Acids and bases
•Download as PPT, PDF•
0 likes•872 views
Acids contain hydrogen and produce hydronium ions in water. They have a sour taste, are corrosive, and react with metals. Common acids include hydrochloric acid and sulfuric acid. Acids are used to make paper, paint, detergents, and fertilizer. Bases contain hydroxide ions and have a bitter taste and slippery feel. They are also corrosive and conduct electricity. Common bases are used to make soap, cleaners, and antacids. Strong acids and bases fully dissociate in water, producing more hydrogen or hydroxide ions, while weak acids and bases only partially dissociate. A neutralization reaction between an acid and base produces a salt and water
Report
Share
Report
Share
Recommended
Acids and bases
The document discusses the properties and characteristics of acids and bases. It explains that acids typically start with hydrogen and have a sour taste, while bases typically end with hydroxide and have a bitter taste. It also distinguishes between strong and weak acids/bases based on how fully they dissociate in water. Common uses of acids and bases are also outlined.
Acids, bases, & salts by sugam raghav
Acids have a pH less than 7 and neutralize bases by donating hydrogen ions in solution. Common acids include hydrochloric acid in stomachs, sulfuric acid in car batteries, and acetic acid in vinegar. Strong acids like hydrochloric and nitric acids fully ionize in water, while weak acids like acetic and phosphoric acids only partially ionize. Bases accept hydrogen ions and include sodium hydroxide, calcium hydroxide, and ammonium hydroxide. The pH scale measures hydrogen ion concentration from 0 to 14, with acids having a lower pH and bases a higher pH. A neutralization reaction occurs when an acid and base react, producing a salt and water.
1 acids & bases introduction
Acids are solutions that contain hydrogen ions or hydronium ions and have a pH below 7. They taste sour and can corrode metals. Bases are solutions that contain hydroxide ions and have a pH above 7. They taste bitter and feel soapy. The document discusses various properties of acids and bases like their reactions, uses in products and industry, and how pH is measured. It also provides examples of experiments to observe the reactivity of acids and bases with different substances.
Acids And Bases
This document discusses acids, bases, and the neutralization reaction between acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as metal oxides or hydroxides. Examples of acids and bases are provided. The document explains that the reaction between an acid and a base, called neutralization, produces a salt and water. Chemical equations for common neutralization reactions are given.
20sec3
Svante Arrhenius was a Swedish chemist who developed one of the first theories of acids and bases in 1887. He defined acids as substances that produce hydrogen ions in aqueous solution and bases as substances that produce hydroxide ions in water. Hubert Alyea was Arrhenius' last graduate student. In 1923, Brønsted and Lowry expanded this definition to include acids as hydrogen ion donors and bases as hydrogen ion acceptors, allowing substances like ammonia to be classified as a base. They also introduced the concept of conjugate acid-base pairs. Finally, in 1923 Gilbert Lewis defined acids and bases more generally as electron pair acceptors and donors, respectively, without requiring hydrogen. This most
Power point presentation acid
The document discusses different types of acids including binary acids like hydrofluoric acid and ternary acids like sulfuric acid. It defines acids according to Arrhenius and Brønsted-Lowry theories and explains that acids ionize in water to form hydronium ions. Strong acids ionize completely while weaker acids do not ionize as much. The document also discusses the ionization of several acids like sulfuric acid and acetic acid. It identifies characteristics of acids such as reacting with active metals and changing the color of indicators.
Acids and bases
Acids produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water. They are sour, can turn litmus paper red, and have a pH below 7. Acids can be divided into strong acids, which ionize completely, and weak acids, which ionize partially. Examples of strong mineral acids are hydrochloric acid, sulfuric acid, and nitric acid. Examples of weak organic acids are acetic acid, formic acid, and oxalic acid. Acids react with bases to form salts and water, and with metals to produce salts and hydrogen gas.
Acids
Acids are chemical substances that form hydrogen ions (H+) in aqueous solutions, resulting in a sour taste and pH lower than 7. They neutralize bases, corrode metals by forming hydrogen gas, and are good conductors of electricity. Common acids include hydrochloric acid in stomachs, sulfuric acid in car batteries, acetic acid in vinegar, and phosphoric acid used in flavorings. Acid rain forms when acids fall as rain, snow, or fog, and can damage plants, aquatic life, and infrastructure.
Recommended
Acids and bases
The document discusses the properties and characteristics of acids and bases. It explains that acids typically start with hydrogen and have a sour taste, while bases typically end with hydroxide and have a bitter taste. It also distinguishes between strong and weak acids/bases based on how fully they dissociate in water. Common uses of acids and bases are also outlined.
Acids, bases, & salts by sugam raghav
Acids have a pH less than 7 and neutralize bases by donating hydrogen ions in solution. Common acids include hydrochloric acid in stomachs, sulfuric acid in car batteries, and acetic acid in vinegar. Strong acids like hydrochloric and nitric acids fully ionize in water, while weak acids like acetic and phosphoric acids only partially ionize. Bases accept hydrogen ions and include sodium hydroxide, calcium hydroxide, and ammonium hydroxide. The pH scale measures hydrogen ion concentration from 0 to 14, with acids having a lower pH and bases a higher pH. A neutralization reaction occurs when an acid and base react, producing a salt and water.
1 acids & bases introduction
Acids are solutions that contain hydrogen ions or hydronium ions and have a pH below 7. They taste sour and can corrode metals. Bases are solutions that contain hydroxide ions and have a pH above 7. They taste bitter and feel soapy. The document discusses various properties of acids and bases like their reactions, uses in products and industry, and how pH is measured. It also provides examples of experiments to observe the reactivity of acids and bases with different substances.
Acids And Bases
This document discusses acids, bases, and the neutralization reaction between acids and bases. It defines acids as substances that produce hydrogen ions in water and bases as metal oxides or hydroxides. Examples of acids and bases are provided. The document explains that the reaction between an acid and a base, called neutralization, produces a salt and water. Chemical equations for common neutralization reactions are given.
20sec3
Svante Arrhenius was a Swedish chemist who developed one of the first theories of acids and bases in 1887. He defined acids as substances that produce hydrogen ions in aqueous solution and bases as substances that produce hydroxide ions in water. Hubert Alyea was Arrhenius' last graduate student. In 1923, Brønsted and Lowry expanded this definition to include acids as hydrogen ion donors and bases as hydrogen ion acceptors, allowing substances like ammonia to be classified as a base. They also introduced the concept of conjugate acid-base pairs. Finally, in 1923 Gilbert Lewis defined acids and bases more generally as electron pair acceptors and donors, respectively, without requiring hydrogen. This most
Power point presentation acid
The document discusses different types of acids including binary acids like hydrofluoric acid and ternary acids like sulfuric acid. It defines acids according to Arrhenius and Brønsted-Lowry theories and explains that acids ionize in water to form hydronium ions. Strong acids ionize completely while weaker acids do not ionize as much. The document also discusses the ionization of several acids like sulfuric acid and acetic acid. It identifies characteristics of acids such as reacting with active metals and changing the color of indicators.
Acids and bases
Acids produce hydrogen ions (H+) or hydronium ions (H3O+) when dissolved in water. They are sour, can turn litmus paper red, and have a pH below 7. Acids can be divided into strong acids, which ionize completely, and weak acids, which ionize partially. Examples of strong mineral acids are hydrochloric acid, sulfuric acid, and nitric acid. Examples of weak organic acids are acetic acid, formic acid, and oxalic acid. Acids react with bases to form salts and water, and with metals to produce salts and hydrogen gas.
Acids
Acids are chemical substances that form hydrogen ions (H+) in aqueous solutions, resulting in a sour taste and pH lower than 7. They neutralize bases, corrode metals by forming hydrogen gas, and are good conductors of electricity. Common acids include hydrochloric acid in stomachs, sulfuric acid in car batteries, acetic acid in vinegar, and phosphoric acid used in flavorings. Acid rain forms when acids fall as rain, snow, or fog, and can damage plants, aquatic life, and infrastructure.
Applications of salts
This document discusses various types of salts and their properties and applications. It defines salts as ionic compounds that result from acid-base neutralization reactions. It provides examples of common salts like sodium chloride, potassium sulfate and lists their properties such as being crystalline solids with high melting/boiling points that dissolve in water and conduct electricity. It then describes specific applications of salts like sodium chloride in the Chlor-alkali process, baking soda in baking and antacids, and plaster of paris in supporting fractured bones.
Chemicals from salts
Sodium chloride, or common salt, is an important raw material used to make many chemicals. When electricity is passed through a solution of salt water, it decomposes to form sodium hydroxide and chlorine in a process called the chlor-alkali process. Chlorine is used to make bleaching powder and sodium hydroxide is used to make baking soda. Baking soda, also known as sodium bicarbonate, is used to make baking powder and as an antacid. Washing soda, or sodium carbonate, can also be derived from salt and is used in glass, soap, and paper industries.
Class 10(CBSE) Uses of Salt
The document discusses how common salt (sodium chloride) is used as a raw material to produce various chemicals. It describes the production of sodium hydroxide, bleaching powder, baking soda and washing soda from sodium chloride. Sodium hydroxide is produced through the electrolysis of sodium chloride solution. Bleaching powder is made by reacting chlorine gas with slaked lime. Baking soda is produced from sodium chloride, water, carbon dioxide and ammonia. Washing soda is obtained by crystallizing sodium carbonate. These chemicals find applications in industries and domestic uses.
Acids and bases
This document provides a review of acids and bases, including their characteristics, common examples, naming conventions, and reactions. It discusses how acids increase hydrogen ion concentration in solution while bases increase hydroxide ion concentration. Strong acids and bases are memorized. Metal oxides form bases in water while non-metal oxides form acids. Acids and bases neutralize through reactions that form water and a salt. Titrations involve using a solution of known concentration to determine the concentration of an analyte. [/SUMMARY]
Chapter 10.3
This document defines acids and bases and explains how pH is measured. Acids donate hydronium ions (H3O+) in water, while bases donate hydroxide ions (OH-). The pH scale measures the concentration of hydronium ions, with lower pH indicating more acidic solutions and higher pH indicating more basic solutions. A difference of one pH unit represents a tenfold change in hydronium ion concentration. pH is measured using indicators, strips, or meters that detect the acidity level of solutions.
Acidsand bases
Acids are corrosive and sour, reacting with metals and bases to produce hydrogen ions and turn litmus paper pink, with a pH between 0-7. Bases are slippery or bitter, react with fats and acids to produce hydroxide ions and turn litmus blue, with a pH of 7-14. Nonmetal oxides like carbon dioxide and nitrogen dioxide form acidic oxides in water, while most metallic oxides react with water to form basic solutions like sodium hydroxide.
Chap 2 sec 1
Matter occupies space and has mass. Volume is the amount of space an object occupies. Mass is the amount of matter in an object and remains constant anywhere, while weight depends on gravitational force and location. Mass is measured in grams using a balance, while weight is measured in Newtons using a spring scale. Mass is a measure of an object's inertia, or resistance to changes in motion. The more mass an object has, the harder it is to start or stop its motion according to Newton's First Law of Motion.
Chap 2 chem & phy properties
This document discusses the differences between physical and chemical properties of matter. Physical properties can be observed or measured without changing the identity of the substance, such as boiling point, density, state, and color. Physical changes alter the substance's form but not its composition, like melting, freezing, or bending. Chemical properties describe a substance's ability to undergo chemical reactions, for example flammability or reactivity. Chemical changes result in one or more new substances forming through chemical reactions. The identity of the original substance is changed in a chemical change.
States of matter
This document discusses the different states of matter and the changes between states. It explains that solids have a definite shape and volume due to the tight packing and vibration of particles. Liquids can change shape but not volume as their particles can slide past one another. Gases expand to fill their containers as their particles are far apart and move independently. Changes between solid, liquid and gas require the addition or removal of energy. The document provides examples of different states and phase changes.
Mixtures, solutions, elements, compounds
This document defines and provides examples of mixtures, solutions, suspensions, colloids, and gas mixtures. It explains that mixtures can be physically separated into their original substances, while solutions appear homogeneous. Suspensions can settle out but colloids cannot. It also defines elements as pure substances that cannot be broken down further, and compounds as pure substances formed by a chemical combination of elements in fixed ratios that have unique properties.
Periodic table shortened
The periodic table organizes elements according to their atomic structure. Dmitri Mendeleev organized the first periodic table by atomic mass, which allowed him to predict undiscovered elements. Henry Moseley later determined that atomic number provided an even more logical ordering. Most elements are metals and are found on the left side of the periodic table, while nonmetals are on the right. Elements in the same column have similar properties due to their valence electron configuration. The periodic table provides a wealth of information about each element and illustrates patterns in their chemical and physical properties.
Ps1 chapter 1
This chapter discusses physical science and the scientific method. Physical science involves the study of matter and energy, including chemistry which examines all forms of matter and physics which analyzes how energy affects matter. The scientific method involves asking a question, forming a hypothesis, testing the hypothesis through experimentation, analyzing results, drawing a conclusion, and communicating findings. Key terms defined include the independent and dependent variables, control groups, and different types of models used to represent scientific concepts. Laws summarize experimental evidence while theories provide explanations for observed phenomena.
Heat
The document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points and Kelvin having absolute zero as its lowest value. Heat transfers between objects with different temperatures in order to equalize thermal energy, which is the kinetic energy of particles. Materials are classified as conductors or insulators based on their ability to transfer thermal energy through conduction, convection, or radiation.
Equipment 2016
The document lists various pieces of scientific equipment commonly found in a laboratory including beakers, erlenmeyer flasks, stir rods, graduated cylinders, microscopes, bunsen burners, weigh papers, rulers, test tubes, funnels, pipettes, filter paper, scales, scissors, probes, forceps, dissecting trays, pins, and scalpels.
Chemical bonding 2 no bonds
Bonds form between elements when their molecules rearrange to become stable compounds. This requires energy and allows the outer electron levels of one element to reach eight electrons. There are three main types of bonds: ionic bonds between metals and nonmetals where electrons are transferred, covalent bonds between nonmetals where electrons are shared, and metallic bonds between metals. To identify bonds, locate the elements on the periodic table to determine if they are metals or nonmetals and then apply the appropriate bonding model.
Atomic theory
This document provides an overview of the development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments and evidence available at the time. Their work established that atoms are the smallest particles of matter, have a small, dense nucleus surrounded by electrons, and can combine to form all chemical elements.
Tools and measurement
This document discusses tools and units for measuring various physical properties including volume, mass, length, force, temperature, time, area, and volume. It lists common tools used to measure each property and their standard metric units. The document also introduces the International System of Units (SI) as the global standard for measurement and explains that density is calculated by dividing an object's mass by its volume rather than being directly measured.
Chemical reactions
This document discusses key concepts in chemistry including types of chemical reactions such as single displacement, synthesis, decomposition, and double displacement reactions. It also covers important laws like the law of conservation of energy and mass. Exothermic and endothermic reactions are defined as well as activation energy, catalysts, and inhibitors. The key components of a balanced chemical equation like reactants and products are outlined. Finally, the six steps for balancing chemical equations are provided.
Energy 2 without alternatives
Energy can exist in various forms and can be transferred from one form to another but not created or destroyed. There are nine main types of energy: kinetic, potential, mechanical, thermal, chemical, electrical, sound, light, and nuclear. Energy transfers allow important functions like photosynthesis, cellular respiration, and power generation. Chemical energy is a common form of stored potential energy that can be released to do work.
Electricity
Electricity is the movement of electric charge. Electric charge can be positive or negative, and like charges repel while opposite charges attract. The amount of charge and distance between charges determine the electric force. An electric field exists around charged objects, and objects become charged through friction, conduction, or induction. Electricity can be used to power circuits consisting of a source, wires, and a load to convert the energy into other forms. Circuit failures are prevented by fuses and circuit breakers.
Work, power and machines with pitucres
The document defines work as energy transferred by a force causing movement, with the formula W=Fxd. Power is the rate of work over time, with the formula P=W/t. Machines make work easier by changing the amount or direction of force, classified as simple machines like levers, pulleys, wheels and axles, inclined planes, wedges, screws, or compound machines combining simple machines. Mechanical advantage is the number of times a machine multiplies force, while efficiency is the ratio of work output to input accounting for energy lost to friction.
Force, mass, acceleration
This document discusses key concepts relating to gravity, motion, and Newton's laws of motion:
- Galileo determined that the rate at which objects fall is not dependent on their mass, and acceleration depends on force and mass.
- All objects accelerate towards Earth at 9.8 m/s^2 due to gravity. Newton's second law relates force, mass, and acceleration.
- Newton's three laws of motion are: 1) an object remains in motion unless acted on by an external force, 2) acceleration depends on net force and mass, and 3) for every action there is an equal and opposite reaction.
More Related Content
What's hot
Applications of salts
This document discusses various types of salts and their properties and applications. It defines salts as ionic compounds that result from acid-base neutralization reactions. It provides examples of common salts like sodium chloride, potassium sulfate and lists their properties such as being crystalline solids with high melting/boiling points that dissolve in water and conduct electricity. It then describes specific applications of salts like sodium chloride in the Chlor-alkali process, baking soda in baking and antacids, and plaster of paris in supporting fractured bones.
Chemicals from salts
Sodium chloride, or common salt, is an important raw material used to make many chemicals. When electricity is passed through a solution of salt water, it decomposes to form sodium hydroxide and chlorine in a process called the chlor-alkali process. Chlorine is used to make bleaching powder and sodium hydroxide is used to make baking soda. Baking soda, also known as sodium bicarbonate, is used to make baking powder and as an antacid. Washing soda, or sodium carbonate, can also be derived from salt and is used in glass, soap, and paper industries.
Class 10(CBSE) Uses of Salt
The document discusses how common salt (sodium chloride) is used as a raw material to produce various chemicals. It describes the production of sodium hydroxide, bleaching powder, baking soda and washing soda from sodium chloride. Sodium hydroxide is produced through the electrolysis of sodium chloride solution. Bleaching powder is made by reacting chlorine gas with slaked lime. Baking soda is produced from sodium chloride, water, carbon dioxide and ammonia. Washing soda is obtained by crystallizing sodium carbonate. These chemicals find applications in industries and domestic uses.
Acids and bases
This document provides a review of acids and bases, including their characteristics, common examples, naming conventions, and reactions. It discusses how acids increase hydrogen ion concentration in solution while bases increase hydroxide ion concentration. Strong acids and bases are memorized. Metal oxides form bases in water while non-metal oxides form acids. Acids and bases neutralize through reactions that form water and a salt. Titrations involve using a solution of known concentration to determine the concentration of an analyte. [/SUMMARY]
Chapter 10.3
This document defines acids and bases and explains how pH is measured. Acids donate hydronium ions (H3O+) in water, while bases donate hydroxide ions (OH-). The pH scale measures the concentration of hydronium ions, with lower pH indicating more acidic solutions and higher pH indicating more basic solutions. A difference of one pH unit represents a tenfold change in hydronium ion concentration. pH is measured using indicators, strips, or meters that detect the acidity level of solutions.
Acidsand bases
Acids are corrosive and sour, reacting with metals and bases to produce hydrogen ions and turn litmus paper pink, with a pH between 0-7. Bases are slippery or bitter, react with fats and acids to produce hydroxide ions and turn litmus blue, with a pH of 7-14. Nonmetal oxides like carbon dioxide and nitrogen dioxide form acidic oxides in water, while most metallic oxides react with water to form basic solutions like sodium hydroxide.
What's hot (6)
Viewers also liked
Chap 2 sec 1
Matter occupies space and has mass. Volume is the amount of space an object occupies. Mass is the amount of matter in an object and remains constant anywhere, while weight depends on gravitational force and location. Mass is measured in grams using a balance, while weight is measured in Newtons using a spring scale. Mass is a measure of an object's inertia, or resistance to changes in motion. The more mass an object has, the harder it is to start or stop its motion according to Newton's First Law of Motion.
Chap 2 chem & phy properties
This document discusses the differences between physical and chemical properties of matter. Physical properties can be observed or measured without changing the identity of the substance, such as boiling point, density, state, and color. Physical changes alter the substance's form but not its composition, like melting, freezing, or bending. Chemical properties describe a substance's ability to undergo chemical reactions, for example flammability or reactivity. Chemical changes result in one or more new substances forming through chemical reactions. The identity of the original substance is changed in a chemical change.
States of matter
This document discusses the different states of matter and the changes between states. It explains that solids have a definite shape and volume due to the tight packing and vibration of particles. Liquids can change shape but not volume as their particles can slide past one another. Gases expand to fill their containers as their particles are far apart and move independently. Changes between solid, liquid and gas require the addition or removal of energy. The document provides examples of different states and phase changes.
Mixtures, solutions, elements, compounds
This document defines and provides examples of mixtures, solutions, suspensions, colloids, and gas mixtures. It explains that mixtures can be physically separated into their original substances, while solutions appear homogeneous. Suspensions can settle out but colloids cannot. It also defines elements as pure substances that cannot be broken down further, and compounds as pure substances formed by a chemical combination of elements in fixed ratios that have unique properties.
Periodic table shortened
The periodic table organizes elements according to their atomic structure. Dmitri Mendeleev organized the first periodic table by atomic mass, which allowed him to predict undiscovered elements. Henry Moseley later determined that atomic number provided an even more logical ordering. Most elements are metals and are found on the left side of the periodic table, while nonmetals are on the right. Elements in the same column have similar properties due to their valence electron configuration. The periodic table provides a wealth of information about each element and illustrates patterns in their chemical and physical properties.
Ps1 chapter 1
This chapter discusses physical science and the scientific method. Physical science involves the study of matter and energy, including chemistry which examines all forms of matter and physics which analyzes how energy affects matter. The scientific method involves asking a question, forming a hypothesis, testing the hypothesis through experimentation, analyzing results, drawing a conclusion, and communicating findings. Key terms defined include the independent and dependent variables, control groups, and different types of models used to represent scientific concepts. Laws summarize experimental evidence while theories provide explanations for observed phenomena.
Heat
The document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points and Kelvin having absolute zero as its lowest value. Heat transfers between objects with different temperatures in order to equalize thermal energy, which is the kinetic energy of particles. Materials are classified as conductors or insulators based on their ability to transfer thermal energy through conduction, convection, or radiation.
Equipment 2016
The document lists various pieces of scientific equipment commonly found in a laboratory including beakers, erlenmeyer flasks, stir rods, graduated cylinders, microscopes, bunsen burners, weigh papers, rulers, test tubes, funnels, pipettes, filter paper, scales, scissors, probes, forceps, dissecting trays, pins, and scalpels.
Chemical bonding 2 no bonds
Bonds form between elements when their molecules rearrange to become stable compounds. This requires energy and allows the outer electron levels of one element to reach eight electrons. There are three main types of bonds: ionic bonds between metals and nonmetals where electrons are transferred, covalent bonds between nonmetals where electrons are shared, and metallic bonds between metals. To identify bonds, locate the elements on the periodic table to determine if they are metals or nonmetals and then apply the appropriate bonding model.
Atomic theory
This document provides an overview of the development of atomic theory from ancient Greek philosophers to modern atomic structure. It describes key contributors such as Democritus, Dalton, Thomson, Rutherford, Bohr, and Schrodinger who proposed models of the atom based on experiments and evidence available at the time. Their work established that atoms are the smallest particles of matter, have a small, dense nucleus surrounded by electrons, and can combine to form all chemical elements.
Tools and measurement
This document discusses tools and units for measuring various physical properties including volume, mass, length, force, temperature, time, area, and volume. It lists common tools used to measure each property and their standard metric units. The document also introduces the International System of Units (SI) as the global standard for measurement and explains that density is calculated by dividing an object's mass by its volume rather than being directly measured.
Chemical reactions
This document discusses key concepts in chemistry including types of chemical reactions such as single displacement, synthesis, decomposition, and double displacement reactions. It also covers important laws like the law of conservation of energy and mass. Exothermic and endothermic reactions are defined as well as activation energy, catalysts, and inhibitors. The key components of a balanced chemical equation like reactants and products are outlined. Finally, the six steps for balancing chemical equations are provided.
Energy 2 without alternatives
Energy can exist in various forms and can be transferred from one form to another but not created or destroyed. There are nine main types of energy: kinetic, potential, mechanical, thermal, chemical, electrical, sound, light, and nuclear. Energy transfers allow important functions like photosynthesis, cellular respiration, and power generation. Chemical energy is a common form of stored potential energy that can be released to do work.
Electricity
Electricity is the movement of electric charge. Electric charge can be positive or negative, and like charges repel while opposite charges attract. The amount of charge and distance between charges determine the electric force. An electric field exists around charged objects, and objects become charged through friction, conduction, or induction. Electricity can be used to power circuits consisting of a source, wires, and a load to convert the energy into other forms. Circuit failures are prevented by fuses and circuit breakers.
Work, power and machines with pitucres
The document defines work as energy transferred by a force causing movement, with the formula W=Fxd. Power is the rate of work over time, with the formula P=W/t. Machines make work easier by changing the amount or direction of force, classified as simple machines like levers, pulleys, wheels and axles, inclined planes, wedges, screws, or compound machines combining simple machines. Mechanical advantage is the number of times a machine multiplies force, while efficiency is the ratio of work output to input accounting for energy lost to friction.
Force, mass, acceleration
This document discusses key concepts relating to gravity, motion, and Newton's laws of motion:
- Galileo determined that the rate at which objects fall is not dependent on their mass, and acceleration depends on force and mass.
- All objects accelerate towards Earth at 9.8 m/s^2 due to gravity. Newton's second law relates force, mass, and acceleration.
- Newton's three laws of motion are: 1) an object remains in motion unless acted on by an external force, 2) acceleration depends on net force and mass, and 3) for every action there is an equal and opposite reaction.
Speed, time, distance
This document defines key concepts related to motion, including speed, velocity, acceleration, force, friction, gravity, and mass. It explains that speed is distance divided by time, velocity includes both speed and direction, and acceleration is the rate of change of velocity. Forces can be added or subtracted depending on their direction. Net force determines if motion occurs, with balanced forces resulting in no motion. Gravity is the force of attraction between objects due to their mass, and increases with mass but decreases with distance. Weight is the measure of gravitational force on an object and depends on its location and mass.
Waves and light without star stuff
This document discusses different types of waves including mechanical waves that require a medium and electromagnetic waves that can travel through empty space. It describes properties of waves like amplitude, wavelength, frequency, and speed. Key behaviors of waves are also outlined such as reflection, refraction, diffraction, interference, and absorption. The document provides details about electromagnetic waves, sound waves, and how lenses and mirrors interact with light waves.
Chap 2 chem & phy properties
This document discusses the differences between physical and chemical properties of matter. Physical properties can be observed or measured without changing the identity of the substance, such as boiling point, density, state, and color. Physical changes alter the substance's form but not its composition, like melting, freezing, or bending. Chemical properties describe a substance's ability to undergo chemical reactions, for example flammability or reactivity. Chemical changes result in one or more new substances forming through chemical reactions. The identity of the original substance is changed in a chemical change.
Heat
This document discusses key concepts relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of particles in an object. As temperature increases, particles move faster, spreading out through thermal expansion. Different temperature scales are presented, with Fahrenheit and Celsius defined by their freezing and boiling points of water, and Kelvin having the lowest possible temperature of absolute zero. Heat is defined as the transfer of thermal energy between objects with different temperatures, while thermal energy is the kinetic energy within an object. Materials are classified as conductors or insulators based on their ability to transfer heat. The three main methods of heat transfer are conduction (direct contact), convection (movement of molecules in gases and liquids), and radiation (
Viewers also liked (20)
Similar to Acids and bases
Acids and bases
The document discusses the properties and characteristics of acids and bases. It explains that acids typically start with hydrogen and have a sour taste, while bases typically end with hydroxide and have a bitter taste. It also distinguishes between strong and weak acids/bases based on how fully they dissociate in water. Common uses of acids and bases are also outlined.
Acids Bases and Salts ppt.ppt
This document defines acids, bases, and salts. It states that acids have a pH below 7 and contain hydrogen ions (H+) in solution. They neutralize bases and are corrosive. Bases have a pH above 7, feel slippery, taste bitter, contain hydroxide (OH-) ions in solution, and neutralize acids. Common acids and bases are listed. Salts are formed from the positive ion of a base and negative ion of an acid during a neutralization reaction between an acid and base, producing water. Examples of salts include NaCl and MgSO4.
Chapter-2_acids__bases_and_salts.pdf
Acids produce hydrogen ions (H+) in water and have a sour taste, corrode materials, and react with metals. Bases produce hydroxide ions (OH-) in water and feel slippery. Common acids include citric, lactic, acetic, and carbonic acids. Common bases include ammonia, sodium hydroxide, and magnesium hydroxide. Indicators like litmus paper are used to determine if a substance is an acid or base by changing color. The pH scale measures the acidity or alkalinity of a solution based on hydrogen ion concentration, with lower pH indicating more acidity. Strong acids and bases fully dissociate in water compared to weak acids and bases. Neutralization is
ACIDS AND BASES
Acids and bases are defined by their properties in aqueous solutions. Acids release hydrogen ions (H+) and have a sour taste, while bases release hydroxide ions (OH-) and feel slippery. The pH scale measures acidity and basicity, with values from 0-14 and neutral substances having a pH of 7. Acid-base indicators change color with pH and can test whether a solution is acidic or basic. When acids and bases are mixed, a neutralization reaction occurs where they cancel out each other's properties and form a salt and water.
ACIDS and BASES.
Properties/characteristics of Acid and Base.
Understanding the pH scale.
Acid-Base Indicator.
Neutralization.
Example of acids and bases
Acids, bases, & salts
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7, forming H+ ions in solution, and neutralizing bases. Common acids include hydrochloric, sulfuric, nitric, acetic, carbonic, and phosphoric acids. Bases are defined as having a pH greater than 7, feeling slippery, and dissolving fats and oils. Common bases include sodium hydroxide, magnesium hydroxide, aluminum hydroxide, and ammonium hydroxide. Salts are formed from the reaction of acids and bases and are composed of the negative ion of an acid and positive ion of a base. A neutralization reaction produces a salt and water when an acid re
acids and bases
1) Acids release H+ ions in water and bases release OH- ions. Strong acids and bases dissociate completely while weak acids and bases only partially dissociate.
2) Acids taste sour, turn litmus red, and react with metals and carbonates. Bases taste bitter and feel slippery.
3) The pH scale measures acidity and alkalinity, with values below 7 being acidic and above 7 being basic. Acid-base indicators change color at specific pH values.
Acids, bases, and salts
This document defines acids, bases, and salts. It explains that acids have a pH below 7 and donate hydrogen ions in solution, forming H+ ions. Bases have a pH above 7 and donate hydroxide ions in solution, feeling slippery. Salts are neutral compounds formed from the reaction of acids and bases, containing the positive ion from the base and negative ion from the acid. Common acids include hydrochloric, sulfuric, nitric, acetic, carbonic, and phosphoric acids. Common bases include sodium hydroxide, magnesium hydroxide, and aluminum hydroxide.
solutions.ppt
Mixtures can be either heterogeneous or homogeneous. Heterogeneous mixtures have visibly distinct components that can be separated physically, like a trail mix. Homogeneous mixtures appear uniform throughout and cannot be separated into distinct components using physical means, like salt water solutions. Solutions are a type of homogeneous mixture where a solute dissolves uniformly in a solvent. The concentration of a solute affects properties of the solvent like freezing point and boiling point. Acids donate hydrogen ions in water and turn litmus paper red, while bases accept hydrogen ions and turn litmus paper blue. A neutralization reaction occurs when an acid and base react and produce water and a salt. The pH scale measures acidity from 0-7 or basicity from
Arrhenius
The document discusses Arrhenius's theory of acids and bases. It defines acids as hydrogen-containing compounds that yield hydrogen ions (H+) in solution, and bases as compounds that yield hydroxide ions (OH-) in solution. It provides examples of common acids like hydrochloric acid and sulfuric acid, as well as bases like sodium hydroxide. It classifies acids based on the number of ionizable hydrogens they contain as mono-, di-, or triprotic. The document also discusses the properties of acids and bases and their reactions in aqueous solutions.
Solutions
This document discusses different types of mixtures including heterogeneous and homogeneous mixtures. Heterogeneous mixtures are mixtures with visibly different parts that can be separated, like trail mix. Homogeneous mixtures are uniform mixtures like salt water solutions that cannot be easily separated. Solutions are a type of homogeneous mixture where a solute dissolves evenly throughout a solvent. Concentration, solubility, acids, bases, and the pH scale are also explained in the context of mixtures and solutions.
Acid Base And Salt.pdf
1) Acids are compounds that form hydrogen (H+) ions in solution and have a pH less than 7. Common strong acids include hydrochloric acid, nitric acid, and sulfuric acid.
2) Bases are compounds that form hydroxide (OH-) ions in solution and have a pH greater than 7. Common bases include sodium hydroxide, calcium hydroxide, and ammonium hydroxide.
3) A salt is formed through a neutralization reaction between an acid and a base, producing water and an ionic compound composed of the cation from the base and the anion from the acid. Examples of salts include sodium chloride, magnesium sulfate, and ammonium nitrate.
Lesson 9 acids and bases
Acids and bases are defined by whether they release H+ or OH- ions in water. Strong acids and bases dissociate completely, while weak ones only partially dissociate. Acids taste sour, react with carbonates and metals to produce gas, and contain hydrogen. Bases taste bitter, feel slippery, and contain hydroxide ions. The pH scale measures acidity and alkalinity, with values below 7 indicating acids and above 7 indicating bases. Acid-base indicators change color at specific pH levels, allowing identification of acids and bases. When acids and bases neutralize, they form water and salts.
notes-acidsandbases-130210121114-phpapp02.pptx
Acids and bases are characterized by their ability to release hydrogen or hydroxide ions in water. Acids release H+ ions and have a sour taste, react with carbonates and metals, and contain hydrogen. Bases release OH- ions and have a bitter taste, feel slippery, and contain hydroxide. The strength of acids and bases is measured by pH, with lower values indicating more H+ ions and higher values indicating more OH- ions. Acid-base indicators change color based on pH and can be used to determine if a solution is acidic or basic. When an acid and base are combined, they neutralize through a reaction that produces a salt and water.
Acids, bases, & salts
This document provides information about acids, bases, and salts. It defines acids as having a pH less than 7 and describes their properties such as neutralizing bases and forming hydrogen ions in solution. Strong acids like hydrochloric acid are described as ionizing completely, while weak acids only partially ionize. Common acids are also listed such as hydrochloric acid found in stomachs. Bases are defined as having a pH greater than 7 and their properties are outlined. The document further discusses pH scales, indicators, buffers, and examples of acid-base reactions. Digestion and pH levels in different parts of the digestive system are briefly covered.
Acids, Bases, & Salts.ppt
Acids have a pH below 7 and donate hydrogen ions in solution. They react with bases, which have a pH above 7 and accept hydrogen ions, to form neutral salts. Strong acids and bases fully ionize in water, while weak ones only partially ionize. The pH scale measures hydrogen ion concentration from 0 to 14. Buffers resist pH changes when small amounts of acids or bases are added. Digestion involves both mechanical and chemical breakdown of food, with the mouth having a neutral pH and the stomach a strongly acidic pH of around 2 to aid in protein breakdown.
Acids, Bases, & Salts (1).ppt
Acids have a pH below 7 and donate hydrogen ions in solution. They neutralize bases and include stomach acid, battery acid, and vinegar. Bases have a pH above 7, feel slippery, and dissolve fats. Common bases are lye, antacids, and ammonia. A salt is the product of a neutralization reaction between an acid and a base, consisting of the positive ion of the base and the negative ion of the acid.
Acids, Bases, & Salts.ppt
Acids have a pH below 7 and donate hydrogen ions in solution, forming H+ ions. They react with metals and bases. Bases have a pH above 7 and accept hydrogen ions, forming OH- ions. Common acids include HCl and H2SO4, while common bases include NaOH and Mg(OH)2. A salt is formed during a neutralization reaction between an acid and a base, producing water. The digestive system uses acids and bases to break down foods, with the stomach having a highly acidic pH around 2 to aid in digestion.
Acid bases n salts
Acids produce hydrogen ions in water and have sour tastes, while bases produce hydroxide ions in water and have bitter tastes. Common acids include citric acid and hydrochloric acid, while common bases include sodium hydroxide and ammonia. Strong acids and bases fully dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures how acidic or basic a solution is. Neutralization is the reaction between an acid and base that produces water and a salt. Indicators change color to determine if a solution is acidic or basic.
Similar to Acids and bases (20)
More from tracyconover
Endocrine and reproduction modified
The endocrine system produces hormones that control body functions and are released by glands. The major glands include the pituitary, thyroid, parathyroid, adrenals, pancreas, ovaries, and testes. Hormones travel through the bloodstream and bind to receptors on cells to regulate processes like metabolism, immune function, reproduction, and stress response. Endocrine disorders occur when hormone levels are too high or too low, leading to conditions such as diabetes, thyroid disorders, and reproductive issues.
Circulatory and lymphatic, respiratory
The circulatory, lymphatic, and respiratory systems work together to transport nutrients, gases, and waste throughout the body. The cardiovascular system uses the heart, blood vessels and blood to carry oxygen and nutrients to cells and remove waste. Blood contains plasma, red blood cells, white blood cells and platelets. The lymphatic system returns fluids leaked from tissues to the bloodstream and fights pathogens using lymph nodes and vessels. The respiratory system takes in oxygen through the nose, pharynx, larynx, trachea, bronchi and lungs where gas exchange occurs in alveoli, then expels carbon dioxide.
Digestion and urinary
The tentative schedule outlines that the class will cover the digestive/circulatory systems from 3-12 to 3-16, the circulatory/respiratory and lymphatic systems from 3-19 to 3-23, and the reproductive/endocrine systems from 3-26 to 4-10. A pig dissection will take place around 4-11 and last until 4-27.
The digestive system breaks down food into nutrients that can be absorbed and used by the body. It consists of the mouth, esophagus, stomach, small intestine, large intestine, and anus. Both mechanical and chemical digestion occur through the actions of teeth/muscles and enzymes. The liver, gallbladder, and pancre
Skeletal, skin, muscle. nervous ppt
The document describes several key body systems including the skeletal, muscular, integumentary, and nervous systems. It explains that cells combine to form tissues, tissues combine to form organs, and organs work together in organ systems to carry out important body functions. The skeletal system provides structure and support, while storing minerals. The muscular system allows for movement via muscles connecting to bones. The integumentary system acts as a protective barrier for the body with the skin, hair, and nails. Lastly, the nervous system collects and processes information as the command center of the body using electrical signals transmitted through the brain and nerves.
Invertebrates
This document summarizes key characteristics of invertebrate animals. It describes their structures and functions including systems for digestion, respiration, circulation, excretion, response, movement, and reproduction. Specific phyla are examined in more detail, including worms, mollusks, arthropods, and echinoderms. Evolutionary trends are discussed such as the development of specialized cells/tissues, body symmetry, cephalization, segmentation, and a coelom.
Invertebrates modified 1 10-18
This document discusses the structure and function of various invertebrate phyla including annelids, mollusks, and insects. It outlines key characteristics like segmented bodies in annelids, soft bodies with shells in mollusks, and three-part bodies in insects. The document also covers evolutionary trends in early invertebrates from soft bodied to forms with shells and skeletons. Additionally, it describes trends in digestion, respiration, circulation, excretion, response, movement, reproduction, and skeletal systems across invertebrate groups.
Mitosis and meiosis
Cells divide through the process of cell division in order to replicate DNA and distribute it equally between daughter cells. Cell division involves mitosis, where the nucleus divides, and cytokinesis, where the cytoplasm divides. Mitosis consists of prophase, metaphase, anaphase, and telophase where chromosomes replicate and separate. Cytokinesis then divides the cell into two identical daughter cells each with a full set of chromosomes. Meiosis produces gametes through two rounds of division resulting in four haploid cells with half the number of chromosomes. This ensures genetic variation in sexual reproduction.
Mitosis and meiosis
Cells divide through the process of cell division in order to replicate DNA and distribute it equally between daughter cells. Cell division involves mitosis, where the nucleus divides, and cytokinesis, where the cytoplasm divides. Mitosis consists of prophase, metaphase, anaphase, and telophase where chromosomes replicate and separate. Cytokinesis then divides the cell into two identical daughter cells each with a full set of chromosomes. Meiosis produces gametes through two rounds of division resulting in four haploid cells with half the number of chromosomes. This ensures genetic variation in sexual reproduction.
Genetics
Gregor Mendel studied traits in pea plants such as color and height. He found that traits are controlled by alleles - dominant alleles will be expressed over recessive alleles in the first generation. Through subsequent generations and self-pollination, he discovered that recessive traits can be expressed according to his laws of inheritance and principles of dominance and segregation. Mendel's experiments laid the foundations for modern genetics.
DNA and RNA
This document discusses the history and key discoveries related to DNA and genetics. It covers:
- Griffith and Avery's early experiments showing DNA carries genetic information between generations
- Watson and Crick developing the double helix model of DNA structure
- DNA replication following Chargaff's rules of base pairing between A=T and G=C
- RNA and protein synthesis through transcription and translation of DNA into mRNA and proteins
- Types of mutations like point mutations, chromosomal mutations, and their harmful or beneficial effects
Cells
Cell theory states that all living things are composed of cells, cells are the basic units of structure and function, and new cells are produced from existing cells. There are two main types of cells - prokaryotic cells which lack a nucleus and eukaryotic cells which contain a nucleus. Organelles in cells such as the nucleus, mitochondria, chloroplasts, endoplasmic reticulum, golgi apparatus, lysosomes, and vacuoles each have specific functions that allow the cell to carry out its activities.
Cells
Cell theory states that all living things are composed of cells, cells are the basic units of structure and function, and new cells are produced from existing cells. There are two main types of cells - prokaryotic cells which lack a nucleus and eukaryotic cells which have a nucleus containing DNA. Organelles in cells such as the nucleus, mitochondria, chloroplasts, endoplasmic reticulum, golgi apparatus, lysosomes, and vacuoles each have specific functions that allow the cell to carry out its activities.
Characteristic of life
This document discusses the key characteristics of living things such as cells, DNA, metabolism, homeostasis, and response to stimuli. It also covers the four main types of organic compounds that make up living things: carbohydrates, lipids, nucleic acids, and proteins. Additionally, it provides information on chemistry of life, enzymes, viruses, bacteria, germ theory, and methods of disease transmission and prevention.
Chapter 9
Cellular respiration involves three main stages - glycolysis, the Krebs cycle, and the electron transport chain - to break down glucose and generate energy in the form of ATP. Glycolysis breaks down glucose and produces some ATP. The Krebs cycle further breaks down these products and generates more ATP and electron carriers. Finally, the electron transport chain uses these electron carriers to generate most of the cell's ATP through oxidative phosphorylation.
Chapter 8
Photosynthesis has two main stages: the light-dependent reaction uses light energy to produce ATP and NADPH, while the light-independent Calvin Cycle uses these products to incorporate CO2 into organic compounds like glucose. Key events in the history of photosynthesis research include the discoveries that plants require water, produce oxygen, and need light to carry out the process. The overall equation is: 6CO2 + 6H2O + light energy → C6H12O6 + 6O2.
Chapter 8
Photosynthesis has two main stages: the light-dependent reaction uses light energy to produce ATP and NADPH, while the light-independent Calvin Cycle uses these products to incorporate CO2 into organic compounds like glucose. Key events in photosynthesis history include discoveries that plants require water, produce oxygen, and need light to do so. The overall reaction is: 6CO2 + 6H2O + light energy → C6H12O6 + 6O2.
Evolution
- Charles Darwin proposed the theory of evolution through natural selection in 1859 after observing species variation on the Galapagos Islands. His theory built upon earlier ideas from scientists like Jean-Baptiste Lamarck and Thomas Malthus.
- Evolution occurs as inherited traits increase the chances of survival and reproduction in an organism's environment through natural selection and adaptation over many generations. The fossil record provides evidence of how species have changed over time.
- The earliest life on Earth was microbial and existed in the oceans around 3.8 billion years ago. Oxygen levels increased around 2.2 billion years ago allowing complex eukaryotic cells and later multi-cellular organisms to evolve. Major extinction events punctuated this pattern
Ecology
The document summarizes key concepts in ecology. It discusses the biosphere and how ecologists study relationships between individuals, populations, communities, ecosystems, and the entire biosphere. It then covers the basic methods used in ecological research - observing, experimenting, and modeling. It explains energy flow through ecosystems via photosynthesis and food chains. Matter is recycled through biogeochemical cycles like the water, carbon, and nitrogen cycles. The document also describes the abiotic and biotic factors that determine ecosystems and biomes, as well as population growth patterns.
Classifications
This document provides an overview of biological classification systems and kingdoms. It discusses how biologists classify organisms based on visible similarities and evolutionary relationships. Organisms are grouped in a hierarchical system with seven main levels from most specific (species) to most general (kingdom). There are currently six recognized kingdoms - Animalia, Plantae, Fungi, Protista, Archaea, and Bacteria. Molecular comparisons of DNA are also used to determine evolutionary relationships and estimate times of species divergence. The key kingdoms are described in terms of their basic characteristics.
Taxonomy, Classifications
This document provides an overview of biological classification systems and kingdoms. It discusses:
1) Carolus Linnaeus' hierarchical classification system with 7 levels (species to kingdom); organisms were grouped based on visible similarities.
2) Evolutionary classification groups organisms based on evolutionary relationships and derived characters rather than just physical similarities.
3) Current systems recognize 6 kingdoms - Animalia, Plantae, Fungi, Protista, Archaea, and Bacteria. DNA comparisons help determine evolutionary relationships.
4) The kingdoms are described in brief, highlighting key distinguishing features of plants, animals, fungi, and protists.
More from tracyconover (20)
Recently uploaded
Accounting for Restricted Grants When and How To Record Properly
In this webinar, member learned how to stay in compliance with generally accepted accounting principles (GAAP) for restricted grants.
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as discipline
How to Manage Reception Report in Odoo 17
A business may deal with both sales and purchases occasionally. They buy things from vendors and then sell them to their customers. Such dealings can be confusing at times. Because multiple clients may inquire about the same product at the same time, after purchasing those products, customers must be assigned to them. Odoo has a tool called Reception Report that can be used to complete this assignment. By enabling this, a reception report comes automatically after confirming a receipt, from which we can assign products to orders.
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 8 - CẢ NĂM - FRIENDS PLUS - NĂM HỌC 2023-2024 (B...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 8 - CẢ NĂM - FRIENDS PLUS - NĂM HỌC 2023-2024 (B...Nguyen Thanh Tu Collection
https://app.box.com/s/nrwz52lilmrw6m5kqeqn83q6vbdp8yzpHow Barcodes Can Be Leveraged Within Odoo 17
In this presentation, we will explore how barcodes can be leveraged within Odoo 17 to streamline our manufacturing processes. We will cover the configuration steps, how to utilize barcodes in different manufacturing scenarios, and the overall benefits of implementing this technology.
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"National Information Standards Organization (NISO)
This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
skeleton System.pdf (skeleton system wow)
🔥🔥🔥🔥🔥🔥🔥🔥🔥
إضغ بين إيديكم من أقوى الملازم التي صممتها
ملزمة تشريح الجهاز الهيكلي (نظري 3)
💀💀💀💀💀💀💀💀💀💀
تتميز هذهِ الملزمة بعِدة مُميزات :
1- مُترجمة ترجمة تُناسب جميع المستويات
2- تحتوي على 78 رسم توضيحي لكل كلمة موجودة بالملزمة (لكل كلمة !!!!)
#فهم_ماكو_درخ
3- دقة الكتابة والصور عالية جداً جداً جداً
4- هُنالك بعض المعلومات تم توضيحها بشكل تفصيلي جداً (تُعتبر لدى الطالب أو الطالبة بإنها معلومات مُبهمة ومع ذلك تم توضيح هذهِ المعلومات المُبهمة بشكل تفصيلي جداً
5- الملزمة تشرح نفسها ب نفسها بس تكلك تعال اقراني
6- تحتوي الملزمة في اول سلايد على خارطة تتضمن جميع تفرُعات معلومات الجهاز الهيكلي المذكورة في هذهِ الملزمة
واخيراً هذهِ الملزمة حلالٌ عليكم وإتمنى منكم إن تدعولي بالخير والصحة والعافية فقط
كل التوفيق زملائي وزميلاتي ، زميلكم محمد الذهبي 💊💊
🔥🔥🔥🔥🔥🔥🔥🔥🔥
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
Richard Seddon, George Grey,
Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
Benner "Expanding Pathways to Publishing Careers"
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
CapTechTalks Webinar Slides June 2024 Donovan Wright.pptx
Slides from a Capitol Technology University webinar held June 20, 2024. The webinar featured Dr. Donovan Wright, presenting on the Department of Defense Digital Transformation.
CHUYÊN ĐỀ ÔN TẬP VÀ PHÁT TRIỂN CÂU HỎI TRONG ĐỀ MINH HỌA THI TỐT NGHIỆP THPT ...
CHUYÊN ĐỀ ÔN TẬP VÀ PHÁT TRIỂN CÂU HỎI TRONG ĐỀ MINH HỌA THI TỐT NGHIỆP THPT ...Nguyen Thanh Tu Collection
https://app.box.com/s/qspvswamcohjtbvbbhjad04lg65waylfHow to Download & Install Module From the Odoo App Store in Odoo 17
Custom modules offer the flexibility to extend Odoo's capabilities, address unique requirements, and optimize workflows to align seamlessly with your organization's processes. By leveraging custom modules, businesses can unlock greater efficiency, productivity, and innovation, empowering them to stay competitive in today's dynamic market landscape. In this tutorial, we'll guide you step by step on how to easily download and install modules from the Odoo App Store.
NIPER 2024 MEMORY BASED QUESTIONS.ANSWERS TO NIPER 2024 QUESTIONS.NIPER JEE 2...
NIPER JEE PYQ
NIPER JEE QUESTIONS
MOST FREQUENTLY ASK QUESTIONS
NIPER MEMORY BASED QUWSTIONS
Recently uploaded (20)
Accounting for Restricted Grants When and How To Record Properly
Accounting for Restricted Grants When and How To Record Properly
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
spot a liar (Haiqa 146).pptx Technical writhing and presentation skills
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
Geography as a Discipline Chapter 1 __ Class 11 Geography NCERT _ Class Notes...
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 8 - CẢ NĂM - FRIENDS PLUS - NĂM HỌC 2023-2024 (B...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 8 - CẢ NĂM - FRIENDS PLUS - NĂM HỌC 2023-2024 (B...
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Jemison, MacLaughlin, and Majumder "Broadening Pathways for Editors and Authors"
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
CapTechTalks Webinar Slides June 2024 Donovan Wright.pptx
CapTechTalks Webinar Slides June 2024 Donovan Wright.pptx
CHUYÊN ĐỀ ÔN TẬP VÀ PHÁT TRIỂN CÂU HỎI TRONG ĐỀ MINH HỌA THI TỐT NGHIỆP THPT ...
CHUYÊN ĐỀ ÔN TẬP VÀ PHÁT TRIỂN CÂU HỎI TRONG ĐỀ MINH HỌA THI TỐT NGHIỆP THPT ...
How to Download & Install Module From the Odoo App Store in Odoo 17
How to Download & Install Module From the Odoo App Store in Odoo 17
NIPER 2024 MEMORY BASED QUESTIONS.ANSWERS TO NIPER 2024 QUESTIONS.NIPER JEE 2...
NIPER 2024 MEMORY BASED QUESTIONS.ANSWERS TO NIPER 2024 QUESTIONS.NIPER JEE 2...
Acids and bases
- 1. Acids • Most acids start with the element H, hydrogen – EX: HCl (hydrochloric acid), H2SO4 (sulfuric acid) • Any compound that increases the number of hydronium ions, (H+ ), when dissolved in water is an acid
- 2. Properties • NEVER TASTE, SMELL OR TOUCH ACIDS • Has sour taste (think vinegar or lemons) • Corrosive – destroys body tissue, clothing and other materials • React with some metals to produce hydrogen gas • Conduct electricity • Most widely made acid H2SO4
- 3. • Common uses of acids • Make paper • Paint • Detergents • Fertilizer • HCl common uses • Separating metals • Swimming pools to stop algae
- 4. Bases • Most bases end with OH- , a hydroxide ion, when dissolved in water • NEVER TASTE, SMELL OR TOUCH BASE • Has bitter taste and slippery feel (think soap) • Corrosive properties • Conducts electric current
- 5. • Commons uses of bases – Make soap – Make paper – Oven cleaner – Drain cleaner – Household cleaners (windex, ammonia) – Antacids (treat heartburn – rolaids or tums)
- 6. Strong -vs- Weak Acids • Strong acids will have additional Hydrogen (H+ ) molecules in the compound • All of the Hydrogen molecules break apart when dissolved in water
- 7. Strong -vs- Weak base • Strong bases will have additional hydroxide (OH- ), molecules in the compound • All of the molecules of a base break apart when dissolved in water and produce hydroxide ions
- 8. Salts • Large group of compounds with similar properties (usually formed with elements in group 17, halogens) • Neutralization reaction - a reaction between an acid and a base, salt and water are produced • NaOH + HCl → NaCl + H2O Base + Acid → Salt + water
- 9. • Indicators are use to identify acids and bases – litmus paper • pH scale is used to determine if an acid or base is strong or weak (compared to other acids and bases) REMEMBER ALL ACIDS AND BASES ARE DANGEROUS • 7 on the pH scale is neutral (H2O) • Bases have a pH greater than 7 • Acids have a pH less than 7.
- 10. The pH Scale