Salts
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A salt is formed when all or part of the hydrogen in an acid is replaced by metal or ammonium ions. There are different types of salts including normal salts, acid salts, basic salts, double salts, and complex salts. Salts can be prepared through reactions such as mixing a dilute acid with a metal to form a soluble salt, reacting an alkali with an acid, and mixing solutions containing ions that form an insoluble salt to produce precipitation. Insoluble salts can also be prepared through double decomposition reactions or by directly combining element constituents.
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Insoluble salts
This document discusses insoluble salts. It defines insoluble salts as salts that cannot dissolve in water at room temperature. It explains that insoluble salts can be prepared through precipitation reactions or double decomposition reactions by mixing aqueous solutions containing the cations and anions that will form the insoluble salt. This causes the ions to interchange and form an insoluble precipitate. Examples of insoluble salts formed and their ionic equations are also provided.
What is Salt?
A salt is formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. The solubility of a salt in water is important for determining the suitable method for preparing it. Common soluble salts include ammonium, sodium, and potassium salts as well as most nitrate, chloride, and sulfate salts. However, some chloride, sulfate, and carbonate salts are insoluble such as silver chloride, lead chloride, mercury chloride, calcium sulfate, lead sulfate, barium sulfate, and most metal carbonates. Knowing whether a salt is soluble or insoluble is crucial before preparing it.
Chapter 8 salt part 1
The document discusses learning outcomes about salts. It defines a salt as a compound formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. Examples of commonly used salts include NaCl, MSG, and CaCO3. Salts can be soluble or insoluble depending on their cation and anion. The document also describes different methods for preparing soluble and insoluble salts, such as titration, evaporation/heating, cooling/crystallization, filtration, and drying.
Chapter 8 salt part 2
This document describes the purification of soluble salts through recrystallization and the preparation of insoluble salts through precipitation reactions. It discusses physical characteristics of salt crystals such as their geometric shape and fixed angles. It then provides examples of precipitation reactions used to prepare specific insoluble salts like lead (II) sulfate, copper (II) carbonate, and barium sulfate through a double decomposition reaction between aqueous solutions of their ions. General and ionic chemical equations are given to represent these precipitation reactions.
Chapter 8 : SALTS
This document discusses the preparation and classification of salts. Salts are formed through the replacement of hydrogen ions in acids by metal ions or ammonium ions. There are two main methods for preparing salts - neutralization and precipitation. Neutralization involves reacting an acid with a metal, alkali, oxide or carbonate to form a soluble salt. Precipitation involves mixing two aqueous solutions of soluble salts to form an insoluble salt precipitate. The document provides examples of preparing various salts such as potassium chloride and lead chloride. It also discusses classifying salts as soluble or insoluble and purifying soluble salts through recrystallization.
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This document describes the process of preparing salts through titration. It explains that titration allows the neutralization of an acid and base to be carried out exactly, producing a soluble salt. It provides the example of preparing sodium chloride through titrating hydrochloric acid with sodium hydroxide. The steps involve adding an indicator, titrating the acid with the base until the endpoint is reached, evaporating the solution to leave behind salt crystals, and filtering and drying the crystals. It asks how ammonium nitrate could be prepared using this method.
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Insoluble salts
This document discusses insoluble salts. It defines insoluble salts as salts that cannot dissolve in water at room temperature. It explains that insoluble salts can be prepared through precipitation reactions or double decomposition reactions by mixing aqueous solutions containing the cations and anions that will form the insoluble salt. This causes the ions to interchange and form an insoluble precipitate. Examples of insoluble salts formed and their ionic equations are also provided.
What is Salt?
A salt is formed when a hydrogen ion from an acid is replaced by a metal ion or ammonium ion. The solubility of a salt in water is important for determining the suitable method for preparing it. Common soluble salts include ammonium, sodium, and potassium salts as well as most nitrate, chloride, and sulfate salts. However, some chloride, sulfate, and carbonate salts are insoluble such as silver chloride, lead chloride, mercury chloride, calcium sulfate, lead sulfate, barium sulfate, and most metal carbonates. Knowing whether a salt is soluble or insoluble is crucial before preparing it.
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Chapter 8 salt part 2
This document describes the purification of soluble salts through recrystallization and the preparation of insoluble salts through precipitation reactions. It discusses physical characteristics of salt crystals such as their geometric shape and fixed angles. It then provides examples of precipitation reactions used to prepare specific insoluble salts like lead (II) sulfate, copper (II) carbonate, and barium sulfate through a double decomposition reaction between aqueous solutions of their ions. General and ionic chemical equations are given to represent these precipitation reactions.
Chapter 8 : SALTS
This document discusses the preparation and classification of salts. Salts are formed through the replacement of hydrogen ions in acids by metal ions or ammonium ions. There are two main methods for preparing salts - neutralization and precipitation. Neutralization involves reacting an acid with a metal, alkali, oxide or carbonate to form a soluble salt. Precipitation involves mixing two aqueous solutions of soluble salts to form an insoluble salt precipitate. The document provides examples of preparing various salts such as potassium chloride and lead chloride. It also discusses classifying salts as soluble or insoluble and purifying soluble salts through recrystallization.
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The document discusses acids, bases, and salts. It defines acids as substances that form hydrogen ions in water, such as hydrochloric acid, sulfuric acid, and nitric acid. Bases are defined as oxides and hydroxides of metals that react with acids to form salts and water. Common strong acids and their ions are listed, as well as common weak acids. The properties, naming, and formula writing of acids and bases are also covered.
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This document describes the preparation of soluble salts through various methods including neutralization reactions, titration, evaporation, crystallization, and filtration. Soluble salts can be prepared by reacting an acid with an alkali, metal, metallic oxide, or metallic carbonate. The reaction mixtures are then heated, filtered, and dried to obtain pure salt crystals. Key steps involve neutralization, evaporation to saturate and crystallize the salt, then filtration to separate and dry the pure salt product.
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Solubility is the ability of a substance to dissolve in a solvent like water. The solubility of salts is important for separating mixtures of salts, preparing salt samples, and identifying cations and anions. A soluble salt dissolves in water at room temperature, including most nitrates, ethanoates, sodium, potassium, and ammonium salts. Soluble salts can be prepared through four types of reactions: between an acid and alkali, acid and base, acid and reactive metal, or acid and metal carbonate. Preparation of soluble salts like potassium nitrate involves a neutralization reaction between an acid and base.
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This chapter discusses acids, bases, and salts. It defines acids as substances that produce hydrogen ions (H+) in water, and bases as substances that react with acids to produce salts and water. Alkalis are soluble bases that produce hydroxide ions (OH-) in water. The chapter covers acid-base theories, pH, strength of acids/bases, concentration of solutions, neutralization reactions, and preparation and properties of salts. Examples of uses of acids and bases in daily life are discussed, such as sulfuric acid in car batteries and sodium hydroxide in soaps.
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6.1 Role of water in showing acidic and alkaline properties (PPT)
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3) The document provides details on solubility rules and characteristic reactions for each group of anions to allow their identification in mixtures
Compounds of metals
The document discusses different types of metal compounds including oxides, hydroxides, carbonates, nitrates, and chlorides. It describes methods of preparing these compounds such as direct combination of metals with oxygen or other reactants, or reactions of metal salts with bases or acids. The properties, reactions and uses of these compounds are also outlined. For example, metal oxides can be basic, acidic, or amphoteric and are used to form salts or in manufacturing. Hydroxides vary in solubility depending on the metal's reactivity and react with acids to form salts. Carbonates and nitrates similarly react with acids.
Acids bases and salts
This document provides information about acids, bases, salts, and pH scale. It defines acids and bases, describes their properties and classifications. It discusses the preparation and uses of acids, bases, and salts. It also explains what the pH scale measures, how it indicates acidity and basicity, and how pH values correspond to acids and bases.
Cxc oxides, acids, bases and salts
1. Oxides can be acidic, basic, neutral or amphoteric depending on whether they react with acids and bases to form salts and water. Acidic oxides form salts with bases while basic oxides form salts with acids.
2. Acids are compounds that form hydrogen ions in aqueous solution and have characteristic properties like turning litmus red. Strong acids fully ionize while weak acids partially ionize.
3. Bases are compounds that form hydroxide ions in aqueous solution and have properties like turning litmus blue. Alkalis are soluble bases that produce hydroxide ions in water.
Acid and bases
This is a summary of the topic "Acids and bases" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
Transition Metals and Complexes, Vanadium and Chromium metal
Shapes and Color of Coordinations Compounds depends upon the Ligands and d-d transition of electrons in the central elements
(NH4)2SO4 is a soluble salt and is fully ionized in solution(NH4).pdf
(NH4)2SO4 is a soluble salt and is fully ionized in solution:
(NH4)2SO4 => 2 NH4+ + SO42-
NH4+ is a weak acid and ionizes further: NH4+<=> NH3 + H+
The H+ formed can react with C2O42- to form the weak acid oxalic acid (H2C2O4):
C2O42- + 2 H+ <=> H2C2O4
Removal of C2O42- causes the equilibrium: ZnC2O4 <=> Zn2+ + C2O42-
to shift to the right according to Le Chatelier\'s principle and more ZnC2O4 dissolves.
Thus the solubility of ZnC2O4 increases in the presence of (NH4)2SO4.
Solution
(NH4)2SO4 is a soluble salt and is fully ionized in solution:
(NH4)2SO4 => 2 NH4+ + SO42-
NH4+ is a weak acid and ionizes further: NH4+<=> NH3 + H+
The H+ formed can react with C2O42- to form the weak acid oxalic acid (H2C2O4):
C2O42- + 2 H+ <=> H2C2O4
Removal of C2O42- causes the equilibrium: ZnC2O4 <=> Zn2+ + C2O42-
to shift to the right according to Le Chatelier\'s principle and more ZnC2O4 dissolves.
Thus the solubility of ZnC2O4 increases in the presence of (NH4)2SO4..
Acids and base for O level chemistry
this topic leads O level students of Tanzania Secondary school and other to gain a knowledge about Acid and Base. ALSAL PREPARED
cbse-class-10-science-notes-chapter-2-acids-bases-and-salts.pptx
This document provides an introduction to acids, bases and salts including:
- The Arrhenius and Bronsted-Lowry theories of acids and bases which define acids as substances that produce H+ ions in water and bases as those that produce OH- ions.
- Common acids like hydrochloric acid and common bases like sodium hydroxide.
- Acid-base reactions include neutralization reactions and reactions with metals and carbonates that produce salts, water and other products.
- Properties of salts like pH, families based on cations and anions, and methods of preparation for common salts.
ammonia presentation.pptx
This document discusses various types of reactions that occur in liquid ammonia, including precipitation, complex formation, ammonolysis, solvation, and amphoteric reactions. Precipitation reactions in ammonia differ from those in water, as most metal chlorides are insoluble except for NaCl, NH4Cl, and BeCl2. Complex formation reactions also occur similarly to those in water, such as the formation of potassium hydroxozincate from zinc chloride and potassium hydroxide. Ammonolysis reactions involve ammonia acting as a reactant in place of water. Solvation involves the formation of ammoniates through coordination bonds, ion dipole interactions, or hydrogen bonding between ammonia molecules and other compounds. Amphoteric behavior
qualitative inorganic analysis anions dry and wet
Qualitative Inorganic Analysis deals with detection and identification of substances in mixtures. This document discusses the qualitative analysis of anions, which are negatively charged ions. Anions are divided into six groups including carbonates/bicarbonates, sulphur-containing anions, halides, cyanogen anions, and nitrogen-containing anions. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions like sulphides, sulphites, thiosulphates and sulphates have characteristic reactions with acids, salts, and oxidizing agents. Their reactions can be used to identify these anions in mixtures.
3 acid base reactions
1. The document describes different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, combustion, acid-base, and neutralization reactions.
2. Metals react with oxygen to form metal oxides which are bases. Non-metals react with oxygen to form non-metal oxides which are acids.
3. Acid-base reactions involve acids and bases reacting to form salts and water in a neutralization reaction.
Types of Oxides.ppt
An oxide is a compound formed from oxygen and another element. There are four main types of oxides: acidic, basic, amphoteric, and neutral. Acidic oxides dissolve in water to form acids, basic oxides are insoluble in water and react with acids to form salts, amphoteric oxides react with both acids and bases, and neutral oxides do not react with acids or bases. Common examples of each type and their reactions are provided.
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Soluble and insoluble Salts and their methods of making.
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Transition Metals and Complexes, Vanadium and Chromium metal
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- 2. What is a salt? A salt is the compound formed when all or part of the ionizable hydrogen of an acid is replaced by metallic or ammonium ions.
- 3. Types Normal salts Acid salts Basic salts Double salts Complex salts
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- 5. Preparation of salts Insoluble salts Double decomposition: 2 soluble compounds, one containing the metalic and the other acidic radical of the required insoluble salt are mixed together . There is exchange 0f raicals leading to precipitation of the required salt. BaCl2 + K2 SO4 BaSO4 + NaNO3 Combination of constituent elements: for preparing binary salts 2Fe + 3Cl2 2FeCl3