P h indicator
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The pH scale measures the concentration of hydrogen ions (H+) in a solution, with pH defined as the negative logarithm of the H+ concentration. The pH scale ranges from 0 to 14, with lower values indicating more acidic solutions and higher values indicating more alkaline or basic solutions. The concentration of H+ ions determines whether a solution is acidic, alkaline, or neutral. Common pH indicators change color depending on the pH level, allowing the acidity or alkalinity of solutions to be measured visually.
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![pH , pOH
pH : Negative
logarithm of
hydrogen ions
concentration
pH= -log[Hᶧ]
pOH : Negative
logarithm of hydroxyl
ions concentration
pOH= -log[pOHˉ]
10-Jan-17 ALINA SHERIN 2](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
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Indicators
This document discusses pH and indicators. It explains that pH is a measure of acidity or alkalinity on a scale from 0 to 14, with acids below 7 and alkalis above. It describes common tools to measure pH like pH papers, meters, and dataloggers. It also defines indicators as substances that change color based on pH and lists common natural and synthetic indicators like litmus, universal indicator, methyl orange, and phenolphthalein.
P h indicators
The document discusses pH indicators and their uses in titration. It provides information on the pH ranges and color changes of common acid-base indicators like methyl orange, methyl red and bromthymol blue. It also lists the ideal properties of pH sensors and describes how different indicators are used to titrate strong acids and bases or weak acids and bases. Common natural pH indicators from foods like red cabbage, beet and blueberries are also mentioned.
P h indicator
This experiment aims to make pH indicators from red cabbage and turmeric extracts and use them to test the pH of various household chemicals. Red cabbage extract changes color from pink in acidic solutions to purple and green in neutral and basic solutions respectively. Turmeric extract is yellow below pH 7.4 and red above pH 8.6. Using the indicators, vinegar and orange juice were found to be acidic, while toothpaste was found to be basic.
Indicator
This document defines and describes various types of indicators used to determine the acidity, alkalinity or redox state of a solution. It discusses natural indicators like turmeric and litmus, as well as artificial pH indicators like methyl orange and phenolphthalein. It also covers complexometric, adsorption and universal indicators, and provides examples of how different indicators are used to test solutions and determine the endpoint in titration reactions.
Ph indicator-----(Pharmaceutics)
pH indicators are organic compounds that change color based on the pH of a solution. They are used to check pH and indicate the endpoint of reactions. Common indicators include litmus, which is red below pH 4.5 and blue above pH 8.2, and phenolphthalein, which is colorless below pH 8.2 and pink above pH 10. In a demonstration, phenolphthalein was added to solutions containing sodium hydroxide, turning them pink, but when one solution was then mixed with acetic acid, the indicator turned colorless due to the drop in pH caused by neutralization.
Natural Indicator Preparation
"STUDY OFACID BASE INDICATOR PROPERTY FOR ETHANOLIC EXTRACT OF NERIUM INDICUM FLOWER ” SUBMITTED BY MISS. VAISHALI D. DANDGE B PHARM 3RD YEAR VI SEMESTER GUIDED BY DR. K. B. GABHANE Vidyabharati College Of Pharmacy, Amravati (2018-2019)
acid-base indicator and neutralization
Acid-base indicators change color based on pH, acting as weak acids or bases. Common indicators and their colors in acidic versus basic conditions are listed. Neutralization occurs when an acid and base react to form water and a salt, involving the combination of H+ and OH- ions. The pH of solutions formed from strong acid-strong base neutralization will be 7, while strong acid-weak base solutions will be less than 7 and strong base-weak acid will be greater than 7.
Acid base indicator
This document discusses acid-base indicators and their use in determining pH. It explains that pH indicators are weak acids that change color based on whether a solution is acidic or basic. The document outlines indicator ranges for common indicators like methyl orange and phenolphthalein. It also discusses how to choose the appropriate indicator based on whether the acid and base being titrated are strong or weak. Indicators are used to determine the equivalence point in acid-base titrations.
Recommended
Indicators
This document discusses pH and indicators. It explains that pH is a measure of acidity or alkalinity on a scale from 0 to 14, with acids below 7 and alkalis above. It describes common tools to measure pH like pH papers, meters, and dataloggers. It also defines indicators as substances that change color based on pH and lists common natural and synthetic indicators like litmus, universal indicator, methyl orange, and phenolphthalein.
P h indicators
The document discusses pH indicators and their uses in titration. It provides information on the pH ranges and color changes of common acid-base indicators like methyl orange, methyl red and bromthymol blue. It also lists the ideal properties of pH sensors and describes how different indicators are used to titrate strong acids and bases or weak acids and bases. Common natural pH indicators from foods like red cabbage, beet and blueberries are also mentioned.
P h indicator
This experiment aims to make pH indicators from red cabbage and turmeric extracts and use them to test the pH of various household chemicals. Red cabbage extract changes color from pink in acidic solutions to purple and green in neutral and basic solutions respectively. Turmeric extract is yellow below pH 7.4 and red above pH 8.6. Using the indicators, vinegar and orange juice were found to be acidic, while toothpaste was found to be basic.
Indicator
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Ph indicator-----(Pharmaceutics)
pH indicators are organic compounds that change color based on the pH of a solution. They are used to check pH and indicate the endpoint of reactions. Common indicators include litmus, which is red below pH 4.5 and blue above pH 8.2, and phenolphthalein, which is colorless below pH 8.2 and pink above pH 10. In a demonstration, phenolphthalein was added to solutions containing sodium hydroxide, turning them pink, but when one solution was then mixed with acetic acid, the indicator turned colorless due to the drop in pH caused by neutralization.
Natural Indicator Preparation
"STUDY OFACID BASE INDICATOR PROPERTY FOR ETHANOLIC EXTRACT OF NERIUM INDICUM FLOWER ” SUBMITTED BY MISS. VAISHALI D. DANDGE B PHARM 3RD YEAR VI SEMESTER GUIDED BY DR. K. B. GABHANE Vidyabharati College Of Pharmacy, Amravati (2018-2019)
acid-base indicator and neutralization
Acid-base indicators change color based on pH, acting as weak acids or bases. Common indicators and their colors in acidic versus basic conditions are listed. Neutralization occurs when an acid and base react to form water and a salt, involving the combination of H+ and OH- ions. The pH of solutions formed from strong acid-strong base neutralization will be 7, while strong acid-weak base solutions will be less than 7 and strong base-weak acid will be greater than 7.
Acid base indicator
This document discusses acid-base indicators and their use in determining pH. It explains that pH indicators are weak acids that change color based on whether a solution is acidic or basic. The document outlines indicator ranges for common indicators like methyl orange and phenolphthalein. It also discusses how to choose the appropriate indicator based on whether the acid and base being titrated are strong or weak. Indicators are used to determine the equivalence point in acid-base titrations.
Beetroot as an indicator
The document discusses the preparation and use of beetroot as a pH indicator. It describes how beetroot juice was prepared and its color change observed between pH 10.8-11.2, indicating its pH range. Various acid-base titrations were conducted using this indicator, finding it worked well for strong acid-strong base and weak acid-strong base titrations using 0.1M NaOH, but not for other titration types or more dilute bases. However, beetroot is not ideal for lab use due to needing preparation and having limited storage life.
chemical Indicators
Indicators are chemical substances that change color based on whether a solution is acidic or basic. Common acid-base indicators include litmus, methyl orange, and phenolphthalein. They change color at specific pH levels, allowing for the determination of a solution's acidity or basicity. Other types of indicators include universal indicators, which change color gradually over a wide pH range, olfactory indicators detected by smell, and redox indicators sensitive to oxidation-reduction reactions. Indicators find uses in titrations, testing soils and swimming pools, and monitoring wastes.
Theory of Indicators/choice of indicator/acid base indicator
1. Indicators are weak acids or bases that change color within a certain pH range and are used to determine the endpoint in acid-base titrations. Common indicators include methyl orange, methyl red, and phenolphthalein.
2. Two theories explain the color change of indicators: Ostwald's theory states it is due to ionization of the indicator, while the quinonoid theory states the indicator exists in different tautomeric forms with different colors.
3. The suitable indicator for a titration depends on the pH change curve near the endpoint - the indicator range should span the steep portion of the curve. Strong acid-strong base titrations can use methyl orange, methyl red,
pH indicator
The document defines pH as the negative logarithm of the hydrogen ion (H+) activity in a solution, with the pH scale ranging from 0 to 14. The hydrogen ions determine if a solution is acidic, alkaline, or neutral - if the hydrogen ion content is measured, the acidity or alkalinity can be determined. Water molecules dissociate into hydrogen and hydroxide ions through autoionization, affecting pH. pH indicators change color depending on the pH of a solution, allowing determination of acidity or alkalinity.
Indicators in Chemistry ll Acid-Base Indicators
Indicators are substances that change color based on pH levels in solutions, acting as visual indicators of acidity and alkalinity. They are usually weak acids or bases whose conjugate forms have different colors, allowing the pH of a solution to be determined visually. A pH indicator detects hydronium or hydrogen ions and causes the solution's color to change based on its pH value, with values below 7.0 indicating acidity and above indicating alkalinity, while a neutral solution has a pH of 7.0.
Theories of acid base indicators
The document discusses theories of acid-base indicators and their use. It describes the Ostwald theory which states that indicators exist in different colored acid and conjugate base forms and reach equilibrium based on solution pH. The resonance theory indicates color changes are due to tautomeric molecular structure changes. A table lists common indicators and their corresponding pH ranges and color changes, such as phenolphthalein changing from colorless to pink to red from pH 8.3 to 10.
Indicators
- Many acid-base indicators are weak acids that partially dissociate in solution, existing in both ionized and un-ionized forms which have different colors. In acidic solution, the equilibrium favors the un-ionized form which is typically red. In alkaline solution, the equilibrium favors the ionized blue form.
- Titration curves show characteristic shapes depending on whether the acid and base are strong or weak. A strong acid-strong base titration has an initial flat region followed by a sharp pH change at the equivalence point. A weak acid-strong base titration has a gradual pH change throughout.
- The suitable indicator for a titration must change color within the sharp pH change region near the
Theory of indicator
This document discusses the theory of acid-base indicators and their use in titrations. It explains that indicators change color within a certain pH range, with examples like methyl orange changing from pink to yellow between pH 3.2-4.5. Two theories are presented for how indicators work: Ostwald's theory, where color change is due to ionization, and the quinonoid theory, where indicators exist in different tautomeric forms with different colors. Phenolphthalein is used to illustrate Ostwald's theory, changing from colorless to pink as it ionizes more in alkaline conditions. Methyl orange is a weak base that changes from yellow to red depending on whether its ionized or unionized form
8. theory of indicators
This document discusses the theory of acid-base indicators used in titration reactions. It explains that indicators change color within a certain pH range, allowing determination of the endpoint. Two theories are presented: Ostwald's theory states that color change is due to ionization of the indicator, while quinonoid theory proposes the indicator exists in two tautomeric forms in equilibrium, with different colors. Common indicators like phenolphthalein and methyl orange are discussed in the context of the two theories.
Acid base titrations & nat unit 2 pa
This document discusses acid-base titration curves. It defines strong and weak acids/bases, and their degree of dissociation. Titration is introduced as a technique used to determine the concentration of an unknown solution by titrating it with a solution of known concentration. The key concepts of equivalence point, indicators, and different types of titration curves are explained. Titration curves are plotted as pH vs volume of titrant added. Examples are given of titration curves for strong acid-strong base, weak acid-strong base, and strong acid-weak base titrations.
Theory of Indicators.pptx
1. Indicators are substances that change color in response to chemical reactions, especially titrations, allowing the determination of an endpoint.
2. There are three types of indicators: self-indicators that change color on their own, internal indicators that participate in the reaction, and external indicators that do not participate but still change color at the endpoint.
3. Indicator color changes are explained by two theories: Ostwald's theory of ionization states that indicators are weak acids or bases whose color depends on whether they are ionized or not. The quinonoid theory proposes that indicators exist in colored or colorless tautomeric forms that interchange depending on pH.
Acid base titrations
The document discusses acid-base titrations, which are procedures used to determine the concentration of an acid or base by titrating with the other substance until reaching the equivalence point where moles of H3O+ and OH- are equal, signaling the end point where an indicator changes color and all the acid or base has been neutralized, forming water and a salt. It also examines the pH ranges that different acid-base indicators change color, types of acid-base reactions, and examples of strong vs. weak acid-base titrations.
Non aq. acid base titration
Non aqueous titration refers to a type of titration in which the analyte substance is dissolved in a solvent which does not contain water. This procedure is a very important one in pharmacopoeial assays.
Indicators
The document discusses acids and bases that are commonly found in households. It explains that acids have a sour taste and are corrosive, providing examples like lemon juice, vinegar, hydrochloric acid, and sulfuric acid. Acids react with metals to form salts and hydrogen, and with carbonates to form salts, carbon dioxide, and water. Bases or alkalis, like sodium hydroxide and calcium hydroxide, feel soapy and are corrosive. The document also introduces pH as a measure of acidity and alkalinity on a scale of 1-14, and mentions common acid-base indicators like litmus and universal indicator that change color over different pH ranges.
Titration introduction
An introduction to titration--why we use it, the advantage of water solution chemistry, and acid-base, conductimetric and redox titrations.
ACID BASE TITRATION
This document provides an overview of acid-base titration and summarizes the key steps and considerations when performing a titration. It discusses selecting an appropriate indicator based on the relative strengths of the acid and base, performing multiple titrations to determine the endpoint accurately, and calculating pH at different points during the titration, including the initial pH, pH before and at the equivalence point, and pH after the equivalence point. Formulas are provided for calculating pH at these different stages of a titration, whether it involves a strong acid-strong base, strong acid-weak base, or weak acid-strong base reaction.
IB Chemistry on Acid Base Indicators and Salt Hydrolysis
- Acid-base indicators change color at their pKa value due to the equilibrium between their acid and conjugate base forms.
- Common indicators and their pKa values and color changes are listed. Methyl orange changes from red to yellow at pH 3.46.
- For an indicator to be suitable in a titration, its color change must occur within the pH range at the equivalence point where amount of acid equals amount of base.
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.
Non aq titrations unit 2
Non-aqueous titration has several advantages over aqueous titration:
1. Organic acids and bases insoluble in water can be soluble in non-aqueous solvents allowing them to be titrated.
2. A non-aqueous solvent may help separate two or more acids in a mixture so they can be titrated individually.
3. More substances can be titrated as the solubility and application ranges are enlarged for weak acids/bases that cannot be titrated in water.
Some common non-aqueous solvents used include acetic acid, acetonitrile, alcohols, DMF. Indicators suitable for specific titrations must be selected to indicate the endpoint
Acid base titration
An acid–base titration is the process which determines the concentration of an acid or base .Which exactly neutralize the acid or base with an acid or base of known concentration. Through acid base reactions Acid-Base titrations usually find the amount of a known acidic or basic substance. This enables the quantitative analysis of the concentration of an unknown acid or base solution. It work with following the neutralization reaction that occurs between acids and bases. To find percent purity of chemicals Acid–base titrations can also be used.
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Beetroot as an indicator
The document discusses the preparation and use of beetroot as a pH indicator. It describes how beetroot juice was prepared and its color change observed between pH 10.8-11.2, indicating its pH range. Various acid-base titrations were conducted using this indicator, finding it worked well for strong acid-strong base and weak acid-strong base titrations using 0.1M NaOH, but not for other titration types or more dilute bases. However, beetroot is not ideal for lab use due to needing preparation and having limited storage life.
chemical Indicators
Indicators are chemical substances that change color based on whether a solution is acidic or basic. Common acid-base indicators include litmus, methyl orange, and phenolphthalein. They change color at specific pH levels, allowing for the determination of a solution's acidity or basicity. Other types of indicators include universal indicators, which change color gradually over a wide pH range, olfactory indicators detected by smell, and redox indicators sensitive to oxidation-reduction reactions. Indicators find uses in titrations, testing soils and swimming pools, and monitoring wastes.
Theory of Indicators/choice of indicator/acid base indicator
1. Indicators are weak acids or bases that change color within a certain pH range and are used to determine the endpoint in acid-base titrations. Common indicators include methyl orange, methyl red, and phenolphthalein.
2. Two theories explain the color change of indicators: Ostwald's theory states it is due to ionization of the indicator, while the quinonoid theory states the indicator exists in different tautomeric forms with different colors.
3. The suitable indicator for a titration depends on the pH change curve near the endpoint - the indicator range should span the steep portion of the curve. Strong acid-strong base titrations can use methyl orange, methyl red,
pH indicator
The document defines pH as the negative logarithm of the hydrogen ion (H+) activity in a solution, with the pH scale ranging from 0 to 14. The hydrogen ions determine if a solution is acidic, alkaline, or neutral - if the hydrogen ion content is measured, the acidity or alkalinity can be determined. Water molecules dissociate into hydrogen and hydroxide ions through autoionization, affecting pH. pH indicators change color depending on the pH of a solution, allowing determination of acidity or alkalinity.
Indicators in Chemistry ll Acid-Base Indicators
Indicators are substances that change color based on pH levels in solutions, acting as visual indicators of acidity and alkalinity. They are usually weak acids or bases whose conjugate forms have different colors, allowing the pH of a solution to be determined visually. A pH indicator detects hydronium or hydrogen ions and causes the solution's color to change based on its pH value, with values below 7.0 indicating acidity and above indicating alkalinity, while a neutral solution has a pH of 7.0.
Theories of acid base indicators
The document discusses theories of acid-base indicators and their use. It describes the Ostwald theory which states that indicators exist in different colored acid and conjugate base forms and reach equilibrium based on solution pH. The resonance theory indicates color changes are due to tautomeric molecular structure changes. A table lists common indicators and their corresponding pH ranges and color changes, such as phenolphthalein changing from colorless to pink to red from pH 8.3 to 10.
Indicators
- Many acid-base indicators are weak acids that partially dissociate in solution, existing in both ionized and un-ionized forms which have different colors. In acidic solution, the equilibrium favors the un-ionized form which is typically red. In alkaline solution, the equilibrium favors the ionized blue form.
- Titration curves show characteristic shapes depending on whether the acid and base are strong or weak. A strong acid-strong base titration has an initial flat region followed by a sharp pH change at the equivalence point. A weak acid-strong base titration has a gradual pH change throughout.
- The suitable indicator for a titration must change color within the sharp pH change region near the
Theory of indicator
This document discusses the theory of acid-base indicators and their use in titrations. It explains that indicators change color within a certain pH range, with examples like methyl orange changing from pink to yellow between pH 3.2-4.5. Two theories are presented for how indicators work: Ostwald's theory, where color change is due to ionization, and the quinonoid theory, where indicators exist in different tautomeric forms with different colors. Phenolphthalein is used to illustrate Ostwald's theory, changing from colorless to pink as it ionizes more in alkaline conditions. Methyl orange is a weak base that changes from yellow to red depending on whether its ionized or unionized form
8. theory of indicators
This document discusses the theory of acid-base indicators used in titration reactions. It explains that indicators change color within a certain pH range, allowing determination of the endpoint. Two theories are presented: Ostwald's theory states that color change is due to ionization of the indicator, while quinonoid theory proposes the indicator exists in two tautomeric forms in equilibrium, with different colors. Common indicators like phenolphthalein and methyl orange are discussed in the context of the two theories.
Acid base titrations & nat unit 2 pa
This document discusses acid-base titration curves. It defines strong and weak acids/bases, and their degree of dissociation. Titration is introduced as a technique used to determine the concentration of an unknown solution by titrating it with a solution of known concentration. The key concepts of equivalence point, indicators, and different types of titration curves are explained. Titration curves are plotted as pH vs volume of titrant added. Examples are given of titration curves for strong acid-strong base, weak acid-strong base, and strong acid-weak base titrations.
Theory of Indicators.pptx
1. Indicators are substances that change color in response to chemical reactions, especially titrations, allowing the determination of an endpoint.
2. There are three types of indicators: self-indicators that change color on their own, internal indicators that participate in the reaction, and external indicators that do not participate but still change color at the endpoint.
3. Indicator color changes are explained by two theories: Ostwald's theory of ionization states that indicators are weak acids or bases whose color depends on whether they are ionized or not. The quinonoid theory proposes that indicators exist in colored or colorless tautomeric forms that interchange depending on pH.
Acid base titrations
The document discusses acid-base titrations, which are procedures used to determine the concentration of an acid or base by titrating with the other substance until reaching the equivalence point where moles of H3O+ and OH- are equal, signaling the end point where an indicator changes color and all the acid or base has been neutralized, forming water and a salt. It also examines the pH ranges that different acid-base indicators change color, types of acid-base reactions, and examples of strong vs. weak acid-base titrations.
Non aq. acid base titration
Non aqueous titration refers to a type of titration in which the analyte substance is dissolved in a solvent which does not contain water. This procedure is a very important one in pharmacopoeial assays.
Indicators
The document discusses acids and bases that are commonly found in households. It explains that acids have a sour taste and are corrosive, providing examples like lemon juice, vinegar, hydrochloric acid, and sulfuric acid. Acids react with metals to form salts and hydrogen, and with carbonates to form salts, carbon dioxide, and water. Bases or alkalis, like sodium hydroxide and calcium hydroxide, feel soapy and are corrosive. The document also introduces pH as a measure of acidity and alkalinity on a scale of 1-14, and mentions common acid-base indicators like litmus and universal indicator that change color over different pH ranges.
Titration introduction
An introduction to titration--why we use it, the advantage of water solution chemistry, and acid-base, conductimetric and redox titrations.
ACID BASE TITRATION
This document provides an overview of acid-base titration and summarizes the key steps and considerations when performing a titration. It discusses selecting an appropriate indicator based on the relative strengths of the acid and base, performing multiple titrations to determine the endpoint accurately, and calculating pH at different points during the titration, including the initial pH, pH before and at the equivalence point, and pH after the equivalence point. Formulas are provided for calculating pH at these different stages of a titration, whether it involves a strong acid-strong base, strong acid-weak base, or weak acid-strong base reaction.
IB Chemistry on Acid Base Indicators and Salt Hydrolysis
- Acid-base indicators change color at their pKa value due to the equilibrium between their acid and conjugate base forms.
- Common indicators and their pKa values and color changes are listed. Methyl orange changes from red to yellow at pH 3.46.
- For an indicator to be suitable in a titration, its color change must occur within the pH range at the equivalence point where amount of acid equals amount of base.
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.
Non aq titrations unit 2
Non-aqueous titration has several advantages over aqueous titration:
1. Organic acids and bases insoluble in water can be soluble in non-aqueous solvents allowing them to be titrated.
2. A non-aqueous solvent may help separate two or more acids in a mixture so they can be titrated individually.
3. More substances can be titrated as the solubility and application ranges are enlarged for weak acids/bases that cannot be titrated in water.
Some common non-aqueous solvents used include acetic acid, acetonitrile, alcohols, DMF. Indicators suitable for specific titrations must be selected to indicate the endpoint
Acid base titration
An acid–base titration is the process which determines the concentration of an acid or base .Which exactly neutralize the acid or base with an acid or base of known concentration. Through acid base reactions Acid-Base titrations usually find the amount of a known acidic or basic substance. This enables the quantitative analysis of the concentration of an unknown acid or base solution. It work with following the neutralization reaction that occurs between acids and bases. To find percent purity of chemicals Acid–base titrations can also be used.
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Lecture 1 - PH and Litmus paper
In chemistry, pH (potential of hydrogen) is a numeric scale used to specify the acidity or basicity of an aqueous solution. It is approximately the negative of the base 10 logarithm of the molar concentration, measured in units of moles per liter, of hydrogen ions.
pH indicator experiment
This experiment aims to make a pH meter and buffer solution. Red cabbage and turmeric extracts were tested as natural pH indicators. Red cabbage juice turns red in acid and purple/blue in neutral/base. Turmeric is yellow below pH 7.4 and pink/red above pH 8.6. Household products like vinegar, orange juice, and toothpaste were found to be acidic, acidic, and basic respectively when tested with the indicators. Both red cabbage and turmeric indicators can distinguish acid from base, with red cabbage having a wider detectable pH range.
P h indicator
This experiment aims to make a pH meter and buffer solution. Red cabbage and turmeric extracts were tested as natural pH indicators. Red cabbage juice turns from red in acid to purple to green-yellow in base. Turmeric is yellow below pH 7.4 and pink above 8.6. Household products like vinegar, orange juice, and toothpaste were found to be respectively acid, acid, and base when tested with the indicators. Both red cabbage and turmeric can act as pH indicators but red cabbage maintains its colors longer.
pH
The document discusses pH, including its definition as the negative logarithm of the hydrogen ion concentration, its scale from 0-14, and methods of measuring it. pH is a measure of acidity or alkalinity and indicates whether a solution is acidic (pH less than 7), basic (pH greater than 7), or neutral (pH of 7). The key methods of measuring pH discussed are pH meters, pH strips, and pH indicators. Common applications of measuring pH include use in pharmaceutical, chemical, food production, and other industries.
Acids bases salt and ph .pdf Grade 11 lesson
This document provides information about acids, bases, and indicators. It defines indicators as substances that change color to indicate whether a solution is acidic or basic. It describes several natural indicators like litmus, turmeric, and red cabbage and how they change color with acids and bases. It also discusses synthetic indicators like phenolphthalein. The document further explains how pH is used to measure acidity or alkalinity on a scale of 0-14. Finally, it provides the pH of several common acids, bases, and neutral substances and gives examples of uses for different acids.
Acids, bases and salts
This document discusses acids, bases, salts, and indicators. It defines acids as sour substances that produce hydrogen ions in solution and have a pH below 7. Bases are defined as having a pH above 7 and forming hydroxide ions in solution. Examples of common acids and bases are provided. Indicators are substances that change color in acidic versus basic solutions, allowing the pH to be determined. Strong acids and bases fully ionize in solution, while weak ones only partially ionize. Neutralization occurs when an acid and base react to form a salt and water. Salts are neutral compounds composed of acid anions and base cations.
Acid base titration
This document discusses acids, bases, and acid-base titration. It defines acids as substances that can donate protons and bases as substances that can accept protons. It explains that acids are sour and turn litmus red, while bases are bitter and slippery and turn litmus blue. Acid-base indicators are then discussed, including how they change color with pH. Two theories of acid-base indicators are described: Ostwald's theory involving ionization equilibrium, and the quinonoid theory involving tautomeric forms. Finally, different types of acid-base titrations are listed along with the typical indicators used for each type.
unit-II (Acid base titration).pptx
This document discusses acid-base titration and indicators. It defines acid-base titration as a quantitative analysis that involves neutralizing an acid or base of unknown concentration with an acid or base of known concentration. The equivalence point occurs when the titrant has exactly neutralized the analyte and allows calculating the concentration of the unknown acid or base. It also describes the Ostwald and quinonoid theories for how acid-base indicators work by changing color depending on their state of ionization or structural form under acidic or basic conditions.
Understanding acids and bases.ppt 2012
This document provides information about acids and bases, including:
- A table listing the pH of common substances like distilled water, lemon juice, milk, etc.
- Characteristics of acids (sour taste, pH less than 7, corrode metal, conduct electricity well) and bases (bitter taste, pH greater than 7, good cleaners, slippery feel)
- An explanation of the logarithmic pH scale and how differences in pH values correspond to differences in acidity or alkalinity.
- Sample questions to check the reader's understanding of comparing acidity using the pH scale and identifying indicators and examples of strong vs. weak acids.
Acids bases by By MUHAMMAD FAHAD ANSARI 12 IEEM 14
This document discusses acids and bases. It defines acids as substances that release H+ ions in solution, donate protons, or accept electron pairs. Bases are defined as substances that release OH- ions in solution, accept protons, or donate electron pairs. A neutralization reaction occurs when an acid and base combine to form water. The pH scale measures how acidic or basic a substance is on a scale from 0-14. Acids have a sour taste, turn litmus paper red, and react with bases. Bases have a slippery feeling, turn litmus paper blue, and react with acids. Common indicators, like litmus paper, change color in acids and bases.
About pH and Buffer .pdf
This document summarizes information about pH and buffers. It defines pH as the negative log of the hydrogen ion concentration, and describes Sorensen's pH scale which ranges from 0-14. Common methods for measuring pH are discussed, including pH strips, indicators, meters, and calorimetric/electrometric methods. The key components and functions of buffers are outlined, including the buffer equation, buffer capacity, and examples of acidic and basic buffers. The roles of important biological buffers and uses of buffers in pharmaceutical systems and applications are highlighted in less than 3 sentences.
ACIDS AND BASES
Indicators change color in acids and bases, allowing them to be used to test whether a substance is acidic or basic. Phenolphthalein is clear in acids but turns pink in bases, while red cabbage juice and litmus paper can also indicate acidity and alkalinity through color changes. The pH scale measures acidity on a scale from 1 to 14, with lower numbers indicating acids and higher numbers indicating bases. Litmus paper and red cabbage juice can test for acids and bases through color changes, though the pH scale provides a more precise measurement of strength. When acids and bases are mixed, they neutralize through a reaction that produces salt and water.
quiz_acids and bases
The document provides instructions for a 15 question true/false and multiple choice test on acids and bases. It explains that each question should be answered honestly by selecting the best answer, and that explanations will be provided for each question after it is answered. It also provides directions on how to navigate between questions and pages of the test.
Acid base indicators chemistry
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Acid base indicators
THIS PRESENTATION IS FOR THE STUDENTS STUDYING IN SENIOR CLASSES .IT WILL HELP THE CHILD TO RECALL THE CONTENT IN SHORT TIME IT WILL HELP TO BUILD THE STRONG AND CLEAR CONCEPT KNOWLEDGE.
Acids and Bases
- Red cabbage contains the pigment anthocyanin, which can be used as a natural pH indicator. Boiling and steeping cabbage produces a purple liquid that changes color in acidic and basic solutions.
- When the cabbage indicator solution is added to lemon juice, vinegar, or other acids, it turns red or purple, indicating an acidic pH below 7. When added to bleach, a strong base, it turns greenish-yellow, showing a basic pH above 7.
- The color change occurs because the anthocyanin pigment absorbs and reflects different wavelengths of light depending on whether the solution is acidic or basic, based on its hydrogen ion concentration.
Acid and alkalis Lesson 3
This document provides information about acids and alkalis. It defines acids as substances with a pH below 7 that turn litmus red and can be neutralized by alkalis. Common strong acids are hydrochloric, sulfuric, and nitric acids. Indicators like litmus and universal indicator can be used to determine if a substance is acidic or alkaline based on color changes. The pH scale quantifies how acidic or alkaline a substance is from 1-14. Examples show how universal indicator is used to test substances and determine their acidity or alkalinity based on color.
Acid base review 2013
The document summarizes key concepts about acids and bases:
- The pH scale measures how acidic or alkaline a substance is from 0-14. Phenolphthalein and bromothymol blue are acid-base indicators that change color. Universal indicator can be used to test unknown solutions and determine pH.
- Strong acids have a pH of 0-1 and strong bases 13-14. Acids contain hydrogen ions and bases contain hydroxide ions. Examples of acidic foods are citrus fruits and milk. Cleaners are often bases.
- Acids taste sour and pure water is neutral. Stronger acids have lower pH numbers. The pH range of normal rain is 5.6-6.
Acid base review 2013
The document summarizes key concepts about acids and bases:
- The pH scale measures how acidic or alkaline a substance is from 0-14. Phenolphthalein and bromothymol blue are acid-base indicators that change color with pH. Universal indicator can be used to test an unknown solution's pH.
- Strong acids have a pH of 0-1 and strong bases 13-14. Acids contain H+ ions and bases contain OH- ions. Common acids include citrus fruits and milk while cleaners contain bases.
- Neutralization is adding a base to an acid until the pH is close to 7. Carbon dioxide forms carbonic acid in water.
Acid base review 2013
The document summarizes key concepts about acids and bases including:
1. The pH scale measures how acidic or alkaline a substance is from 0-14. Strong acids have a pH of 0-1 while strong bases are 13-14.
2. Phenolphthalein and bromothymol blue are acid-base indicators that change color depending on whether a solution is acidic or basic.
3. Universal indicator can be used to test unknown solutions and determine their pH level on the scale.
4. Strong acids have lower pH values than weak acids. The difference in pH numbers indicates the strength of acidity on a logarithmic scale.
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Acids bases by By MUHAMMAD FAHAD ANSARI 12 IEEM 14
Acids bases by By MUHAMMAD FAHAD ANSARI 12 IEEM 14
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P h indicator
- 1. : The definition of pH is the negative logarithm of the hydrogen ion (H+) activity in a given solution. • The range of the ph scale is from 0 to 14. 10-Jan-17 ALINA SHERIN 1
- 2. pH , pOH pH : Negative logarithm of hydrogen ions concentration pH= -log[Hᶧ] pOH : Negative logarithm of hydroxyl ions concentration pOH= -log[pOHˉ] 10-Jan-17 ALINA SHERIN 2
- 3. Acidity or alkalinity of a solution • So why are the hydrogen (H+) ions of interest? The hydrogen ions (H+) are what determines if a solution is acidic, alkaline or neutral. If we can measure the hydrogen ion content of a solution, we can determine the acidity or alkalinity of that solution. 10-Jan-17 ALINA SHERIN 3
- 4. • Water molecules are in continuous motion. When two water molecules collide, a hydrogen and hydroxide ion are created. This process in which water itself dissociates (splits) into hydrogen and hydroxide ions is called auto dissociation or self ionization. 10-Jan-17 ALINA SHERIN 4
- 5. pH INDICATOR pH indicators are substances, usually a weak acid or base, that changes color depending on the pH of the solution it is mixed with. 10-Jan-17 ALINA SHERIN 5
- 6. Universal Indicator A universal indicator interprets how acidic or basic a solution is. A universal indicator can be in paper form or present in a form of a solution 10-Jan-17 ALINA SHERIN 6
- 7. Example of common indicators of pH LITMUS Color in Acid: Red Color in Base: Blue A commonly used acid- base indicator is litmus. Litmus is a natural indicator obtained from certain lichens. It is useful for detecting acids and bases because it changes color around pH 7. 10-Jan-17 7ALINA SHERIN
- 8. Ph Scale 10-Jan-17 ALINA SHERIN 8
- 9. • Phenolphthalein Phenolphthalein, an acid-base indicator used to test the pH of a solution, turns pink due to the presence of a weak base. The indicator itself is a weak, colorless acid that forms pink anions when it dissolves in water. Color in Acid: Colorless Color in Base: Pinkish violet color Approximate pH range for color change: 8.3 -10.0 10-Jan-17 9ALINA SHERIN
- 10. 10-Jan-17 ALINA SHERIN 10 Colorless in acids pink in base
- 11. • Methyl Orange: Methyl orange is an intensely colored compound used in dyeing and printing textiles. Color in Acid: Red Color in Base: Yellow Approximate pH range for color change: 3.1(red)-4.4 The yellow form is basic, the red form is acidic 10-Jan-17 11ALINA SHERIN
- 12. 10-Jan-17 ALINA SHERIN 12
- 13. 10-Jan-17 ALINA SHERIN 13