ACID, ALKALI, SALT click at http/www.jendelaipa.co.cc
ACID, ALKALI, AND SALT
Acid and alkalis are two important solutions.
They are not only being used in the laboratory but also in our in daily life.
ACID
1. The word ‘acid’ come from the Latin word ‘Acidus’, which means sour.
2. Acid in food gives the food a sour and tangy taste.
A few examples of acids in our food able 1 shows.
Food Acid in food
Grapes Tartaric acid
Apples Malic acid
Oranges, lemons Citric acid
Tomatoes Salicylic acid
Vinegar Acetic acid (ethanoic acid)
Yoghurt drinks Lactic acid
3. Acids used in the laboratory are harmful. Hydrochloric acid and nitric acid are three common acids used in the laboratory.
Properties of acid:
1. Has a sour taste
2. Has a pH value less than 7
3. Have a corrosive nature
4. Turn blue litmus paper red
5. React with reactive metals such as zinc, magnesium and iron to produce hydrogen gas. The hydrogen gas gives out a squeaky pop when tested with a lighted splinter.
ALKALI
1. Alkali is the chemical ‘opposite’ of acid.
2. Alkali are often used in many household.
3. Ammonia solution, sodium hydroxide solution and potassium hydroxide solution are tree common alkalis used in the laboratory.
Properties of alkali
1. Has a bitter taste
2. Has a soapy feel
3. Have a pH value greater than 7
4. Has a corrosive nature
5. Turn red litmus paper blue
6. Reach with ammonium salt to release ammonia when heated.
Acid Uses of acid
Citric acid • Added to food and drinks to give a pleasant sour taste
• As a polishing agent for metals.
Tartaric acid • As a flavoring in food and drinks
• To produce fruit salts or health salts.
Benzoic acid • As a preservative in food such as sauces
Ascorbic acid (Vit. C) • Needed by humans to increase the body’s resistance to infections and to prevent scurvy
Formic acid • Used to coagulate latex
Acetic acid • Used as vinegar.
• As a preservative in food such as pickles.
• To produce paints, plastics, and rayon
Sulphuric acid • Used in car batteries and fire extinguishers
• To produce fertilizers and detergents
Hydrochloric acid • To clean metals before they are coated
• As cleansing agent in toilet cleaners.
Nitric acid • To produce fertilizers, dyes and explosives
Alkali Uses of acid
Sodium hydroxide • To produce soaps, detergents, plastics and rayon
Calcium hydroxide • To produce cement, mortar, soda lime and glass.
Ammonia • To neutralize acidic soil in agriculture
• As a cleaning agent in glass and window cleaners.
• To produce nitric acid and fertilizers
Magnesium hydroxide • To produce medicines such as antacids
Caustic soda • As cleansing agent in oven cleaners
Salts
The most familiar salt is sodium chloride, the principal component of common table salt. Sodium chloride, NaCl, and water, H2O, are formed by neutralization of sodium hydroxide, NaOH, a base, with hydrogen chloride, HCl, an acid: HCl+NaOH→NaCl+H2O. Most salts are ionic compounds (see chemical bond); they are made up of ions rather than molecules. The chemical formula for an ionic salt is an empirical formula; it does not represent a molecule but shows the proportion of atoms of the elements that make up the salt. The formula for sodium chloride, NaCl, indicates that equal numbers of sodium and chlorine atoms combine to form the salt. In the reaction of sodium with chlorine, each sodium atom loses an electron, becoming positively charged, and each chlorine atom gains an electron, becoming negatively charged (see oxidation and reduction); there are equal numbers of positively charged sodium ions and negatively charged chloride ions in sodium chloride. The ions in a solid salt are usually arranged in a definite crystalline structure, each positive ion being associated with a fixed number of negative ions, and vice versa.
A salt that has neither hydrogen (H) nor hydroxyl (OH) in its formula, e.g., sodium chloride (NaCl), is called a normal salt. A salt that has hydrogen in its formula, e.g., sodium bicarbonate (NaHCO3), is called an acid salt. A salt that has hydroxyl in its formula, e.g., basic lead nitrate (Pb[OH]NO3), is called a basic salt. Since a salt may react with a solvent to yield different ions than were present in the salt (see hydrolysis), a solution of a normal salt may be acidic or basic; e.g., trisodium phosphate, Na3PO4, dissolves in and reacts with water to form a basic solution.
In addition to being classified as normal, acid, or basic, salts are categorized as simple salts, double salts, or complex salts. Simple salts, e.g., sodium chloride, contain only one kind of positive ion (other than the hydrogen ion in acid salts). Double salts contain two different positive ions, e.g., the mineral dolomite, or calcium magnesium carbonate, CaMg(CO3)2. Alums are a special kind of double salt. Complex salts, e.g., potassium ferricyanide, K3Fe(CN)6, contain a complex ion that does not dissociate in solution. A hydrate is a salt that includes water in its solid crystalline form; Glauber's salt and Epsom salts are hydrates.
Salts are often grouped according to the negative ion they contain, e.g., bicarbonate or carbonate, chlorate, chloride, cyanide, fulminate, nitrate, phosphate, silicate, sulfate, or sulfide.
OPINION
Acids have the general formula HX where X is an anion (nonmetal ion or negative polyatonic ion) in aqueous
Defanition Hyrogen compound that yeilds hydrogen ion(H+)
acids are a 1-6.9 on the PH scale and bases are 7-14
Bases have the general formula MOH, where M is a metal cation.
Defanition compound that contains a metal ion and one or more hydroxide (OH-) ions
bases release OH- ions in solution (hydroxide ions) and are slippery and bitter.
Acids taste sour, are corrosive to metals, change litmus (a dye extracted from lichens) red, and become less acidic when mixed with bases.
Bases feel slippery, change litmus blue, and become less basic when mixed with acids.
Properties
Bronsted-Lowry acids:
• Are generally sour in taste
• Strong or concentrated acids often produce a stinging feeling on mucous membranes
• Change the color of pH indicators as follows: turn blue litmus and methyl orange red, turn phenolphthalein colorless
• React with metals to produce a metal salt and hydrogen
• React with metal carbonates to produce water, CO2 and a salt
• React with a base to produce a salt and water
• React with a metal oxide to produce water and a salt
• Conduct electricity, depending on the degree of dissociation
• Produce solvonium ions, such as oxonium (H3O+) ions in water
Acids can be gases, liquids, or solids. Respective examples (at 20 °C and 1 atm) are hydrogen chloride, sulfuric acid and citric acid. Solutions of acids in water are liquids, such as hydrochloric acid - an aqueous solution of hydrogen chloride. At 20 °C and 1 atm, linear carboxylic acids are liquids up to nonanoic acid (nine carbon atoms) and solids beginning from decanoic acid (ten carbon atoms). Aromatic carboxylic acids, the simplest being benzoic acid, are solids.
Strong acids and many concentrated acids, being corrosive, can be dangerous; causing severe burns for even minor contact. Generally, acid burns on the skin are treated by rinsing the affected area abundantly with running water, followed up with immediate medical attention. In the case of highly concentrated mineral acids such as sulfuric acid or nitric acid, the acid should first be wiped off, otherwise the exothermic mixing of the acid and the water could cause thermal burns.[citation needed] Particular acids may also be dangerous for reasons not related to their acidity. Material Safety Data Sheets (MSDS) can be consulted for detailed information on dangers and handling instructions.
Mineral acids
• Solutions of hydrogen halides, such as hydrochloric acid (HCl) and hydrobromic acid (HBr)
• Sulfuric acid (H2SO4)
• Nitric acid (HNO3)
• Phosphoric acid (H3PO4)
• Chromic acid (H2CrO4)
Sulfonic acids
• Methanesulfonic acid (aka mesylic acid) (MeSO3H)
• Ethanesulfonic acid (aka esylic acid) (EtSO3H)
• Benzenesulfonic acid (aka besylic acid) (PhSO3H)
• Toluenesulfonic acid (aka tosylic acid, or (C6H4(CH3) (SO3H))
Carboxylic acids
• Formic acid
• Acetic acid
• Citric acid
Vinylogous carboxylic acids
• Ascorbic acid
• Meldrum's acid
Task for RSBI class.
Exercise Question:
1. Mention at least 5 properties of acid!
2. A few examples of acids in our food, mention at least 5!
3. Mention at least 5 the benefic of acid in daily life!
4. Mention at least 5 properties of alkali!
5. A few examples of akalis in our food, mention at least 5!
6. Mention at least 5 the benefic of alkali in daily life!
7. Mention at least 5 properties of salt!
8. A few examples of salts in our food, mention at least 5!
9. Mention at least 5 the benefic of salt in daily life!
10 Make formula of chemistry Sulfonic acids!
Next click at.
WWW.jendelaipa.co.cc
Acid and alkalis are two important solutions.
They are not only being used in the laboratory but also in our in daily life.
ACID
1. The word ‘acid’ come from the Latin word ‘Acidus’, which means sour.
2. Acid in food gives the food a sour and tangy taste.
A few examples of acids in our food able 1 shows.
Food Acid in food
Grapes Tartaric acid
Apples Malic acid
Oranges, lemons Citric acid
Tomatoes Salicylic acid
Vinegar Acetic acid (ethanoic acid)
Yoghurt drinks Lactic acid
3. Acids used in the laboratory are harmful. Hydrochloric acid and nitric acid are three common acids used in the laboratory.
Properties of acid:
1. Has a sour taste
2. Has a pH value less than 7
3. Have a corrosive nature
4. Turn blue litmus paper red
5. React with reactive metals such as zinc, magnesium and iron to produce hydrogen gas. The hydrogen gas gives out a squeaky pop when tested with a lighted splinter.
ALKALI
1. Alkali is the chemical ‘opposite’ of acid.
2. Alkali are often used in many household.
3. Ammonia solution, sodium hydroxide solution and potassium hydroxide solution are tree common alkalis used in the laboratory.
Properties of alkali
1. Has a bitter taste
2. Has a soapy feel
3. Have a pH value greater than 7
4. Has a corrosive nature
5. Turn red litmus paper blue
6. Reach with ammonium salt to release ammonia when heated.
Acid Uses of acid
Citric acid • Added to food and drinks to give a pleasant sour taste
• As a polishing agent for metals.
Tartaric acid • As a flavoring in food and drinks
• To produce fruit salts or health salts.
Benzoic acid • As a preservative in food such as sauces
Ascorbic acid (Vit. C) • Needed by humans to increase the body’s resistance to infections and to prevent scurvy
Formic acid • Used to coagulate latex
Acetic acid • Used as vinegar.
• As a preservative in food such as pickles.
• To produce paints, plastics, and rayon
Sulphuric acid • Used in car batteries and fire extinguishers
• To produce fertilizers and detergents
Hydrochloric acid • To clean metals before they are coated
• As cleansing agent in toilet cleaners.
Nitric acid • To produce fertilizers, dyes and explosives
Alkali Uses of acid
Sodium hydroxide • To produce soaps, detergents, plastics and rayon
Calcium hydroxide • To produce cement, mortar, soda lime and glass.
Ammonia • To neutralize acidic soil in agriculture
• As a cleaning agent in glass and window cleaners.
• To produce nitric acid and fertilizers
Magnesium hydroxide • To produce medicines such as antacids
Caustic soda • As cleansing agent in oven cleaners
Salts
The most familiar salt is sodium chloride, the principal component of common table salt. Sodium chloride, NaCl, and water, H2O, are formed by neutralization of sodium hydroxide, NaOH, a base, with hydrogen chloride, HCl, an acid: HCl+NaOH→NaCl+H2O. Most salts are ionic compounds (see chemical bond); they are made up of ions rather than molecules. The chemical formula for an ionic salt is an empirical formula; it does not represent a molecule but shows the proportion of atoms of the elements that make up the salt. The formula for sodium chloride, NaCl, indicates that equal numbers of sodium and chlorine atoms combine to form the salt. In the reaction of sodium with chlorine, each sodium atom loses an electron, becoming positively charged, and each chlorine atom gains an electron, becoming negatively charged (see oxidation and reduction); there are equal numbers of positively charged sodium ions and negatively charged chloride ions in sodium chloride. The ions in a solid salt are usually arranged in a definite crystalline structure, each positive ion being associated with a fixed number of negative ions, and vice versa.
A salt that has neither hydrogen (H) nor hydroxyl (OH) in its formula, e.g., sodium chloride (NaCl), is called a normal salt. A salt that has hydrogen in its formula, e.g., sodium bicarbonate (NaHCO3), is called an acid salt. A salt that has hydroxyl in its formula, e.g., basic lead nitrate (Pb[OH]NO3), is called a basic salt. Since a salt may react with a solvent to yield different ions than were present in the salt (see hydrolysis), a solution of a normal salt may be acidic or basic; e.g., trisodium phosphate, Na3PO4, dissolves in and reacts with water to form a basic solution.
In addition to being classified as normal, acid, or basic, salts are categorized as simple salts, double salts, or complex salts. Simple salts, e.g., sodium chloride, contain only one kind of positive ion (other than the hydrogen ion in acid salts). Double salts contain two different positive ions, e.g., the mineral dolomite, or calcium magnesium carbonate, CaMg(CO3)2. Alums are a special kind of double salt. Complex salts, e.g., potassium ferricyanide, K3Fe(CN)6, contain a complex ion that does not dissociate in solution. A hydrate is a salt that includes water in its solid crystalline form; Glauber's salt and Epsom salts are hydrates.
Salts are often grouped according to the negative ion they contain, e.g., bicarbonate or carbonate, chlorate, chloride, cyanide, fulminate, nitrate, phosphate, silicate, sulfate, or sulfide.
OPINION
Acids have the general formula HX where X is an anion (nonmetal ion or negative polyatonic ion) in aqueous
Defanition Hyrogen compound that yeilds hydrogen ion(H+)
acids are a 1-6.9 on the PH scale and bases are 7-14
Bases have the general formula MOH, where M is a metal cation.
Defanition compound that contains a metal ion and one or more hydroxide (OH-) ions
bases release OH- ions in solution (hydroxide ions) and are slippery and bitter.
Acids taste sour, are corrosive to metals, change litmus (a dye extracted from lichens) red, and become less acidic when mixed with bases.
Bases feel slippery, change litmus blue, and become less basic when mixed with acids.
Properties
Bronsted-Lowry acids:
• Are generally sour in taste
• Strong or concentrated acids often produce a stinging feeling on mucous membranes
• Change the color of pH indicators as follows: turn blue litmus and methyl orange red, turn phenolphthalein colorless
• React with metals to produce a metal salt and hydrogen
• React with metal carbonates to produce water, CO2 and a salt
• React with a base to produce a salt and water
• React with a metal oxide to produce water and a salt
• Conduct electricity, depending on the degree of dissociation
• Produce solvonium ions, such as oxonium (H3O+) ions in water
Acids can be gases, liquids, or solids. Respective examples (at 20 °C and 1 atm) are hydrogen chloride, sulfuric acid and citric acid. Solutions of acids in water are liquids, such as hydrochloric acid - an aqueous solution of hydrogen chloride. At 20 °C and 1 atm, linear carboxylic acids are liquids up to nonanoic acid (nine carbon atoms) and solids beginning from decanoic acid (ten carbon atoms). Aromatic carboxylic acids, the simplest being benzoic acid, are solids.
Strong acids and many concentrated acids, being corrosive, can be dangerous; causing severe burns for even minor contact. Generally, acid burns on the skin are treated by rinsing the affected area abundantly with running water, followed up with immediate medical attention. In the case of highly concentrated mineral acids such as sulfuric acid or nitric acid, the acid should first be wiped off, otherwise the exothermic mixing of the acid and the water could cause thermal burns.[citation needed] Particular acids may also be dangerous for reasons not related to their acidity. Material Safety Data Sheets (MSDS) can be consulted for detailed information on dangers and handling instructions.
Mineral acids
• Solutions of hydrogen halides, such as hydrochloric acid (HCl) and hydrobromic acid (HBr)
• Sulfuric acid (H2SO4)
• Nitric acid (HNO3)
• Phosphoric acid (H3PO4)
• Chromic acid (H2CrO4)
Sulfonic acids
• Methanesulfonic acid (aka mesylic acid) (MeSO3H)
• Ethanesulfonic acid (aka esylic acid) (EtSO3H)
• Benzenesulfonic acid (aka besylic acid) (PhSO3H)
• Toluenesulfonic acid (aka tosylic acid, or (C6H4(CH3) (SO3H))
Carboxylic acids
• Formic acid
• Acetic acid
• Citric acid
Vinylogous carboxylic acids
• Ascorbic acid
• Meldrum's acid
Task for RSBI class.
Exercise Question:
1. Mention at least 5 properties of acid!
2. A few examples of acids in our food, mention at least 5!
3. Mention at least 5 the benefic of acid in daily life!
4. Mention at least 5 properties of alkali!
5. A few examples of akalis in our food, mention at least 5!
6. Mention at least 5 the benefic of alkali in daily life!
7. Mention at least 5 properties of salt!
8. A few examples of salts in our food, mention at least 5!
9. Mention at least 5 the benefic of salt in daily life!
10 Make formula of chemistry Sulfonic acids!
Next click at.
WWW.jendelaipa.co.cc
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