Acids and Bases
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Acids and bases can be defined in three ways: Arrhenius acids release H+ ions in water, Bronsted-Lowry acids donate protons, and Lewis acids accept electron pairs. Similarly, Arrhenius bases release OH- ions in water, Bronsted-Lowry bases accept protons, and Lewis bases donate electron pairs. A neutralization reaction occurs when an acid and base combine to form water, and the pH scale ranges from 0 to 14 with values below 7 being acidic and above 7 being basic.
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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.
Properties of acids; bases
Acids have a sour taste, are electrolytes, turn indicators red, and have a pH less than 7. They donate protons and can neutralize bases to form salts and water. Bases have a bitter taste, are electrolytes, turn indicators blue or yellow, and have a pH greater than 7. They accept protons and can neutralize acids to form salts and water. Common acids include nitric acid, hydrochloric acid, acetic acid, sulfuric acid, and phosphoric acid. Common bases include lithium hydroxide, sodium hydroxide, potassium hydroxide, magnesium hydroxide, and calcium hydroxide.
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This document provides an overview of key concepts about acids and bases from sections 18.1 through 18.4. It introduces the Arrhenius, Brønsted-Lowry, and Lewis models of acids and bases. It describes the properties of acids and bases and how pH and pKa/pKb values relate to acid and base strength. Neutralization reactions between acids and bases are discussed along with acid-base titrations and buffered solutions.
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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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- Hard acids prefer to interact with hard bases that have donor atoms like N, O, F, while soft acids prefer soft bases with donor atoms like P, S, Se, Cl, Br.
- Examples of hard acids are H+, Li+, Na+, K+ and hard bases are OH-, F-. Soft acids include Cu+, Ag+, Au+ and soft bases include S2-, Se2-.
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Example of acids and bases
Acids bases by By MUHAMMAD FAHAD ANSARI 12 IEEM 14
This document discusses acids and bases. It defines acids as substances that release H+ ions in solution, donate protons, or accept electron pairs. Bases are defined as substances that release OH- ions in solution, accept protons, or donate electron pairs. A neutralization reaction occurs when an acid and base combine to form water. The pH scale measures how acidic or basic a substance is on a scale from 0-14. Acids have a sour taste, turn litmus paper red, and react with bases. Bases have a slippery feeling, turn litmus paper blue, and react with acids. Common indicators, like litmus paper, change color in acids and bases.
Chapter 18.3 : Equilibria of Acids, Bases, and Salts
The document discusses acid-base equilibria, including acid ionization constants, the ionization of acetic acid as a weak acid, and buffer solutions. It explains that buffer solutions contain a weak acid and salt of the weak acid and can resist changes in pH when small amounts of acid or base are added. The document also covers the ionization of water, hydrolysis of salts, and how hydrolysis can affect the pH of salt solutions depending on whether the salt contains ions from strong vs. weak acids and bases.
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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.
Properties of acids; bases
Acids have a sour taste, are electrolytes, turn indicators red, and have a pH less than 7. They donate protons and can neutralize bases to form salts and water. Bases have a bitter taste, are electrolytes, turn indicators blue or yellow, and have a pH greater than 7. They accept protons and can neutralize acids to form salts and water. Common acids include nitric acid, hydrochloric acid, acetic acid, sulfuric acid, and phosphoric acid. Common bases include lithium hydroxide, sodium hydroxide, potassium hydroxide, magnesium hydroxide, and calcium hydroxide.
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This document provides an overview of key concepts about acids and bases from sections 18.1 through 18.4. It introduces the Arrhenius, Brønsted-Lowry, and Lewis models of acids and bases. It describes the properties of acids and bases and how pH and pKa/pKb values relate to acid and base strength. Neutralization reactions between acids and bases are discussed along with acid-base titrations and buffered solutions.
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Ionic Equilibria
1. The document discusses ionic equilibria, including acids and bases, and how to identify strong and weak acids/bases. It also discusses calculating pH and pOH values.
2. It explains how to determine if a salt is neutral, acidic, or basic based on whether the cation or anion comes from a strong or weak acid/base.
3. For sparingly soluble salts, it discusses using Ksp expressions and concentrations to determine if a precipitate will form from mixing solutions of ions.
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The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
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This document discusses acid-base theories and reactions. It begins with a brief history of acids and bases, noting they were originally defined based on their sour taste. It then focuses on three main acid-base theories:
1) Arrhenius theory defines acids as producing H+ ions in water and bases as producing OH- ions.
2) Brønsted-Lowry theory provides a more general definition, with acids as proton donors and bases as proton acceptors that form conjugate acid-base pairs.
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This document contains 20 questions and answers about acids, bases and salts. Some key points:
- Common household substances with pH >7 include eggs, baking soda and bleach. Substances with pH <7 include coffee, oranges and vinegar. Pure water has pH=7.
- A base is a substance that can accept protons or donate electron pairs. All alkalies are bases but not all bases are alkalies since alkalies must be water-soluble.
- Bronsted-Lowry bases accept protons, as in the reaction of HCl dissolving in water where H2O acts as the base. This theory applies to all protic solvents.
pH meassurement
The document defines pH and describes how it is measured. It begins by explaining that pH was introduced in 1909 by Sorensen to express the concentration of hydrogen ions (H+) in a solution. It then defines pH mathematically as the negative logarithm of the H+ concentration. The rest of the document discusses:
- How pH is measured using indicators and pH meters
- How the pH scale was developed based on experimental measurements of H+ concentrations
- Examples of calculating pH from H+ concentration and calculating H- concentration from pH
- Applications of pH including in nature, soil, and acid rain
Acidos y bases definiciones, ejemplos, escalas de acidez
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2. Acid strength is measured by an equilibrium constant (Ka) or pKa value, with a lower pKa indicating a stronger acid. Factors that increase acid strength include the electronegativity, size, inductive effects, and resonance stabilization of the conjugate base.
3. Common organic acids used in reactions include acetic acid and p-toluenesulfonic acid. Lewis acids, such as BF3 and AlCl3, are electron pair acceptors and react
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This document provides an overview of acids and bases including:
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- How acids and bases react in water, forming conjugates
- Factors that influence acid and base strength such as polarity, resonance, and electronegativity
- Calculations involving acid and base dissociation constants (Ka and Kb) to determine pH
pH
The document discusses pH, which is a measure of how acidic or basic a solution is. pH is defined as the negative logarithm of the hydrogen ion concentration and is measured on a scale from 0 to 14. A pH below 7 is acidic, above 7 is basic, and 7 is neutral. The document outlines how pH is measured, factors that affect pH in nature and living systems, and provides examples of pH levels in common foods and water quality standards.
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Water and p h
Water makes up 65-70% of the human body. It has unique properties like high melting and boiling points due to hydrogen bonding between water molecules. The bent shape of water molecules gives them a partial positive and negative charge, allowing them to form hydrogen bonds with other water molecules. These bonds contribute to water's high heat capacity and heat of vaporization. Water's pH measures the concentration of hydronium ions, with values below 7 indicating acidity and above 7 indicating alkalinity. pH is important in biological and chemical systems and can be measured using indicators, meters, and the Henderson-Hasselbalch equation.
pH indicator
The document defines pH as the negative logarithm of the hydrogen ion (H+) activity in a solution, with the pH scale ranging from 0 to 14. The hydrogen ions determine if a solution is acidic, alkaline, or neutral - if the hydrogen ion content is measured, the acidity or alkalinity can be determined. Water molecules dissociate into hydrogen and hydroxide ions through autoionization, affecting pH. pH indicators change color depending on the pH of a solution, allowing determination of acidity or alkalinity.
Bt 202 aug 12 2011 ppt1997-2004
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pH by KK SAHU sir
Introduction
History
Acid & Base
Ionization of water
Definitions of pH
(1) Mathematical Definition
(2) pH
(3) pOH
Buffer solution
(1) Types
(2) Buffer action
(3) Biological buffer systems
Henderson – Hasselbalch Equation
Measurement of pH
(1) pH Scale
(2) pH indicators
(3) pH meter
pH in human body and nature
Importance
Conclusion
Reference
UNIT 5TH - pH, buffers and Isotonic solutions
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(electrometric and calorimetric), applications of buffers, buffer equation, buffer capacity,
buffers in pharmaceutical and biological systems, buffered isotonic solutions
Intermolecular forces
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Intermolecular Forces and Solubility
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1. The document discusses ionic equilibria, including acids and bases, and how to identify strong and weak acids/bases. It also discusses calculating pH and pOH values.
2. It explains how to determine if a salt is neutral, acidic, or basic based on whether the cation or anion comes from a strong or weak acid/base.
3. For sparingly soluble salts, it discusses using Ksp expressions and concentrations to determine if a precipitate will form from mixing solutions of ions.
Acid and base
The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
- Lewis in 1923 expanded the definition to electron pair transfers between any acids and bases, not just involving hydrogen.
- Other theories such as Lux-Flood's oxygen theory of 1939 and Pearson's hard/soft acid base principle
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This document discusses weak bases and how they react with water to form the conjugate acid and hydroxide ions. It defines the base dissociation constant Kb and explains how it refers to the equilibrium of a base reacting with water. It provides examples of calculating the concentration of hydroxide ions produced from a weak base solution and calculating Kb or Ka values for conjugate acid-base pairs using known constants. The document also discusses how the properties of salt solutions are determined by the constituent ions and how buffers resist changes in pH upon addition of acids or bases.
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- Organic bases usually contain nitrogen atoms that can accept protons. Common organic bases include amines, which have a lone pair of electrons on the nitrogen that can accept protons.
- Acid strength is determined by the amount of hydronium (H3O+) ions produced when the acid dissociates in water. Base strength is determined by the amount of hydroxide (OH-) ions produced upon dissolution in water. Factors like bond strength, stability of the conjugate base, and inductive effects influence
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Water is essential for life and makes up about two-thirds of the human body. It has no taste or smell and exists in solid, liquid, and gas forms. Water regulates body temperature, transports nutrients and waste, cushions joints, and maintains pH levels. The pH scale measures hydrogen ion concentration from 0-14, with 7 being neutral. Acids donate protons and have a pH below 7, while bases accept protons and have a pH above 7. Buffers resist pH changes and are important for biological processes.
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This document discusses acid-base theories and reactions. It begins with a brief history of acids and bases, noting they were originally defined based on their sour taste. It then focuses on three main acid-base theories:
1) Arrhenius theory defines acids as producing H+ ions in water and bases as producing OH- ions.
2) Brønsted-Lowry theory provides a more general definition, with acids as proton donors and bases as proton acceptors that form conjugate acid-base pairs.
3) Lewis theory defines acids and bases based on their ability to accept or donate electron pairs in chemical bonds.
The document goes on to discuss the properties of acids and bases, ion
Chap 8 acids, basis and salts
This document discusses acids, bases, and salts. It defines acids as substances that taste sour, react with metals and carbonates, and change litmus color. Bases taste bitter, feel slippery, and also change litmus color. Salts are water-soluble ionic compounds that can be acidic, basic, or neutral depending on whether they contain ions from strong/weak acids or bases. The document also covers ionization of water, pH and pOH calculations, acid-base concepts, conjugate pairs, and salt hydrolysis reactions that can produce acidic or basic solutions.
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Slides giving an overview on pH and its measurement.
Contains information about pH meters, its calibration, maintenance , types of ph electrode and modern definition of pH
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This document contains 20 questions and answers about acids, bases and salts. Some key points:
- Common household substances with pH >7 include eggs, baking soda and bleach. Substances with pH <7 include coffee, oranges and vinegar. Pure water has pH=7.
- A base is a substance that can accept protons or donate electron pairs. All alkalies are bases but not all bases are alkalies since alkalies must be water-soluble.
- Bronsted-Lowry bases accept protons, as in the reaction of HCl dissolving in water where H2O acts as the base. This theory applies to all protic solvents.
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The document defines pH and describes how it is measured. It begins by explaining that pH was introduced in 1909 by Sorensen to express the concentration of hydrogen ions (H+) in a solution. It then defines pH mathematically as the negative logarithm of the H+ concentration. The rest of the document discusses:
- How pH is measured using indicators and pH meters
- How the pH scale was developed based on experimental measurements of H+ concentrations
- Examples of calculating pH from H+ concentration and calculating H- concentration from pH
- Applications of pH including in nature, soil, and acid rain
Acidos y bases definiciones, ejemplos, escalas de acidez
1. Brønsted-Lowry acids are proton donors and bases are proton acceptors. A Brønsted-Lowry acid-base reaction involves the transfer of a proton from an acid to a base.
2. Acid strength is measured by an equilibrium constant (Ka) or pKa value, with a lower pKa indicating a stronger acid. Factors that increase acid strength include the electronegativity, size, inductive effects, and resonance stabilization of the conjugate base.
3. Common organic acids used in reactions include acetic acid and p-toluenesulfonic acid. Lewis acids, such as BF3 and AlCl3, are electron pair acceptors and react
AP Chemistry Chapter 16 Outline
This document provides an overview of acids and bases including:
- Definitions of acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories
- How acids and bases react in water, forming conjugates
- Factors that influence acid and base strength such as polarity, resonance, and electronegativity
- Calculations involving acid and base dissociation constants (Ka and Kb) to determine pH
pH
The document discusses pH, which is a measure of how acidic or basic a solution is. pH is defined as the negative logarithm of the hydrogen ion concentration and is measured on a scale from 0 to 14. A pH below 7 is acidic, above 7 is basic, and 7 is neutral. The document outlines how pH is measured, factors that affect pH in nature and living systems, and provides examples of pH levels in common foods and water quality standards.
P h metric titration
This document describes the procedure for determining the strength of a strong acid using pH-metric titration. The titration involves adding a strong base (NaOH) to a strong acid (HCl) until the equivalence point is reached. The pH is measured after each addition of base. By determining the volume of base required to reach the equivalence point and using the concentrations of the acid and base, the concentration of the original acid solution can be calculated. Calibrating the pH meter using buffer solutions ensures accurate pH measurements during the titration.
Water and p h
Water makes up 65-70% of the human body. It has unique properties like high melting and boiling points due to hydrogen bonding between water molecules. The bent shape of water molecules gives them a partial positive and negative charge, allowing them to form hydrogen bonds with other water molecules. These bonds contribute to water's high heat capacity and heat of vaporization. Water's pH measures the concentration of hydronium ions, with values below 7 indicating acidity and above 7 indicating alkalinity. pH is important in biological and chemical systems and can be measured using indicators, meters, and the Henderson-Hasselbalch equation.
pH indicator
The document defines pH as the negative logarithm of the hydrogen ion (H+) activity in a solution, with the pH scale ranging from 0 to 14. The hydrogen ions determine if a solution is acidic, alkaline, or neutral - if the hydrogen ion content is measured, the acidity or alkalinity can be determined. Water molecules dissociate into hydrogen and hydroxide ions through autoionization, affecting pH. pH indicators change color depending on the pH of a solution, allowing determination of acidity or alkalinity.
Bt 202 aug 12 2011 ppt1997-2004
This document discusses acids and bases including definitions, the pH scale, dissociation of weak acids and bases, buffers, and buffering in biological systems. Key points covered include the ionization of water, proton hopping, the definition of pH and pKa, acid-base reactions and conjugate pairs, Henderson-Hasselbalch equation, and examples of buffers in the body.
pH by KK SAHU sir
Introduction
History
Acid & Base
Ionization of water
Definitions of pH
(1) Mathematical Definition
(2) pH
(3) pOH
Buffer solution
(1) Types
(2) Buffer action
(3) Biological buffer systems
Henderson – Hasselbalch Equation
Measurement of pH
(1) pH Scale
(2) pH indicators
(3) pH meter
pH in human body and nature
Importance
Conclusion
Reference
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(electrometric and calorimetric), applications of buffers, buffer equation, buffer capacity,
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Walmart Business + (https://business.walmart.com/plus) is a new shopping experience for nonprofits, schools, and local business customers that connects an exclusive online shopping experience to stores. Benefits include free delivery and shipping, a 'Spend Analytics” feature, special discounts, deals and tax-exempt shopping.
Special TechSoup offer for a free 180 days membership, and up to $150 in discounts on eligible orders.
Spark Good (walmart.com/sparkgood) is a charitable platform that enables nonprofits to receive donations directly from customers and associates.
Answers about how you can do more with Walmart!"
Leveraging Generative AI to Drive Nonprofit Innovation
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
Wound healing PPT
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
Mule event processing models | MuleSoft Mysore Meetup #47
Mule event processing models | MuleSoft Mysore Meetup #47
Event Link:- https://meetups.mulesoft.com/events/details/mulesoft-mysore-presents-mule-event-processing-models/
Agenda
● What is event processing in MuleSoft?
● Types of event processing models in Mule 4
● Distinction between the reactive, parallel, blocking & non-blocking processing
For Upcoming Meetups Join Mysore Meetup Group - https://meetups.mulesoft.com/mysore/YouTube:- youtube.com/@mulesoftmysore
Mysore WhatsApp group:- https://chat.whatsapp.com/EhqtHtCC75vCAX7gaO842N
Speaker:-
Shivani Yasaswi - https://www.linkedin.com/in/shivaniyasaswi/
Organizers:-
Shubham Chaurasia - https://www.linkedin.com/in/shubhamchaurasia1/
Giridhar Meka - https://www.linkedin.com/in/giridharmeka
Priya Shaw - https://www.linkedin.com/in/priya-shaw
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Acids and Bases
- 2. What is an acid? Defined three ways: Arrhenius Acids: release H+ ions (protons) in aqueous solution. Bronsted-Lowry Acids: are proton donors. Lewis Acids: are electron pair acceptors
- 4. Arrhenius Bases: release OH- ions in aqueous solution
- 5. Bronsted-Lowry Bases: are proton acceptors
- 7. the pH scale The pH scale ranges from 0 to 14 7 is neutral on the pH scale Numbers below 7 are acidic The acidity increases as the number decreases Numbers above 7 are basic The basicity increases as the number increases The pH of a solution is exponential pH= -log(H+)