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19.1 acids, base and salts By Hamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
Final acid and bases rev.
Simplified understandable Acid and bases For nutrition and dietetics students at North Coast Medical Training.
4.2 acids and bases
This document discusses acids and bases according to the Arrhenius and Brønsted-Lowry theories. It defines acids as substances that produce hydrogen ions (H+) or donate protons in water according to Arrhenius, and substances that donate protons according to Brønsted-Lowry. Bases are defined as substances that produce hydroxide ions (OH-) in water according to Arrhenius, and substances that accept protons according to Brønsted-Lowry. Examples of strong and weak acids and bases are given. The limitations of the Arrhenius theory and the concept of conjugate acid-base pairs are also outlined.
Acids and Bases
This document discusses acids and bases. It defines pH as the negative log of the hydrogen ion concentration. The pH scale runs from 0 to 14, with pH 7 being neutral. A change of one pH unit corresponds to a tenfold change in hydrogen ion concentration. Buffers resist changes in pH when small amounts of acid or base are added. They are made by combining a weak acid with its conjugate base, or a weak base with the salt of its conjugate acid.
Acid and bases
This is a summary of the topic "Acids and bases" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
Acids and Bases
An acid is a substance that produces hydrogen ions in water and has a pH less than 7. Strong acids, like hydrochloric acid, are completely ionized in water, while weak acids like acetic acid only partially ionize. Acids react with metals to produce salts and hydrogen gas, with carbonates to produce salts, water and carbon dioxide gas, and with bases to produce salts and water. They have sour tastes and are corrosive.
Chemistry Slides
This document discusses acids, bases and salts. It defines acids as substances that produce hydrogen ions in water, and classifies them as strong or weak based on how completely they ionize. Bases are defined as substances that produce hydroxide ions in water. Salts are formed when hydrogen ions in an acid are replaced by metal ions. The document also describes the reactions of acids with metals and carbonates, as well as the neutralization reaction between acids and bases to form water and a salt.
Diploma_I_Applied science(chemistry)U-III Acid & bases
1) Acids cause substances like lemons and food to be sour and can damage materials like teeth and sculptures. Acids have positively charged hydrogen ions and turn litmus red.
2) Bases have negatively charged hydroxide ions, feel slippery, and turn litmus blue. Common bases include hand soaps and drain cleaners.
3) The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors in reversible acid-base reactions. Both acids and bases can act as conjugates of each other by gaining or losing protons.
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19.1 acids, base and salts By Hamdy Karim
Students will be able to compare between Arrhenius, Bronsted-Lowry, and Lewis theories to identify the acids and bases concept. They also will study the conjugated acids and bases in addition to the Amphoteric Substances as well!
Final acid and bases rev.
Simplified understandable Acid and bases For nutrition and dietetics students at North Coast Medical Training.
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This document discusses acids and bases according to the Arrhenius and Brønsted-Lowry theories. It defines acids as substances that produce hydrogen ions (H+) or donate protons in water according to Arrhenius, and substances that donate protons according to Brønsted-Lowry. Bases are defined as substances that produce hydroxide ions (OH-) in water according to Arrhenius, and substances that accept protons according to Brønsted-Lowry. Examples of strong and weak acids and bases are given. The limitations of the Arrhenius theory and the concept of conjugate acid-base pairs are also outlined.
Acids and Bases
This document discusses acids and bases. It defines pH as the negative log of the hydrogen ion concentration. The pH scale runs from 0 to 14, with pH 7 being neutral. A change of one pH unit corresponds to a tenfold change in hydrogen ion concentration. Buffers resist changes in pH when small amounts of acid or base are added. They are made by combining a weak acid with its conjugate base, or a weak base with the salt of its conjugate acid.
Acid and bases
This is a summary of the topic "Acids and bases" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
Acids and Bases
An acid is a substance that produces hydrogen ions in water and has a pH less than 7. Strong acids, like hydrochloric acid, are completely ionized in water, while weak acids like acetic acid only partially ionize. Acids react with metals to produce salts and hydrogen gas, with carbonates to produce salts, water and carbon dioxide gas, and with bases to produce salts and water. They have sour tastes and are corrosive.
Chemistry Slides
This document discusses acids, bases and salts. It defines acids as substances that produce hydrogen ions in water, and classifies them as strong or weak based on how completely they ionize. Bases are defined as substances that produce hydroxide ions in water. Salts are formed when hydrogen ions in an acid are replaced by metal ions. The document also describes the reactions of acids with metals and carbonates, as well as the neutralization reaction between acids and bases to form water and a salt.
Diploma_I_Applied science(chemistry)U-III Acid & bases
1) Acids cause substances like lemons and food to be sour and can damage materials like teeth and sculptures. Acids have positively charged hydrogen ions and turn litmus red.
2) Bases have negatively charged hydroxide ions, feel slippery, and turn litmus blue. Common bases include hand soaps and drain cleaners.
3) The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors in reversible acid-base reactions. Both acids and bases can act as conjugates of each other by gaining or losing protons.
Acid bases and salts.part 2
This document provides an overview of acids and bases according to the Arrhenius and Brønsted-Lowry theories. It discusses how acids and bases were originally categorized based on their physical properties. The Arrhenius theory defined acids as substances that produce H+ ions in water and bases as substances that produce OH- ions. It also explains that H+ ions actually exist as hydronium ions (H3O+) in water. The Brønsted-Lowry theory expanded this to define acids as proton donors and bases as proton acceptors. Other topics covered include strong vs. weak acids/bases, the autoionization of water, and the pH scale.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
Chapter 7 Acid & Bases part 1
The document discusses acids, bases, and alkalis. It defines them, provides examples, and explains their properties and uses. Acids donate H+ ions in water, bases accept H+ ions and alkalis dissolve in water to form hydroxide ions. Properties of acids include sour taste and turning litmus red, while alkalis have a bitter taste and turn litmus blue. Common acids and bases are used in products like cleaners, soaps, batteries, and more.
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The document discusses acids, bases, and salts. It defines acids as substances that form hydrogen ions in water, such as hydrochloric acid, sulfuric acid, and nitric acid. Bases are defined as oxides and hydroxides of metals that react with acids to form salts and water. Common strong acids and their ions are listed, as well as common weak acids. The properties, naming, and formula writing of acids and bases are also covered.
Chapter No 1 : Acids, Bases and Buffers
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Lecture 19.1b- Bronsted-Lowry Acids & Bases
Here are the key points about measuring pH:
- pH is a measure of hydrogen ion concentration in a solution on a scale from 0-14.
- A pH below 7 is acidic, above 7 is basic, and 7 is neutral.
- The pH scale is logarithmic, so each unit change in pH represents a 10-fold change in [H+].
- Common indicators like litmus paper, phenolphthalein, and universal indicator can be used to estimate pH based on their color changes.
- pH meters provide a precise numerical measurement of pH by measuring voltage.
So in summary, pH is a quantitative measure of acidity or basicity that can be estimated qualitatively with indicators
Oxides
This document discusses different types of oxides based on their reactions with water and acids or bases. It defines acidic, basic, amphoteric, and neutral oxides. Acidic oxides react with water to form acids, while basic oxides react with acids to form salts and water. Amphoteric oxides can behave as either acidic or basic oxides depending on the reaction. Neutral oxides show no acidic or basic properties and are insoluble in water. The document provides examples of common oxides that fall into each category and an decision tree for classifying an unknown oxide based on its solubility properties.
Acids And Bases
This document provides information about acids and bases, including their properties and reactions. It defines acids as substances that produce hydrogen ions in aqueous solution, and bases as metal oxides or hydroxides. Strong acids are fully ionized in water, while weak acids are only partially ionized. The strength of an acid does not relate to its concentration. Common uses of acids include battery electrolytes, rust removal, and food preservation.
Acids, bases and salts IGCSE Chemistry
This document provides an introduction to acids, bases, and salts for GCSE chemistry students. It discusses key topics like acidity and alkalinity, indicators, the pH scale, types of acids including strong and weak acids, and various methods for making salts through reactions between acids and metals, metal oxides, metal carbonates, metal hydroxides, and ammonia. The document is intended to help students understand and revise these core chemistry concepts in preparation for their exams.
Acid –base reaction
Strong acids and strong bases always react in the same format since the dissociate nearly 100% in water.
Solutions of hydrochloric acid and sodium hydroxide are mixed the reaction occurs as follows:
Weak acids dissociate only slightly in water, and therefore should be left combined and not written as its ions. When weak acids react with strong bases, the H+ from the weak acid is transferred to the OH- from the strong base to form water and a salt. The salt formed, however, will most likely be soluble, and should be written as its respective ions. Remember also, to cancel out any spectator ions.
3.3 Acids and Bases
The pink colour in test tubes #2 and #4 was caused by the basic solution (NaOH) reacting with the phenolphthalein indicator, which turns pink in basic solutions with a pH between 8.2-12.
The colour disappeared in test tube #5 because the acidic solution (HCl) was added, and phenolphthalein is colourless in acidic solutions below pH 8.2.
We could use an acidic solution like HCl to take away the pink colour in test tube #6, as it would neutralize the basic solution and lower the pH below 8.2, making the phenolphthalein colourless again.
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This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
Unit 2, Lesson 2.8 - Acids, Bases, and Salts
Unit 2, Lesson 2.8 - Acids, Bases, and Salts
Lesson Outline:
1. Acids vs. Bases Comparison
2. Neutralization reaction
3. pH scale
4. Salts
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPoints
This document provides an overview of acids and bases according to different theories:
1. Arrhenius theory defines acids as producing hydrogen ions in water and bases as producing hydroxide ions.
2. Brønsted-Lowry theory defines acids as hydrogen ion donors and bases as hydrogen ion acceptors.
3. Lewis theory focuses on electron pair donation and acceptance between reactants.
It also discusses the pH scale, ion product constant of water, and using indicators to determine if a solution is acidic, basic, or neutral.
Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
Acids, bases and salts
This document discusses acids, bases, salts, and indicators. It defines acids as sour substances that produce hydrogen ions in solution and have a pH below 7. Bases are defined as having a pH above 7 and forming hydroxide ions in solution. Examples of common acids and bases are provided. Indicators are substances that change color in acidic versus basic solutions, allowing the pH to be determined. Strong acids and bases fully ionize in solution, while weak ones only partially ionize. Neutralization occurs when an acid and base react to form a salt and water. Salts are neutral compounds composed of acid anions and base cations.
C10 acids, bases and salts
This document provides information on acids, bases, and salts. It defines acids as substances that produce hydrogen ions in water. Examples of strong acids that fully ionize include sulfuric acid and hydrochloric acid, while weak acids only partially ionize, such as ethanoic acid. Bases are metal oxides or hydroxides, and those that dissolve in water producing hydroxide ions are called alkalis like sodium hydroxide. The pH scale measures the hydrogen ion concentration in solutions from 0-14, with lower values being more acidic and higher more alkaline. Common indicators change color at specific pH values to show acidity or alkalinity.
Strength Of Acid And Alkali
Strong acids and bases ionize completely in water, producing high concentrations of hydrogen or hydroxide ions. Weak acids and bases only partially ionize in water, resulting in lower concentrations of ions. Specifically, hydrochloric acid and sodium hydroxide fully dissociate whereas ethanoic acid and ammonia only partially dissociate, making the latter acids and bases weaker. Strong acids and bases have higher pH values and degrees of ionization compared to their weaker counterparts.
Chemistry M2 Acids bases salts
Acids provide H+ ions in water, while bases provide OH- ions. Examples of acids include HCl and H2SO4, while examples of bases include NaOH and KOH. When acids and bases react, they undergo a neutralization reaction producing water and a salt. For example, HCl + NaOH produces H2O + NaCl. Strong acids and bases fully dissociate in water, while weak ones only partially dissociate.
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This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Acids, Bases, and Buffers (1).pdf
This document discusses acids, bases, and buffers. It defines Bronsted-Lowry acids and bases as proton donors and acceptors, respectively. It explains that water can act as both an acid and a base depending on the substance it is combined with. The document also defines pH and pOH as measures of hydronium and hydroxide ion concentration. Finally, it states that buffer solutions resist changes in pH through mixtures of weak acids/bases and their conjugates that do not neutralize each other.
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,
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This document provides an overview of acids and bases according to the Arrhenius and Brønsted-Lowry theories. It discusses how acids and bases were originally categorized based on their physical properties. The Arrhenius theory defined acids as substances that produce H+ ions in water and bases as substances that produce OH- ions. It also explains that H+ ions actually exist as hydronium ions (H3O+) in water. The Brønsted-Lowry theory expanded this to define acids as proton donors and bases as proton acceptors. Other topics covered include strong vs. weak acids/bases, the autoionization of water, and the pH scale.
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This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
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The document discusses acids, bases, and alkalis. It defines them, provides examples, and explains their properties and uses. Acids donate H+ ions in water, bases accept H+ ions and alkalis dissolve in water to form hydroxide ions. Properties of acids include sour taste and turning litmus red, while alkalis have a bitter taste and turn litmus blue. Common acids and bases are used in products like cleaners, soaps, batteries, and more.
Acid bases and salts (1)
The document discusses acids, bases, and salts. It defines acids as substances that form hydrogen ions in water, such as hydrochloric acid, sulfuric acid, and nitric acid. Bases are defined as oxides and hydroxides of metals that react with acids to form salts and water. Common strong acids and their ions are listed, as well as common weak acids. The properties, naming, and formula writing of acids and bases are also covered.
Chapter No 1 : Acids, Bases and Buffers
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
Lecture 19.1b- Bronsted-Lowry Acids & Bases
Here are the key points about measuring pH:
- pH is a measure of hydrogen ion concentration in a solution on a scale from 0-14.
- A pH below 7 is acidic, above 7 is basic, and 7 is neutral.
- The pH scale is logarithmic, so each unit change in pH represents a 10-fold change in [H+].
- Common indicators like litmus paper, phenolphthalein, and universal indicator can be used to estimate pH based on their color changes.
- pH meters provide a precise numerical measurement of pH by measuring voltage.
So in summary, pH is a quantitative measure of acidity or basicity that can be estimated qualitatively with indicators
Oxides
This document discusses different types of oxides based on their reactions with water and acids or bases. It defines acidic, basic, amphoteric, and neutral oxides. Acidic oxides react with water to form acids, while basic oxides react with acids to form salts and water. Amphoteric oxides can behave as either acidic or basic oxides depending on the reaction. Neutral oxides show no acidic or basic properties and are insoluble in water. The document provides examples of common oxides that fall into each category and an decision tree for classifying an unknown oxide based on its solubility properties.
Acids And Bases
This document provides information about acids and bases, including their properties and reactions. It defines acids as substances that produce hydrogen ions in aqueous solution, and bases as metal oxides or hydroxides. Strong acids are fully ionized in water, while weak acids are only partially ionized. The strength of an acid does not relate to its concentration. Common uses of acids include battery electrolytes, rust removal, and food preservation.
Acids, bases and salts IGCSE Chemistry
This document provides an introduction to acids, bases, and salts for GCSE chemistry students. It discusses key topics like acidity and alkalinity, indicators, the pH scale, types of acids including strong and weak acids, and various methods for making salts through reactions between acids and metals, metal oxides, metal carbonates, metal hydroxides, and ammonia. The document is intended to help students understand and revise these core chemistry concepts in preparation for their exams.
Acid –base reaction
Strong acids and strong bases always react in the same format since the dissociate nearly 100% in water.
Solutions of hydrochloric acid and sodium hydroxide are mixed the reaction occurs as follows:
Weak acids dissociate only slightly in water, and therefore should be left combined and not written as its ions. When weak acids react with strong bases, the H+ from the weak acid is transferred to the OH- from the strong base to form water and a salt. The salt formed, however, will most likely be soluble, and should be written as its respective ions. Remember also, to cancel out any spectator ions.
3.3 Acids and Bases
The pink colour in test tubes #2 and #4 was caused by the basic solution (NaOH) reacting with the phenolphthalein indicator, which turns pink in basic solutions with a pH between 8.2-12.
The colour disappeared in test tube #5 because the acidic solution (HCl) was added, and phenolphthalein is colourless in acidic solutions below pH 8.2.
We could use an acidic solution like HCl to take away the pink colour in test tube #6, as it would neutralize the basic solution and lower the pH below 8.2, making the phenolphthalein colourless again.
TOPIC 8 : Acids and Bases
This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
Unit 2, Lesson 2.8 - Acids, Bases, and Salts
Unit 2, Lesson 2.8 - Acids, Bases, and Salts
Lesson Outline:
1. Acids vs. Bases Comparison
2. Neutralization reaction
3. pH scale
4. Salts
Chemistry - Chp 19 - Acids, Bases, and Salt - PowerPoints
This document provides an overview of acids and bases according to different theories:
1. Arrhenius theory defines acids as producing hydrogen ions in water and bases as producing hydroxide ions.
2. Brønsted-Lowry theory defines acids as hydrogen ion donors and bases as hydrogen ion acceptors.
3. Lewis theory focuses on electron pair donation and acceptance between reactants.
It also discusses the pH scale, ion product constant of water, and using indicators to determine if a solution is acidic, basic, or neutral.
Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
Acids, bases and salts
This document discusses acids, bases, salts, and indicators. It defines acids as sour substances that produce hydrogen ions in solution and have a pH below 7. Bases are defined as having a pH above 7 and forming hydroxide ions in solution. Examples of common acids and bases are provided. Indicators are substances that change color in acidic versus basic solutions, allowing the pH to be determined. Strong acids and bases fully ionize in solution, while weak ones only partially ionize. Neutralization occurs when an acid and base react to form a salt and water. Salts are neutral compounds composed of acid anions and base cations.
C10 acids, bases and salts
This document provides information on acids, bases, and salts. It defines acids as substances that produce hydrogen ions in water. Examples of strong acids that fully ionize include sulfuric acid and hydrochloric acid, while weak acids only partially ionize, such as ethanoic acid. Bases are metal oxides or hydroxides, and those that dissolve in water producing hydroxide ions are called alkalis like sodium hydroxide. The pH scale measures the hydrogen ion concentration in solutions from 0-14, with lower values being more acidic and higher more alkaline. Common indicators change color at specific pH values to show acidity or alkalinity.
Strength Of Acid And Alkali
Strong acids and bases ionize completely in water, producing high concentrations of hydrogen or hydroxide ions. Weak acids and bases only partially ionize in water, resulting in lower concentrations of ions. Specifically, hydrochloric acid and sodium hydroxide fully dissociate whereas ethanoic acid and ammonia only partially dissociate, making the latter acids and bases weaker. Strong acids and bases have higher pH values and degrees of ionization compared to their weaker counterparts.
Chemistry M2 Acids bases salts
Acids provide H+ ions in water, while bases provide OH- ions. Examples of acids include HCl and H2SO4, while examples of bases include NaOH and KOH. When acids and bases react, they undergo a neutralization reaction producing water and a salt. For example, HCl + NaOH produces H2O + NaCl. Strong acids and bases fully dissociate in water, while weak ones only partially dissociate.
Chapter No 1 : Acids, Bases and Buffers
This is chapter No 1 of Pharmaceutical Chemistry - I for Diploma in Pharmacy (D. Pharmacy)
Details notes for Diploma in Pharmacy (D.Pharmacy) Students.
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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.
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This document provides an overview of acids, bases, and pH. It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. Acids are substances that produce H+ ions in water or donate protons in reactions, while bases produce OH- ions or accept protons. The document also discusses acid and base strength, pH, self-ionization of water, and examples of calculating pH from H+ concentration and vice versa. Common acids, bases, and pH indicators are listed.
B sc_I_General chemistry U-II Ionic equilibria in aqueous solution
This document provides an overview of acids, bases, and pH. It defines acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories. Acids are substances that produce H+ ions in water or donate protons in reactions, while bases produce OH- ions or accept protons. The document also discusses acid and base strength, pH, self-ionization of water, and using pH to calculate hydrogen or hydroxide ion concentrations. Common examples like acids in orange juice and blood pH are provided.
Acids, bases and salt
This document defines acids, bases, and salts according to three theories:
1) Arrhenius defines acids as substances that yield hydrogen ions in water and bases as substances that yield hydroxide ions in water. Neutralization produces salt and water.
2) Bronsted-Lowry defines acids as proton donors and bases as proton acceptors. Neutralization involves the transfer of a proton from an acid to a base.
3) Lewis defines acids as electron pair acceptors and bases as electron pair donors. Neutralization involves the sharing of an electron pair between an acid and base.
Acids, bases, & salts
This document discusses acids, bases, and salts. It defines acids as compounds that produce hydrogen ions (H+) in water, have a pH below 7, and react with metals. Bases are defined as compounds that produce hydroxide ions (OH-) in water and have a pH above 7. Salts are neutral compounds formed by the reaction of acids and bases. Common acids and bases are listed, along with their uses. The pH scale and indicators are also explained.
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.
Acid base and acid base titration
This chapter discusses acids and bases according to the Arrhenius and Brønsted-Lowry definitions. The Arrhenius definition states that acids are substances that produce hydronium ions (H3O+) in water and bases produce hydroxide ions (OH-). Brønsted-Lowry defines acids as proton donors and bases as proton acceptors. Both definitions are discussed along with their advantages and limitations. Strong and weak acids/bases are compared based on their extent of ionization in water. Neutralization reactions between acids and bases are outlined. Conjugate acid-base pairs are introduced in the context of Brønsted-Lowry acid-base reactions. Certain substances, called
Apchemunit14presentationpart2 120227191453-phpapp02
This document discusses various properties of bases and salts. It explains that Group 1 and 2 hydroxides are strong bases, while NaOH and KOH are common laboratory reagents. Weak bases produce hydroxide ions when dissolved in water through reactions. Salts can behave as acids or bases depending on whether their ions are from conjugate acid-base pairs. The pH of solutions can be predicted based on comparing Ka and Kb values of constituent ions. Acid-base behavior is also influenced by structural factors like electronegativity and number of oxygen atoms.
Acids and bases and salts
The document discusses the key properties and reactions of acids and bases. It defines acids as substances with a pH less than 7 that produce hydrogen ions in water. Bases are defined as having a pH greater than 7 and producing hydroxide ions in water. The document also discusses acid-base indicators, the pH scale, and neutralization reactions between acids and bases that produce salts and water.
Acids andbases cheat sheet
This document provides an overview of key concepts related to acids and bases in chemistry. It defines different types of acids and bases according to several theories. It also discusses properties of acids and bases such as tastes and colors of litmus paper. Strong and weak acids and bases are compared. Buffers are described as mixtures of weak acids and bases that resist pH change. The pH scale is introduced and methods for solving pH problems are outlined, including using Ka, Kb, and Kw values and ICE charts. Acid-base properties of salts and the principles of titrations are also summarized.
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B sc i chemistry i u ii ionic equilibria in aqueous solution a
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Apchemunit14presentationpart2 120227191453-phpapp02
Apchemunit14presentationpart2 120227191453-phpapp02
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Moles and Concentration Calculations Course
This course covers the fundamentals of chemistry including atomic and molecular masses, calculating relative atomic mass using a mass spectrometer, formula mass and relative molecular mass, amount of substances, Avogadro's constant, chemical formulas and equations, empirical and molecular formulas, balancing chemical equations, mole calculations, stoichiometry, solutions and concentrations, titration experiments, gas volume calculations, and exercises to practice these concepts. The goal is to learn essential chemistry topics through this comprehensive high school or introductory college chemistry course.
Writing in Science and Research
This 4-section course aims to help undergraduate and graduate science students at any stage of their research to write effectively. The course covers starting a research project, collecting and writing up data, using writing tools to report results, and editing drafts.
Principles of Polymer Chemistry
This document discusses different types of polymers including natural, synthetic, and semi-synthetic polymers. It describes methods of polymerization such as step-growth, chain-growth, ring-opening, and coordination polymerization. Specific polymers are also mentioned including polyesters, polycarbonates, polyamides, polyurethane, nylon 6, polyethylene oxide, and polypropylene oxide. The document provides an overview of polymer chemistry concepts like molecular weight calculation, crystalline structures, glass transition and melt temperatures, and different polymerization reactions.
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Vitamin D
This document discusses vitamin D, including what it is, how the body processes and activates it, its functions, sources, and requirements. Vitamin D is a fat-soluble vitamin synthesized in the skin upon exposure to sunlight and found in some foods. It is activated through two hydroxylation steps in the liver and kidneys. Vitamin D promotes calcium absorption and bone mineralization and supports immune function. While sunlight is the major source, many factors impact skin synthesis, so dietary sources and supplements are also important to meet daily requirements.
Naming compounds and Balancing chemical equations using oxidation numbers
1) The document discusses naming compounds and balancing chemical equations using oxidation numbers. It provides examples of naming metal and non-metal compounds as well as oxide compounds.
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Calorimeter and enthalpy measurements
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This document summarizes different types of enthalpy changes in chemical reactions. It defines exothermic reactions as releasing energy to the surroundings and endothermic reactions as absorbing energy from the surroundings. Enthalpy change is the energy exchange between a reaction and its surroundings at constant pressure. The document explains how to calculate enthalpy change and represents reaction pathways using enthalpy profile diagrams to show enthalpy changes for exothermic and endothermic reactions. It also defines standard enthalpy changes of combustion, neutralization, solution, and hydration of salts.
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快速办理(UAM毕业证书)马德里自治大学毕业证学位证一模一样
学校原件一模一样【微信：741003700 】《(UAM毕业证书)马德里自治大学毕业证学位证》【微信：741003700 】学位证，留信认证（真实可查，永久存档）原件一模一样纸张工艺/offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
本公司拥有海外各大学样板无数，能完美还原。
1:1完美还原海外各大学毕业材料上的工艺：水印，阴影底纹，钢印LOGO烫金烫银，LOGO烫金烫银复合重叠。文字图案浮雕、激光镭射、紫外荧光、温感、复印防伪等防伪工艺。材料咨询办理、认证咨询办理请加学历顾问Q/微741003700
【主营项目】
一.毕业证【q微741003700】成绩单、使馆认证、教育部认证、雅思托福成绩单、学生卡等！
二.真实使馆公证(即留学回国人员证明,不成功不收费)
三.真实教育部学历学位认证（教育部存档！教育部留服网站永久可查）
四.办理各国各大学文凭(一对一专业服务,可全程监控跟踪进度)
如果您处于以下几种情况：
◇在校期间，因各种原因未能顺利毕业……拿不到官方毕业证【q/微741003700】
◇面对父母的压力，希望尽快拿到；
◇不清楚认证流程以及材料该如何准备；
◇回国时间很长，忘记办理；
◇回国马上就要找工作，办给用人单位看；
◇企事业单位必须要求办理的
◇需要报考公务员、购买免税车、落转户口
◇申请留学生创业基金
留信网认证的作用:
1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
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MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...
MICROBIAL INTERACTION PPT/ MICROBIAL INTERACTION AND THEIR TYPES // PLANT MIC...ABHISHEK SONI NIMT INSTITUTE OF MEDICAL AND PARAMEDCIAL SCIENCES , GOVT PG COLLEGE NOIDA
Microbial interaction
Microorganisms interacts with each other and can be physically associated with another organisms in a variety of ways.
One organism can be located on the surface of another organism as an ectobiont or located within another organism as endobiont.
Microbial interaction may be positive such as mutualism, proto-cooperation, commensalism or may be negative such as parasitism, predation or competition
Types of microbial interaction
Positive interaction: mutualism, proto-cooperation, commensalism
Negative interaction: Ammensalism (antagonism), parasitism, predation, competition
I. Mutualism:
It is defined as the relationship in which each organism in interaction gets benefits from association. It is an obligatory relationship in which mutualist and host are metabolically dependent on each other.
Mutualistic relationship is very specific where one member of association cannot be replaced by another species.
Mutualism require close physical contact between interacting organisms.
Relationship of mutualism allows organisms to exist in habitat that could not occupied by either species alone.
Mutualistic relationship between organisms allows them to act as a single organism.
Examples of mutualism:
i. Lichens:
Lichens are excellent example of mutualism.
They are the association of specific fungi and certain genus of algae. In lichen, fungal partner is called mycobiont and algal partner is called
II. Syntrophism:
It is an association in which the growth of one organism either depends on or improved by the substrate provided by another organism.
In syntrophism both organism in association gets benefits.
Compound A
Utilized by population 1
Compound B
Utilized by population 2
Compound C
utilized by both Population 1+2
Products
In this theoretical example of syntrophism, population 1 is able to utilize and metabolize compound A, forming compound B but cannot metabolize beyond compound B without co-operation of population 2. Population 2is unable to utilize compound A but it can metabolize compound B forming compound C. Then both population 1 and 2 are able to carry out metabolic reaction which leads to formation of end product that neither population could produce alone.
Examples of syntrophism:
i. Methanogenic ecosystem in sludge digester
Methane produced by methanogenic bacteria depends upon interspecies hydrogen transfer by other fermentative bacteria.
Anaerobic fermentative bacteria generate CO2 and H2 utilizing carbohydrates which is then utilized by methanogenic bacteria (Methanobacter) to produce methane.
ii. Lactobacillus arobinosus and Enterococcus faecalis:
In the minimal media, Lactobacillus arobinosus and Enterococcus faecalis are able to grow together but not alone.
The synergistic relationship between E. faecalis and L. arobinosus occurs in which E. faecalis require folic acid
fermented food science of sauerkraut.pptx
This ppt contains the production of a fermented food name - sauerkraut
Gadgets for management of stored product pests_Dr.UPR.pdf
Insectsplayamajorroleinthedeteriorationoffoodgrainscausingbothquantitativeandqualitativelosses
Wellprovedthatnogranariescanbefilledwithgrainswithoutinsectsastheharvestedproducecontainegg(or)larvae(or)pupae(or)adultinsectinthembecauseoffieldcarryoverinfestationwhichcannotbeavoidedindevelopingcountrieslikeIndia
Simpletechnologiesfortimelydetectionofinsectsinthestoredproduceandtherebyplantimelycontrolmeasures
JAMES WEBB STUDY THE MASSIVE BLACK HOLE SEEDS
The pathway(s) to seeding the massive black holes (MBHs) that exist at the heart of galaxies in the present and distant Universe remains an unsolved problem. Here we categorise, describe and quantitatively discuss the formation pathways of both light and heavy seeds. We emphasise that the most recent computational models suggest that rather than a bimodal-like mass spectrum between light and heavy seeds with light at one end and heavy at the other that instead a continuum exists. Light seeds being more ubiquitous and the heavier seeds becoming less and less abundant due the rarer environmental conditions required for their formation. We therefore examine the different mechanisms that give rise to different seed mass spectrums. We show how and why the mechanisms that produce the heaviest seeds are also among the rarest events in the Universe and are hence extremely unlikely to be the seeds for the vast majority of the MBH population. We quantify, within the limits of the current large uncertainties in the seeding processes, the expected number densities of the seed mass spectrum. We argue that light seeds must be at least 103 to 105 times more numerous than heavy seeds to explain the MBH population as a whole. Based on our current understanding of the seed population this makes heavy seeds (Mseed > 103 M⊙) a significantly more likely pathway given that heavy seeds have an abundance pattern than is close to and likely in excess of 10−4 compared to light seeds. Finally, we examine the current state-of-the-art in numerical calculations and recent observations and plot a path forward for near-future advances in both domains.
Anti-Universe And Emergent Gravity and the Dark Universe
Recent theoretical progress indicates that spacetime and gravity emerge together from the entanglement structure of an underlying microscopic theory. These ideas are best understood in Anti-de Sitter space, where they rely on the area law for entanglement entropy. The extension to de Sitter space requires taking into account the entropy and temperature associated with the cosmological horizon. Using insights from string theory, black hole physics and quantum information theory we argue that the positive dark energy leads to a thermal volume law contribution to the entropy that overtakes the area law precisely at the cosmological horizon. Due to the competition between area and volume law entanglement the microscopic de Sitter states do not thermalise at sub-Hubble scales: they exhibit memory effects in the form of an entropy displacement caused by matter. The emergent laws of gravity contain an additional ‘dark’ gravitational force describing the ‘elastic’ response due to the entropy displacement. We derive an estimate of the strength of this extra force in terms of the baryonic mass, Newton’s constant and the Hubble acceleration scale a0 = cH0, and provide evidence for the fact that this additional ‘dark gravity force’ explains the observed phenomena in galaxies and clusters currently attributed to dark matter.
Discovery of An Apparent Red, High-Velocity Type Ia Supernova at 𝐳 = 2.9 wi...
We present the JWST discovery of SN 2023adsy, a transient object located in a host galaxy JADES-GS
+
53.13485
−
27.82088
with a host spectroscopic redshift of
2.903
±
0.007
. The transient was identified in deep James Webb Space Telescope (JWST)/NIRCam imaging from the JWST Advanced Deep Extragalactic Survey (JADES) program. Photometric and spectroscopic followup with NIRCam and NIRSpec, respectively, confirm the redshift and yield UV-NIR light-curve, NIR color, and spectroscopic information all consistent with a Type Ia classification. Despite its classification as a likely SN Ia, SN 2023adsy is both fairly red (
�
(
�
−
�
)
∼
0.9
) despite a host galaxy with low-extinction and has a high Ca II velocity (
19
,
000
±
2
,
000
km/s) compared to the general population of SNe Ia. While these characteristics are consistent with some Ca-rich SNe Ia, particularly SN 2016hnk, SN 2023adsy is intrinsically brighter than the low-
�
Ca-rich population. Although such an object is too red for any low-
�
cosmological sample, we apply a fiducial standardization approach to SN 2023adsy and find that the SN 2023adsy luminosity distance measurement is in excellent agreement (
≲
1
�
) with
Λ
CDM. Therefore unlike low-
�
Ca-rich SNe Ia, SN 2023adsy is standardizable and gives no indication that SN Ia standardized luminosities change significantly with redshift. A larger sample of distant SNe Ia is required to determine if SN Ia population characteristics at high-
�
truly diverge from their low-
�
counterparts, and to confirm that standardized luminosities nevertheless remain constant with redshift.
Pests of Storage_Identification_Dr.UPR.pdf
InIndia-post-harvestlosses-unscientificstorage,insects,rodents,micro-organismsetc.,accountforabout10percentoftotalfoodgrains
Graininfestation
Directdamage
Indirectly
•theexuviae,skin,deadinsects
•theirexcretawhichmakefoodunfitforhumanconsumption
About600speciesofinsectshavebeenassociatedwithstoredgrainproducts
100speciesofinsectpestsofstoredproductscauseeconomiclosses
在线办理(salfor毕业证书)索尔福德大学毕业证毕业完成信一模一样
学校原件一模一样【微信：741003700 】《(salfor毕业证书)索尔福德大学毕业证》【微信：741003700 】学位证，留信认证（真实可查，永久存档）原件一模一样纸张工艺/offer、雅思、外壳等材料/诚信可靠,可直接看成品样本，帮您解决无法毕业带来的各种难题！外壳，原版制作，诚信可靠，可直接看成品样本。行业标杆！精益求精，诚心合作，真诚制作！多年品质 ,按需精细制作，24小时接单,全套进口原装设备。十五年致力于帮助留学生解决难题，包您满意。
本公司拥有海外各大学样板无数，能完美还原。
1:1完美还原海外各大学毕业材料上的工艺：水印，阴影底纹，钢印LOGO烫金烫银，LOGO烫金烫银复合重叠。文字图案浮雕、激光镭射、紫外荧光、温感、复印防伪等防伪工艺。材料咨询办理、认证咨询办理请加学历顾问Q/微741003700
【主营项目】
一.毕业证【q微741003700】成绩单、使馆认证、教育部认证、雅思托福成绩单、学生卡等！
二.真实使馆公证(即留学回国人员证明,不成功不收费)
三.真实教育部学历学位认证（教育部存档！教育部留服网站永久可查）
四.办理各国各大学文凭(一对一专业服务,可全程监控跟踪进度)
如果您处于以下几种情况：
◇在校期间，因各种原因未能顺利毕业……拿不到官方毕业证【q/微741003700】
◇面对父母的压力，希望尽快拿到；
◇不清楚认证流程以及材料该如何准备；
◇回国时间很长，忘记办理；
◇回国马上就要找工作，办给用人单位看；
◇企事业单位必须要求办理的
◇需要报考公务员、购买免税车、落转户口
◇申请留学生创业基金
留信网认证的作用:
1:该专业认证可证明留学生真实身份
2:同时对留学生所学专业登记给予评定
3:国家专业人才认证中心颁发入库证书
4:这个认证书并且可以归档倒地方
5:凡事获得留信网入网的信息将会逐步更新到个人身份内，将在公安局网内查询个人身份证信息后，同步读取人才网入库信息
6:个人职称评审加20分
7:个人信誉贷款加10分
8:在国家人才网主办的国家网络招聘大会中纳入资料，供国家高端企业选择人才
8.Isolation of pure cultures and preservation of cultures.pdf
Isolation of pure culture, its various method.
Compexometric titration/Chelatorphy titration/chelating titration
Classification
Metal ion ion indicators
Masking and demasking reagents
Estimation of Magnisium sulphate
Calcium gluconate
Complexometric Titration/ chelatometry titration/chelating titration, introduction, Types-
1.Direct Titration
2.Back Titration
3.Replacement Titration
4.Indirect Titration
Masking agent, Demasking agents
formation of complex
comparition between masking and demasking agents,
Indicators/Metal ion indicators/ Metallochromic indicators/pM indicators,
Visual Technique,PM indicators (metallochromic), Indicators of pH, Redox Indicators
Instrumental Techniques-Photometry
Potentiometry
Miscellaneous methods.
Complex titration with EDTA.
The debris of the ‘last major merger’ is dynamically young
The Milky Way’s (MW) inner stellar halo contains an [Fe/H]-rich component with highly eccentric orbits, often referred to as the
‘last major merger.’ Hypotheses for the origin of this component include Gaia-Sausage/Enceladus (GSE), where the progenitor
collided with the MW proto-disc 8–11 Gyr ago, and the Virgo Radial Merger (VRM), where the progenitor collided with the
MW disc within the last 3 Gyr. These two scenarios make different predictions about observable structure in local phase space,
because the morphology of debris depends on how long it has had to phase mix. The recently identified phase-space folds in Gaia
DR3 have positive caustic velocities, making them fundamentally different than the phase-mixed chevrons found in simulations
at late times. Roughly 20 per cent of the stars in the prograde local stellar halo are associated with the observed caustics. Based
on a simple phase-mixing model, the observed number of caustics are consistent with a merger that occurred 1–2 Gyr ago.
We also compare the observed phase-space distribution to FIRE-2 Latte simulations of GSE-like mergers, using a quantitative
measurement of phase mixing (2D causticality). The observed local phase-space distribution best matches the simulated data
1–2 Gyr after collision, and certainly not later than 3 Gyr. This is further evidence that the progenitor of the ‘last major merger’
did not collide with the MW proto-disc at early times, as is thought for the GSE, but instead collided with the MW disc within
the last few Gyr, consistent with the body of work surrounding the VRM.
Mending Clothing to Support Sustainable Fashion_CIMaR 2024.pdf
Ozturkcan, S., Berndt, A., & Angelakis, A. (2024). Mending clothing to support sustainable fashion. Presented at the 31st Annual Conference by the Consortium for International Marketing Research (CIMaR), 10-13 Jun 2024, University of Gävle, Sweden.
Candidate young stellar objects in the S-cluster: Kinematic analysis of a sub...
Context. The observation of several L-band emission sources in the S cluster has led to a rich discussion of their nature. However, a definitive answer to the classification of the dusty objects requires an explanation for the detection of compact Doppler-shifted Brγ emission. The ionized hydrogen in combination with the observation of mid-infrared L-band continuum emission suggests that most of these sources are embedded in a dusty envelope. These embedded sources are part of the S-cluster, and their relationship to the S-stars is still under debate. To date, the question of the origin of these two populations has been vague, although all explanations favor migration processes for the individual cluster members. Aims. This work revisits the S-cluster and its dusty members orbiting the supermassive black hole SgrA* on bound Keplerian orbits from a kinematic perspective. The aim is to explore the Keplerian parameters for patterns that might imply a nonrandom distribution of the sample. Additionally, various analytical aspects are considered to address the nature of the dusty sources. Methods. Based on the photometric analysis, we estimated the individual H−K and K−L colors for the source sample and compared the results to known cluster members. The classification revealed a noticeable contrast between the S-stars and the dusty sources. To fit the flux-density distribution, we utilized the radiative transfer code HYPERION and implemented a young stellar object Class I model. We obtained the position angle from the Keplerian fit results; additionally, we analyzed the distribution of the inclinations and the longitudes of the ascending node. Results. The colors of the dusty sources suggest a stellar nature consistent with the spectral energy distribution in the near and midinfrared domains. Furthermore, the evaporation timescales of dusty and gaseous clumps in the vicinity of SgrA* are much shorter ( 2yr) than the epochs covered by the observations (≈15yr). In addition to the strong evidence for the stellar classification of the D-sources, we also find a clear disk-like pattern following the arrangements of S-stars proposed in the literature. Furthermore, we find a global intrinsic inclination for all dusty sources of 60 ± 20◦, implying a common formation process. Conclusions. The pattern of the dusty sources manifested in the distribution of the position angles, inclinations, and longitudes of the ascending node strongly suggests two different scenarios: the main-sequence stars and the dusty stellar S-cluster sources share a common formation history or migrated with a similar formation channel in the vicinity of SgrA*. Alternatively, the gravitational influence of SgrA* in combination with a massive perturber, such as a putative intermediate mass black hole in the IRS 13 cluster, forces the dusty objects and S-stars to follow a particular orbital arrangement. Key words. stars: black holes– stars: formation– Galaxy: center– galaxies: star formation
The cost of acquiring information by natural selection
This is a short talk that I gave at the Banff International Research Station workshop on Modeling and Theory in Population Biology. The idea is to try to understand how the burden of natural selection relates to the amount of information that selection puts into the genome.
It's based on the first part of this research paper:
The cost of information acquisition by natural selection
Ryan Seamus McGee, Olivia Kosterlitz, Artem Kaznatcheev, Benjamin Kerr, Carl T. Bergstrom
bioRxiv 2022.07.02.498577; doi: https://doi.org/10.1101/2022.07.02.498577
Describing and Interpreting an Immersive Learning Case with the Immersion Cub...
Current descriptions of immersive learning cases are often difficult or impossible to compare. This is due to a myriad of different options on what details to include, which aspects are relevant, and on the descriptive approaches employed. Also, these aspects often combine very specific details with more general guidelines or indicate intents and rationales without clarifying their implementation. In this paper we provide a method to describe immersive learning cases that is structured to enable comparisons, yet flexible enough to allow researchers and practitioners to decide which aspects to include. This method leverages a taxonomy that classifies educational aspects at three levels (uses, practices, and strategies) and then utilizes two frameworks, the Immersive Learning Brain and the Immersion Cube, to enable a structured description and interpretation of immersive learning cases. The method is then demonstrated on a published immersive learning case on training for wind turbine maintenance using virtual reality. Applying the method results in a structured artifact, the Immersive Learning Case Sheet, that tags the case with its proximal uses, practices, and strategies, and refines the free text case description to ensure that matching details are included. This contribution is thus a case description method in support of future comparative research of immersive learning cases. We then discuss how the resulting description and interpretation can be leveraged to change immersion learning cases, by enriching them (considering low-effort changes or additions) or innovating (exploring more challenging avenues of transformation). The method holds significant promise to support better-grounded research in immersive learning.
(June 12, 2024) Webinar: Development of PET theranostics targeting the molecu...
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Targeting Hsp90 and its pathogen Orthologs with Tethered Inhibitors as a Diagnostic and Therapeutic Strategy for cancer and infectious diseases with Dr. Timothy Haystead.Randomised Optimisation Algorithms in DAPHNE
Slides from talk:
Aleš Zamuda: Randomised Optimisation Algorithms in DAPHNE .
Austrian-Slovenian HPC Meeting 2024 – ASHPC24, Seeblickhotel Grundlsee in Austria, 10–13 June 2024
https://ashpc.eu/
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Acid and bases
- 1. Acid and bases by Dr. Rania S. Seoudi 1
- 2. Acid and bases Brønsted acid: A substance capable of donating a proton. Brønsted base: A substance capable of accepting a proton. Conjugate acid-base pair: an acid and its conjugate base or a base and its conjugate acid. 2
- 3. Acid –base properties of water - Water is a poor conductor - Ionize in a small extent: 3
- 4. The ion product of water 4
- 5. 5
- 6. pH- A measure of acidity - H+ and OH- ions in aqueous solution are frequently very small numbers to work with. Instead we work with pH: - pH is simple way to express hydrogen ion concentration, and acidic and basic solution can be distinguish by their pHs values: - If pH value is given and hydrogen ion concentration is needed to be calculated: - 6
- 7. - Again for ion – product constant of water at 25oC: 7
- 8. 8
- 9. Strength of acids and bases - Strong acids are strong electrolytes that, for practical purposes, are assumed to ionize completely in water. - Most of strong acids are inorganic acids such as: hydrochloric acid (HCl), nitric acid (HNO3), perchloric acid (HClO4), and sulfuric acid (H2SO4): - Most acids are weak acids (ionize to limit extent). - Weak acids contain nonionized acid moleucles such as: hydrofluoric acid (HF), acetic acid (CH3COOH), and the ammonium ion (NH+ 4). 9
- 10. - Conjugate acid-base pairs have the following properties: 1. If an acid is strong, its conjugate base has no measurable strength. Thus, the Cl2 ion, which is the conjugate base of the strong acid HCl, is an extremely weak base. 2. H3O+ is the strongest acid that can exist in aqueous solution. Acids stronger than H3O+ react with water to produce H3O+ and their conjugate bases. For weak acids than H3O+ 1. The OH- ion is the strongest base that can exist in aqueous solution. Bases stronger than OH- react with water to produce OH- and their conjugate acids. 10
- 11. Weak acids and acid ionization constants - The vast majority of acids are weak acids. - Consider the weak monprotic acid HA - The equilibrium expression for this ionization is 11
- 12. - If we know pH of weak acid and initial concentration we can know Ka - Example: calculate pH od 0.50M HF solution at 25oC (Ka=7.1x10-4): So, 12
- 13. In summary, the main steps for solving weak acid ionization problems are: 1. Identify the major species that can affect the pH of the solution. In most cases we can ignore the ionization of water. We omit the hydroxide ion because its concentration is determined by that of the H+ ion. 2. Express the equilibrium concentrations of these species in terms of the initial concentration of the acid and a single unknown x, which represents the change in concentration. 3. Write the weak acid ionization and express the ionization constant Ka in terms of the equilibrium concentrations of H+, the conjugate base, and the unionized acid and solve x. 4. Having solved for x, calculate the equilibrium concentrations of all species and/or the pH of the solution. 13