Introacidsandbases 130416101155-phpapp02
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This document defines acids and bases and their key characteristics. Acids release H+ ions in water and have sour tastes, react with metals, and contain hydrogen. Strong acids completely dissociate into H+ ions while weak acids only partially dissociate. Common strong acids include sulfuric acid and hydrochloric acid. Bases release OH- ions in water and usually taste bitter and feel slippery. Strong bases contain hydroxide ions and are also corrosive. When acids and bases react through neutralization, they form water and a salt like NaCl. The pH scale measures the concentration of H+ ions in a solution, with lower pH indicating more H+ ions.
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9TH STD SCIENCE MAHARASHTRA
Acids, Bases and Salts
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Source:9th text book of science mh
Acids and Bases
The document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). It lists examples of acids and bases and discusses their characteristics, including their effect on pH. It also discusses factors that affect reaction rates and methods for testing whether a substance is acidic or basic, such as pH indicators and the litmus test.
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This document defines key terms related to solutions and concentration, including solute, solvent, solution, and concentration. It discusses different units used to express concentration, such as grams per liter and molarity. The document also explains that acids and bases dissociate in water, releasing H+ and OH- ions, and that the pH scale measures the concentration of H+ ions from 0 to 14, with pH 7 being neutral. Common methods to determine pH are then listed.
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This document provides information about acids and bases for a Year 10 chemistry class. It defines acids and bases, gives examples of common acids and bases, and describes how to test substances as acids or bases using indicators like litmus paper. It also discusses acid-base reactions, acid rain, testing gases, and factors that affect reaction rates. Experiments are described for investigating indicators, reactions with acids, evaporation, and using Benedict's solution to test for glucose.
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1) When acids or bases dissolve in water, they dissociate or break apart into ions. For acids, this takes the form HA + H2O ⇌ A- + H3O+.
2) Strong acids and bases dissociate completely in water, forming a high concentration of ions. Weak acids and bases only partially dissociate, forming a low concentration of ions.
3) A titration experiment determines the concentration of an unknown solution by neutralizing it with a solution of known concentration and tracking the equivalence point where [H+] = [OH-].
Sandeep ppt on acids, bases and salts for vii
This document discusses acids and bases. It defines acids as sour tasting substances that produce hydrogen ions and turn litmus red. Common acids include those found in vinegar, citrus fruits, and other foods. Bases are defined as bitter tasting and soapy substances that turn litmus blue. Common bases include baking soda, detergents, and antacids. The document also explains how litmus paper can be used as a natural indicator to test whether a substance is acidic or basic by changing color.
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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.
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For B.Ed
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Educational reference
Research
Source:9th text book of science mh
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The document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). It lists examples of acids and bases and discusses their characteristics, including their effect on pH. It also discusses factors that affect reaction rates and methods for testing whether a substance is acidic or basic, such as pH indicators and the litmus test.
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Neutralization.
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This document defines key terms related to solutions and concentration, including solute, solvent, solution, and concentration. It discusses different units used to express concentration, such as grams per liter and molarity. The document also explains that acids and bases dissociate in water, releasing H+ and OH- ions, and that the pH scale measures the concentration of H+ ions from 0 to 14, with pH 7 being neutral. Common methods to determine pH are then listed.
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This document provides information about acids and bases for a Year 10 chemistry class. It defines acids and bases, gives examples of common acids and bases, and describes how to test substances as acids or bases using indicators like litmus paper. It also discusses acid-base reactions, acid rain, testing gases, and factors that affect reaction rates. Experiments are described for investigating indicators, reactions with acids, evaporation, and using Benedict's solution to test for glucose.
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1) When acids or bases dissolve in water, they dissociate or break apart into ions. For acids, this takes the form HA + H2O ⇌ A- + H3O+.
2) Strong acids and bases dissociate completely in water, forming a high concentration of ions. Weak acids and bases only partially dissociate, forming a low concentration of ions.
3) A titration experiment determines the concentration of an unknown solution by neutralizing it with a solution of known concentration and tracking the equivalence point where [H+] = [OH-].
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This document discusses acids and bases. It defines acids as sour tasting substances that produce hydrogen ions and turn litmus red. Common acids include those found in vinegar, citrus fruits, and other foods. Bases are defined as bitter tasting and soapy substances that turn litmus blue. Common bases include baking soda, detergents, and antacids. The document also explains how litmus paper can be used as a natural indicator to test whether a substance is acidic or basic by changing color.
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.
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This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
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Acids and bases can be identified by their names or chemical formulas. Acids contain hydrogen (H) or a carboxyl group (COOH) and have a pH below 7. Bases contain a metallic or ammonium ion and hydroxide (OH) and have a pH above 7. Acid-base indicators change color at specific pH levels and can be used to determine if a solution is acidic or basic. A neutralization reaction occurs between an acid and base, producing water and a salt.
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This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures hydrogen ion concentration and indicates whether a substance is acidic, basic, or neutral. Acid rain occurs when atmospheric pollutants like sulfur and nitrogen oxides dissolve in water to form strong acids. Some substances can act as both acids and bases and are called amphoteric or amphiprotic.
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1. The document discusses acid-base reactions and how salts can affect pH.
2. Salts containing conjugate acids of weak bases or conjugate bases of weak acids can change the pH, making solutions acidic or basic respectively.
3. Group 1 and 2 metal ions like Li+ and Mg2+ do not affect pH, except for Be2+ which makes solutions acidic. Metals with 3+ charges or higher often hydrolyze to form acidic solutions.
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The ph scale
The pH scale measures how acidic or alkaline a substance is on a scale from 0 to 14. A pH below 7 is acidic, above 7 is alkaline, and 7 is neutral. Universal indicator changes color depending on the pH, allowing it to indicate whether a substance is acidic, alkaline, or neutral. Litmus paper also changes color, with acids turning it red and bases turning it blue, providing a simple test to distinguish between acids and bases.
Acids, bases, & salts
Acids have a pH below 7 and donate hydrogen ions in solution. They react with bases and metals. Common acids include hydrochloric acid and citric acid. Bases have a pH above 7 and accept hydrogen ions, feeling slippery. Common bases are sodium hydroxide and ammonia. When an acid and base react, they form a salt and water. Salts are neutral and composed of the ions of the original acid and base. The digestive system uses acids and bases to break down foods, with acid in the stomach and bases in the intestines.
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The document discusses acid-base titration, including the analyte, standard, neutralization reaction, equivalence point, and procedure. It explains that an acid-base titration involves titrating an acid with a base until the moles of H+ equal the moles of OH-. It also discusses using a pH sensor and indicator to determine the equivalence point, and using stoichiometry to calculate unknown concentrations from experimental data.
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1. The document discusses acids and bases, including their definitions and properties.
2. An acid is defined as a proton donor, donating hydrogen ions (H+) in water. A base is a proton acceptor, accepting hydrogen ions.
3. Common strong acids include hydrochloric acid (HCl), nitric acid (HNO3), and sulfuric acid (H2SO4) which fully ionize in water.
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The document discusses acids and bases according to different definitions. The Arrhenius definition defines acids as substances that increase the concentration of hydronium ions and bases as substances that increase the concentration of hydroxide ions in a solution. The Brønsted-Lowry definition is broader, defining acids as substances that donate protons and bases as substances that accept protons. Amphoteric substances can act as both acids and bases, while amphiprotic substances are acids and bases according to the Brønsted-Lowry definition. The document also discusses acid-base reactions, the pH scale, and titrations.
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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.
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This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in aqueous solutions, with a pH range of 0-7. Bases, also called alkalines, produce hydroxide ions (OH-) in aqueous solutions with a pH range of 7-14. A pH of 7 indicates a neutral substance. The goals are to determine the differences between acids and bases, discuss their importance, and perform an experiment testing the pH of various substances.
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Acids are substances that are sour, such as lemon juice and vinegar, and are known as acidic. Bases are the opposite of acids and can also be corrosive, while alkalis are bases that are soluble in water. The litmus test and pH scale are used to determine whether a substance is an acid or base and the strength of acids and bases.
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Acids are substances that donate protons (H+) in aqueous solutions, increasing the concentration of H+ ions. Common acids include HCl, HNO3, and HC2H3O2. Bases are substances that accept H+ ions, producing hydroxide (OH-) ions when dissolved in water. Common bases include NaOH, KOH, and Ca(OH)2. Strong acids and bases are completely ionized in solution, while weak acids and bases are only partially ionized. The strength of an acid or base determines how reactive it is.
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This document discusses acids and bases, including their properties and how to test for them. It provides information on:
- The pH scale ranges from 0-14, with acids having lower values and bases having higher values. A pH of 7 is neutral.
- Acids donate H+ ions in solution and have a pH below 7. Bases donate OH- ions and have a pH above 7.
- Indicators like litmus paper and cabbage juice can be used to test if a substance is acidic or basic - acids turn indicators one color while bases turn them another.
- Common household substances like lemon juice, vinegar, baking soda and bleach are identified along the pH scale.
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This document provides an introduction to acids and bases, including:
1) How acids and bases are defined according to the Arrhenius, Bronsted-Lowry, and Lewis theories. Acids donate protons while bases accept protons.
2) Examples of strong acids like HCl and weak acids like acetic acid. Strong acids fully dissociate in water while weak acids only partially dissociate.
3) The pH scale measures hydrogen ion concentration from 0-14, with lower values being more acidic and higher more basic. Neutral solutions have a pH of 7.
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The document discusses key concepts about solutions including:
- The components of a solution are a solvent and one or more solutes. Common solvents include water and gases.
- Factors that affect solubility and the rate of dissolving include temperature, agitation, and surface area of the solute. Increasing these factors generally increases solubility.
- Solutions can be classified as saturated, unsaturated, or supersaturated depending on the amount of solute dissolved compared to the maximum amount possible at a given temperature.
- Solubility is also affected by properties of the solute molecules like polarity, charge, and size - more polar or charged molecules or smaller ions tend to be more soluble.
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Acids Bases and Salts
Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Common strong acids include sulfuric acid and hydrochloric acid, while strong bases include lithium hydroxide and sodium hydroxide. When acids and bases are mixed, they neutralize each other through a reaction that produces water and a salt. Indicators change color depending on whether the solution is acidic or basic, and can be used to measure the pH of a solution.
Acids, bases, & salts
This document discusses acids, bases, and salts. It defines acids as having a pH less than 7 and forming H+ ions in solution, and bases as having a pH greater than 7 and forming OH- ions in solution. Acids are classified as weak or strong depending on how completely they ionize in water. Common acids include hydrochloric acid, sulfuric acid, and acetic acid. Bases are also classified as weak or strong. Common bases include sodium hydroxide, magnesium hydroxide, and ammonium hydroxide. A salt is formed when an acid and base react, consisting of the negative ion from the acid and positive ion from the base.
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This document discusses the properties and reactions of acids and bases. It states that acids have a sour taste and cause color changes in indicators like litmus. Acids react with metals to produce hydrogen gas and with carbonates to produce carbon dioxide gas. Bases have a bitter taste and feel slippery. Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. The Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Water can act as both an acid and a base depending on the reaction.
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Acids and bases can be identified by their names or chemical formulas. Acids contain hydrogen (H) or a carboxyl group (COOH) and have a pH below 7. Bases contain a metallic or ammonium ion and hydroxide (OH) and have a pH above 7. Acid-base indicators change color at specific pH levels and can be used to determine if a solution is acidic or basic. A neutralization reaction occurs between an acid and base, producing water and a salt.
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This document provides an introduction to acids, bases, and salts for GCSE chemistry students. It discusses key topics like acidity and alkalinity, indicators, the pH scale, types of acids including strong and weak acids, and various methods for making salts through reactions between acids and metals, metal oxides, metal carbonates, metal hydroxides, and ammonia. The document is intended to help students understand and revise these core chemistry concepts in preparation for their exams.
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This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Strong acids and bases completely dissociate in water, while weak acids and bases only partially dissociate. The pH scale measures hydrogen ion concentration and indicates whether a substance is acidic, basic, or neutral. Acid rain occurs when atmospheric pollutants like sulfur and nitrogen oxides dissolve in water to form strong acids. Some substances can act as both acids and bases and are called amphoteric or amphiprotic.
Tang 06 salt acid-base 2
1. The document discusses acid-base reactions and how salts can affect pH.
2. Salts containing conjugate acids of weak bases or conjugate bases of weak acids can change the pH, making solutions acidic or basic respectively.
3. Group 1 and 2 metal ions like Li+ and Mg2+ do not affect pH, except for Be2+ which makes solutions acidic. Metals with 3+ charges or higher often hydrolyze to form acidic solutions.
Acid & Base - Physical Chemistry Presentation
Slide show of the topic Acid & Base as a part of the assignment in our Physical Chemistry course.
Created by: Annisa Hayatunnufus
Bachelor of Pharmacy
Management & Science University
The ph scale
The pH scale measures how acidic or alkaline a substance is on a scale from 0 to 14. A pH below 7 is acidic, above 7 is alkaline, and 7 is neutral. Universal indicator changes color depending on the pH, allowing it to indicate whether a substance is acidic, alkaline, or neutral. Litmus paper also changes color, with acids turning it red and bases turning it blue, providing a simple test to distinguish between acids and bases.
Acids, bases, & salts
Acids have a pH below 7 and donate hydrogen ions in solution. They react with bases and metals. Common acids include hydrochloric acid and citric acid. Bases have a pH above 7 and accept hydrogen ions, feeling slippery. Common bases are sodium hydroxide and ammonia. When an acid and base react, they form a salt and water. Salts are neutral and composed of the ions of the original acid and base. The digestive system uses acids and bases to break down foods, with acid in the stomach and bases in the intestines.
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The document discusses acid-base titration, including the analyte, standard, neutralization reaction, equivalence point, and procedure. It explains that an acid-base titration involves titrating an acid with a base until the moles of H+ equal the moles of OH-. It also discusses using a pH sensor and indicator to determine the equivalence point, and using stoichiometry to calculate unknown concentrations from experimental data.
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1. The document discusses acids and bases, including their definitions and properties.
2. An acid is defined as a proton donor, donating hydrogen ions (H+) in water. A base is a proton acceptor, accepting hydrogen ions.
3. Common strong acids include hydrochloric acid (HCl), nitric acid (HNO3), and sulfuric acid (H2SO4) which fully ionize in water.
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The document discusses acids and bases according to different definitions. The Arrhenius definition defines acids as substances that increase the concentration of hydronium ions and bases as substances that increase the concentration of hydroxide ions in a solution. The Brønsted-Lowry definition is broader, defining acids as substances that donate protons and bases as substances that accept protons. Amphoteric substances can act as both acids and bases, while amphiprotic substances are acids and bases according to the Brønsted-Lowry definition. The document also discusses acid-base reactions, the pH scale, and titrations.
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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.
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This presentation contains the important points for NCERT - Class 10 - Science - Chapter 2 - Acids, Bases and Salts
Acids & bases
This document discusses acids and bases. It defines acids as substances that produce hydrogen ions (H+) in aqueous solutions, with a pH range of 0-7. Bases, also called alkalines, produce hydroxide ions (OH-) in aqueous solutions with a pH range of 7-14. A pH of 7 indicates a neutral substance. The goals are to determine the differences between acids and bases, discuss their importance, and perform an experiment testing the pH of various substances.
Acids and bases power point
Acids are substances that are sour, such as lemon juice and vinegar, and are known as acidic. Bases are the opposite of acids and can also be corrosive, while alkalis are bases that are soluble in water. The litmus test and pH scale are used to determine whether a substance is an acid or base and the strength of acids and bases.
Acids and Bases
Acids are substances that donate protons (H+) in aqueous solutions, increasing the concentration of H+ ions. Common acids include HCl, HNO3, and HC2H3O2. Bases are substances that accept H+ ions, producing hydroxide (OH-) ions when dissolved in water. Common bases include NaOH, KOH, and Ca(OH)2. Strong acids and bases are completely ionized in solution, while weak acids and bases are only partially ionized. The strength of an acid or base determines how reactive it is.
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This document discusses acids and bases, including their properties and how to test for them. It provides information on:
- The pH scale ranges from 0-14, with acids having lower values and bases having higher values. A pH of 7 is neutral.
- Acids donate H+ ions in solution and have a pH below 7. Bases donate OH- ions and have a pH above 7.
- Indicators like litmus paper and cabbage juice can be used to test if a substance is acidic or basic - acids turn indicators one color while bases turn them another.
- Common household substances like lemon juice, vinegar, baking soda and bleach are identified along the pH scale.
- A
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This document provides an introduction to acids and bases, including:
1) How acids and bases are defined according to the Arrhenius, Bronsted-Lowry, and Lewis theories. Acids donate protons while bases accept protons.
2) Examples of strong acids like HCl and weak acids like acetic acid. Strong acids fully dissociate in water while weak acids only partially dissociate.
3) The pH scale measures hydrogen ion concentration from 0-14, with lower values being more acidic and higher more basic. Neutral solutions have a pH of 7.
19 solutions and solubility
The document discusses key concepts about solutions including:
- The components of a solution are a solvent and one or more solutes. Common solvents include water and gases.
- Factors that affect solubility and the rate of dissolving include temperature, agitation, and surface area of the solute. Increasing these factors generally increases solubility.
- Solutions can be classified as saturated, unsaturated, or supersaturated depending on the amount of solute dissolved compared to the maximum amount possible at a given temperature.
- Solubility is also affected by properties of the solute molecules like polarity, charge, and size - more polar or charged molecules or smaller ions tend to be more soluble.
- Solub
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Ncert class 10 - science - chapter 2 - acids, bases and salts
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Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Common strong acids include sulfuric acid and hydrochloric acid, while strong bases include lithium hydroxide and sodium hydroxide. When acids and bases are mixed, they neutralize each other through a reaction that produces water and a salt. Indicators change color depending on whether the solution is acidic or basic, and can be used to measure the pH of a solution.
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ACIDS AND BASES
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This document discusses the key characteristics and properties of acids and bases. It defines acids as substances that taste sour, feel rough, turn litmus paper red, and have a pH less than 7. Bases are defined as substances that taste bitter, feel slippery, turn litmus paper blue, and have a pH greater than 7. It then provides examples of common acids and bases and discusses the Arrhenius and Bronsted-Lowry theories of acids and bases in terms of proton donation and acceptance. Key reactions are given to illustrate these theories using common acids and bases like HCl, NH3, H2O, HCO3-.
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This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and bases as substances that produce OH- ions. Acids are classified as strong or weak depending on how fully they dissociate in water. Strong acids fully dissociate while weak acids only partially dissociate. The pH scale is used to measure acidity and alkalinity. Neutral solutions have a pH of 7 while acids have a pH less than 7 and bases have a pH greater than 7. Acid rain is caused by atmospheric pollutants like sulfur and nitrogen oxides dissolving in water to form acids. Some substances like carbonic acid and the amino acid glycine can act as both acids and bases, making
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This document discusses acids and bases. It defines acids as substances that produce hydrogen ions in water, and bases as substances that produce hydroxide ions in water. Strong acids and bases completely ionize, while weak ones only partially ionize. Neutral substances have equal concentrations of hydrogen and hydroxide ions. When acids and bases are mixed, they neutralize to form salts and water through balanced chemical reactions. pH indicators can be used to determine if a solution is acidic, basic, or neutral.
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1) Arrhenius defines acids as substances that yield hydrogen ions in water and bases as substances that yield hydroxide ions in water. Neutralization produces salt and water.
2) Bronsted-Lowry defines acids as proton donors and bases as proton acceptors. Neutralization involves the transfer of a proton from an acid to a base.
3) Lewis defines acids as electron pair acceptors and bases as electron pair donors. Neutralization involves the sharing of an electron pair between an acid and base.
Acid base and acid base titration
This chapter discusses acids and bases according to the Arrhenius and Brønsted-Lowry definitions. The Arrhenius definition states that acids are substances that produce hydronium ions (H3O+) in water and bases produce hydroxide ions (OH-). Brønsted-Lowry defines acids as proton donors and bases as proton acceptors. Both definitions are discussed along with their advantages and limitations. Strong and weak acids/bases are compared based on their extent of ionization in water. Neutralization reactions between acids and bases are outlined. Conjugate acid-base pairs are introduced in the context of Brønsted-Lowry acid-base reactions. Certain substances, called
acids-and-bases-lecture.ppt
1. There are three classes of strong electrolytes: strong acids, strong bases, and most water soluble salts. Weak acids and bases only partially dissociate in water.
2. pH is a measure of the concentration of hydrogen ions [H+] in a solution. Low pH indicates high [H+] and an acidic solution, while high pH indicates low [H+] and a basic solution. Household substances like coffee, milk, and baking soda have different pH values.
3. The acid dissociation constant Ka and base dissociation constant Kb are equilibrium constants that indicate the strength of an acid or base. Strong acids and bases fully dissociate while weak acids and bases only partially dissociate,
25 acids and bases
1. Acids are substances that liberate hydrogen ions (H+) when dissolved in water. Common acids include hydrochloric acid, nitric acid, and sulfuric acid.
2. Bases are substances that form hydroxide ions (OH-) when dissolved in water, such as sodium hydroxide and potassium hydroxide.
3. Acids and bases react through neutralization reactions, where hydrogen and hydroxide ions exchange partners to form water and a salt. This is illustrated by the reaction of sulfuric acid and calcium hydroxide to form calcium sulfate and water.
Acids and bases
This document discusses acids and bases. It defines acids as substances that produce H+ ions in water and have a pH less than 7. Acids have properties such as turning litmus red and reacting with metals. Bases are defined as substances that produce OH- ions in water and have a pH greater than 7. They have properties such as turning litmus blue and reacting with acids to form salt and water. Strong acids and bases are fully dissociated in water while weak acids and bases are only partially dissociated. The document also discusses Bronsted-Lowry and Lewis acid-base theories.
properties of acids base and the law given by scientists
All acid base concept for First Year B.pharm
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.
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Introacidsandbases 130416101155-phpapp02
- 2. Acid: A substance that releases H+ ions in an aqueous solution “aqueous” means: water
- 3. Characteristics of Acids: Acids have a sour taste Acids react with metals Acids contain Hydrogen Many are poisonous and corrosive to skin H
- 4. Strong Acids (break down completely to give off many H+ ions)
- 5. Weak Acids (only partially breaks down, gives less H+) Mark Bishop Acid animation
- 6. Common Acids: All others considered Weak (examples) Strong Acids The Formula Sulphuric acid Hydrochloric acid Hybrobromic acid Hydroiodic acid Nitric acid Perchloric acid H2 SO4 HCl HBr HI HNO3 HClO4 Acetic acid (vinegar) HC2H3O2 Carbonic acid HCO3 Weak Acid The Formula
- 7. Base: A substance that releases OH- ions in an aqueous solution
- 8. Characteristics of Bases: Bases usually taste bitter Bases feel slippery Bases contain hydroxide ions STRONG bases are also poisonous and corrosive to skin OH-
- 9. Strong Bases The Formulae Lithium hydroxide Sodium hydroxide Potassium hydroxide Rubidium hydroxide Caesium hydroxide Barium hydroxide Calcium hydroxide Strontium hydroxide LiOH NaOH KOH RbOH CsOH Ba(OH)2 Ca(OH)2 Sr(OH)2 Common Bases: (Hydroxides of Group 1 and Group 2 Metals are STRONG) All others are WEAK
- 10. Some bases (VERY FEW) don’t have OH- Most commonly: ammonia NH3
- 11. Reactions between acids and bases When and acid and a base react with each other, the characteristic properties of both are destroyed. This is called neutralization.
- 12. Reactions between acids and bases General formula for acid base reaction: Acid + Base → H2O + Salt “Salt” means any ionic compound formed from an acid/base reaction NOT JUST NaCl !! Neutralization Reaction Animation
- 13. Neutralization HCl + NaOH → H2O + NaCl acid base water salt
- 14. Neutralization Another Example HNO3 + KOH → H2O + KNO3 H OHKNO3 acid base water salt
- 15. Indicators An indicator is a compound that will change color in the presence of an acid or base Universal indicator (pH paper) Used for the full pH range Red Litmus-Turns blue in base Blue Litmus-Turns red in acid Phenolphthalein-Turns pink in base
- 16. pH pH stands for “potential hydrogen” and is a measure of how many H+ ions there are in solution. The MORE H+ there are, the LOWER the pH will be.
- 17. pH Scale Shows the range of H+ concentrations High H+ concentration Low H+ concentration