex- Solution of glycine.
5. Solution of strong acid and solution of strong base. Ex- Strong HCl with KCl Mechanism of Buffer action: Mechanism of Action of acidic buffers: Buffer equation-Henderson-Hasselbalch equation:
Standard Buffer Solutions Preparation of Buffer Solutions: Buffers in pharmaceutical systems or Application of buffer: Stability of buffers Buffered isotonic solution Types of Buffer Isotonic solution
1. Isotonic Solutions:
2. Hypertonic Solutions:
3. Hypotonic Solution:
Measurement of Tonicity: 1. Hemolytic method: 2. Cryoscopic method or depression of freezing point:
Methods of adjusting the tonicity:
Class I methods:
In this type, sodium chloride or other substances are added to the solution in sufficient quantity to make it isotonic. Then the preparation is brought to its final volume withan isotonic or a buffered isotonic diluting solution.
These methods are of two types:
Cryoscopic method
Sodium chloride equivalent method.
Class II methods:
In this type, water is added in sufficient quantity make the preparation isotonic. Then the preparation is brought to its volume with an isotonic or a buffered isotonic diluting solution.
These methods are of two types:
White-Vincent method
Sprowls method.
22 acids + bases
The document discusses the key properties and reactions of acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Acids react with metals, carbonates, conduct electricity, turn litmus paper red, and neutralize bases. Bases conduct electricity, turn litmus paper blue, and neutralize acids. Theories of acids and bases including Arrhenius, Brønsted-Lowry, and Lewis are explained. Strong and weak acids/bases, monoprotic/diprotic/triprotic acids, pH, titrations, and acid-base indicators are also covered.
Non aqueous titration- Pharmaceutical Analysis
This document discusses non-aqueous acid-base titration. It begins by explaining that non-aqueous titrations are used for substances that are too weakly acidic or basic to give a sharp endpoint in water, or for substances that are insoluble in water. It then covers the major acid-base theories of Arrhenius, Bronsted-Lowry, and Lewis. The document discusses the effects of different solvent types on acid/base strength and how this enables the titration of weaker acids and bases. It provides examples of titrating benzoic acid with sodium methoxide in n-butylamine and titrating ephedrine alkaloid with perchloric acid in glacial acetic acid or d
Apchemunit14presentationpart1 120226122440-phpapp02
This document provides an overview of acids and bases including:
- The Arrhenius, Bronsted-Lowry, and Lewis models of acids and bases
- Key concepts such as conjugate acid-base pairs, acid dissociation constants, and the pH scale
- How to calculate the pH of strong acid solutions, weak acid solutions, and solutions involving conjugate acid-base pairs
- Common strong/weak acids and bases and their properties
The document explains acid and base chemistry concepts thoroughly and provides practice problems to illustrate applications of these concepts.
body fluids (water, acid, base and buffers).pptx
Water is a polar molecule made of two hydrogen atoms bonded to one oxygen atom in a covalent bond. It has many unique properties including being a universal solvent, having high surface tension and specific heat, and exhibiting strong cohesion and adhesion. These properties arise from water's polar nature and hydrogen bonding between water molecules. Buffers help maintain pH and resist changes upon addition of acids or bases through acid-base reactions between their components. The body maintains pH levels through important buffer systems including bicarbonate, phosphate, and proteins that buffer cellular fluids and blood.
22 acids + bases
This document discusses acids and bases. It defines their key properties including reacting with metals, carbonates, conducting electricity, turning litmus paper colors, and neutralizing each other. It explains the theories of Arrhenius, Brønsted-Lowry, and Lewis on acids and bases. It also covers acid-base reactions, indicators, pH, titrations, strong/weak acids and bases, and acid-base stoichiometry.
Acid base information in daily life of people,the theory regarding it in scie...
This document discusses acids, bases, and salts. It covers the key properties of acids and bases, as well as three major theories of acids and bases: Arrhenius, Bronsted-Lowry, and Lewis. It also discusses acid and base strength in terms of acid dissociation constants, as well as neutralization reactions between acids and bases and the use of titrations.
Chapter 7 acids and bases
This document discusses acid-base theories and equilibria in water. It describes the Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases. The autoionization of water and definitions of pH and pOH are explained. Calculations of pH for strong/weak acids and bases, salts, and buffer solutions using the ionization constant and Henderson-Hasselbalch equation are presented with examples. The role of buffers in resisting pH change upon addition of acids or bases is also summarized.
4 acids & bases
This document discusses acids and bases. It defines strong acids as acids that dissociate completely in water, such as HCl, while weak acids like acetic acid dissociate only slightly. The concentration of H3O+ ions in strong acids equals the concentration of the acid. In weak acids it is much less. Strong bases like NaOH also dissociate completely while weak bases like ammonia dissociate slightly. pH is a measure of H3O+ concentration and indicates if a solution is acidic (pH < 7) or basic (pH > 7). Acid-base reactions involve neutralization of acids by bases to form salts and water. Titration can be used to determine unknown concentrations using indicators and the
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Chemistry GCSE Chapter 8 Acid bases and Salts .pptx
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Acids, Bases And Buffers Pharmaceutical Inorganic chemistry UNIT-II (Part-I)
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Apchemunit14presentationpart1 120226122440-phpapp02
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Acid base information in daily life of people,the theory regarding it in scie...
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Nuetralization reaction
- 1. Classify the following solutions as: Acidic Basic Neutral 1. A solution which has more H3O+ ions than OH- ions Acidic 2. A solution with equal amounts of OH ions and H3O+ ions Neutral Basic 3. A bitter liquid with a pH of 8.0 Acidic 4. A sour liquid with a pH of 2.0
- 3. 1. Control: 1. Bottle A 2. Constants: 2. Containers, Kool-Aid 3. Independent Variable: 3. What was added to the KoolAid 4. Dependent Variable: 4. Color change A B C
- 6. Acid/Base Reactions When mixed in the right amounts An Acid + a Base = A “salt” and water Neutralization reaction
- 7. Acid/Base Reactions Many types of “salts” A combination of a cation and an anion
- 8. Acid/Base Reactions Examples: CaCl2 used for de-icing KCl a table salt substitute
- 9. Acid/Base Reactions Example: NaOH (base) + HCl (acid) NaCl + H2O
- 10. Acid/Base Reactions Example: NaOH (base) + HCl (acid) NaCl + H2O