Common ion effect
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This pdf is about the concept of the common ion effect with examples and its precipitation and a flow chart with diagrams.
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Presentation 5 1 common ion power.pptx
The document discusses the common ion effect, which is when adding a soluble compound containing one of the ions of a precipitate decreases the solubility of the precipitate. It provides examples like adding dilute sulfuric acid (which contains sulfate ions) to a saturated calcium sulfate solution, causing more calcium sulfate to precipitate out. It also discusses how adding sodium chloride to a solution of hydrochloric acid and water, or during soap making, provides more chloride or sodium ions that reduce the solubility of salts through competition.
COMMON ION EFFECT
The statement of the common ion effect can be written as follows – in a solution wherein there are several species associating with each other via a chemical equilibrium process, an increase in the concentration of one of the ions dissociated in the solution by the addition of another species containing the same ion will lead to an increase in the degree of association of ions.
An example of the common ion effect can be observed when gaseous hydrogen chloride is passed through a sodium chloride solution, leading to the precipitation of the NaCl due to the excess of chloride ions in the solution (brought on by the dissociation of HCl).
This effect cannot be observed in the compounds of transition metals. This is because the d-block elements tend to form complex ions. This can be observed in the compound cuprous chloride, which is insoluble in water. This compound can be dissolved in water by the addition of chloride ions leading to the formation of the CuCl2– complex ion, which is soluble in water.
Effect on Solubility:
How the solubility of a salt in a solution is affected by the addition of a common ion is discussed in this subsection.
The common ion effect can be used to obtain drinking water from aquifers (underground layers of water mixed with permeable rocks or other unconsolidated materials) containing chalk or limestone. Sodium carbonate (chemical formula Na2CO3) is added to the water to decrease the hardness of the water.
In the treatment of water, the common ion effect is used to precipitate out the calcium carbonate (which is sparingly soluble) from the water via the addition of sodium carbonate, which is highly soluble.
A finely divided calcium carbonate precipitate of a very pure composition is obtained from this addition of sodium carbonate. The CaCO3 precipitate is, therefore, a valuable by-product that can be used in the process of manufacturing toothpaste.
Since soaps are the sodium salts of carboxylic acids containing a long aliphatic chain (fatty acids), the common ion effect can be observed in the salting-out process which is used in the manufacturing of soaps. The soaps are precipitated out by adding sodium chloride to the soap solution to reduce its solubility.
However, it can be noted that water containing a respectable amount of Na+ ions, such as seawater and brackish water, can hinder the action of soaps by reducing their solubility and therefore their effectiveness.
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.
Anions
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
Salt hydrolysis
Salt hydrolysis can produce acidic, basic, or neutral solutions depending on the salt. Salts are classified based on whether they contain strong acids/bases or weak acids/bases. Salts of strong acids and bases do not undergo hydrolysis and produce neutral solutions. Salts of weak acids and strong bases produce basic solutions, while salts of strong acids and weak bases produce acidic solutions. Salts of weak acids and bases may produce neutral, acidic, or basic solutions. Solubility products define the solubility of sparingly soluble salts in solution. The common ion effect suppresses the dissociation of weak electrolytes in the presence of strong electrolytes with a common ion. Solubility products and common ion effects can be applied
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Presentation 5 1 common ion power.pptx
The document discusses the common ion effect, which is when adding a soluble compound containing one of the ions of a precipitate decreases the solubility of the precipitate. It provides examples like adding dilute sulfuric acid (which contains sulfate ions) to a saturated calcium sulfate solution, causing more calcium sulfate to precipitate out. It also discusses how adding sodium chloride to a solution of hydrochloric acid and water, or during soap making, provides more chloride or sodium ions that reduce the solubility of salts through competition.
COMMON ION EFFECT
The statement of the common ion effect can be written as follows – in a solution wherein there are several species associating with each other via a chemical equilibrium process, an increase in the concentration of one of the ions dissociated in the solution by the addition of another species containing the same ion will lead to an increase in the degree of association of ions.
An example of the common ion effect can be observed when gaseous hydrogen chloride is passed through a sodium chloride solution, leading to the precipitation of the NaCl due to the excess of chloride ions in the solution (brought on by the dissociation of HCl).
This effect cannot be observed in the compounds of transition metals. This is because the d-block elements tend to form complex ions. This can be observed in the compound cuprous chloride, which is insoluble in water. This compound can be dissolved in water by the addition of chloride ions leading to the formation of the CuCl2– complex ion, which is soluble in water.
Effect on Solubility:
How the solubility of a salt in a solution is affected by the addition of a common ion is discussed in this subsection.
The common ion effect can be used to obtain drinking water from aquifers (underground layers of water mixed with permeable rocks or other unconsolidated materials) containing chalk or limestone. Sodium carbonate (chemical formula Na2CO3) is added to the water to decrease the hardness of the water.
In the treatment of water, the common ion effect is used to precipitate out the calcium carbonate (which is sparingly soluble) from the water via the addition of sodium carbonate, which is highly soluble.
A finely divided calcium carbonate precipitate of a very pure composition is obtained from this addition of sodium carbonate. The CaCO3 precipitate is, therefore, a valuable by-product that can be used in the process of manufacturing toothpaste.
Since soaps are the sodium salts of carboxylic acids containing a long aliphatic chain (fatty acids), the common ion effect can be observed in the salting-out process which is used in the manufacturing of soaps. The soaps are precipitated out by adding sodium chloride to the soap solution to reduce its solubility.
However, it can be noted that water containing a respectable amount of Na+ ions, such as seawater and brackish water, can hinder the action of soaps by reducing their solubility and therefore their effectiveness.
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.
Anions
1. Qualitative inorganic analysis involves the detection and identification of anions in samples. Anions are divided into six groups including carbonates, sulphur-containing anions, halides, cyanogen, arsenic/phosphorus, and nitrogen-containing.
2. Carbonates and bicarbonates react with acids to produce carbon dioxide gas. Sulphur-containing anions such as sulphides, sulphites, thiosulphates and sulphates are identified through reactions that produce precipitates, gases, or color changes with reagents like barium chloride, silver nitrate, and iron (III) chloride.
3. Common tests involve observing properties like solubility, as
Salt hydrolysis
Salt hydrolysis can produce acidic, basic, or neutral solutions depending on the salt. Salts are classified based on whether they contain strong acids/bases or weak acids/bases. Salts of strong acids and bases do not undergo hydrolysis and produce neutral solutions. Salts of weak acids and strong bases produce basic solutions, while salts of strong acids and weak bases produce acidic solutions. Salts of weak acids and bases may produce neutral, acidic, or basic solutions. Solubility products define the solubility of sparingly soluble salts in solution. The common ion effect suppresses the dissociation of weak electrolytes in the presence of strong electrolytes with a common ion. Solubility products and common ion effects can be applied
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1) A list of group members and their student IDs working on the project.
2) Learning outcomes about defining acids, bases and alkalis and their uses.
3) A video link about the introduction to acids and bases.
4) Definitions and examples of acids, bases, and alkalis. Chemical reactions are shown to demonstrate their properties.
5) Types of acids and bases. Uses of acids, bases and alkalis in daily life are discussed.
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How the addition of CaCl2 affects the molar solubility of the compound.docx
How the addition of CaCl2 affects the molar solubility of the compound Ca(OH)2? Explain and justify
How the addition of CaCl2 affects the molar solubility of the compound Ca(OH)2? Explain and justify
Solution
Calcium hydroxide (Ca(OH)2) is a sparingly soluble salt. The salt which is dissolved in the water is normally ionized as follows.
Ca(OH)2 <---------------> Ca+2 + 2OH-
This is equilibrium ionization process and can be affected by several factors.
According to le chateliers principle if you increase the concentration of either Ca+2 or OH- ions in the solution, the equilibrium shifts towards backward direction and thereby the solubility of Ca(OH)2 would be decreased.
ISo, by the addition of CaCl2 which is normally ionize as follows CaCl2 <--------> Ca+2 + 2Cl-, would increase the concentration of Ca+2 ions in the solution. So, the number of Ca+2 ions is increased in the solution and the equilibrium is shifted towards backside due to the formation of Ca(OH)2.
So the equilibrium constant for the Ca(OH)2 in the absence of CaCl2 > in the presence of CaCl2
So the molar solubility of Ca(OH)2 would be decreased by the addition of CaCl2 salt.
.
Anions 120108105251-phpapp02
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2) Key reactions described include the evolution of carbon dioxide gas from carbonates and bicarbonates with hydrochloric acid, and the evolution of sulfur dioxide gas from sulfites and thiosulfates with hydrochloric acid.
3) Precipitation reactions with reagents like barium chloride, calcium chloride, and silver nitrate are used to identify anions based on the insoluble compounds formed.
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1) Carbonates and bicarbonates react with acids to produce carbon dioxide gas, which turns limewater milky. Sulfur-containing anions like sulfides, sulfites and thiosulfates are reducing and react with acids.
2) Common tests involve adding reagents like barium chloride, silver nitrate, and iron (III) chloride to detect anions via formation of insoluble precipitates.
3) The document provides details on solubility rules and characteristic reactions for each group of anions to allow their identification in mixtures
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This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
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The document discusses qualitative inorganic analysis of anions, specifically focusing on carbonates/bicarbonates and sulfur-containing anions. It describes the general characteristics, solubility, and common reactions of these anion groups. Key points include that carbonates and bicarbonates react with acids to produce carbon dioxide gas, while sulfur-containing anions like sulfides, sulfites, and thiosulfates act as reducing agents and react with reagents to produce characteristic colors or precipitates. Common tests involve the use of acids, silver nitrate, barium chloride, and iron (III) chloride.
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.
Question 1. Dscribe the change you observed when you added 1 mL of 0.pdf
Question 1 5 pts Given the cash flow diagram below, evaluate the value of \"A\" if the \"F\"
value is $24.000 for an interest rate of 7%. ?? 4A
Solution
Future Value of investents: Year Investment Future Value of Investment of 1 Future
Value of Investment a b c=1.07^(5-a) d=b*c 1 A 1.3108
1.3108 A 2 2A 1.2250 2.4501 A 3 3A 1.1449
3.4347 A 4 4A 1.0700 4.2800 A
11.4756 A Now, As per question, 11.4756 A = $
24,000 or, A = $ 2,091.40 Thus, Value of A $ 2,091.40.
Ch19 130105195803-phpapp02
This document summarizes Chapter 19 from a general chemistry textbook. The chapter covers solubility product constants, solubility equilibria, common ion effects, limitations of Ksp, precipitation criteria, fractional precipitation, solubility and pH, and equilibria involving complex ions. It provides examples and explanations of these concepts. Qualitative cation analysis is also discussed, describing how cations can be selectively precipitated into groups for identification purposes.
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Sodium, magnesium, and aluminium react with oxygen to form ionic oxides. Sodium oxide and magnesium oxide are basic due to their oxide ions and react with water to form alkaline solutions. Aluminium oxide is amphoteric as it displays both acidic and basic properties, reacting with both acids and bases. Silicon dioxide does not react with water or acids due to its covalent bonding. Phosphorus and sulphur form acidic oxides that react with water to produce acids. Chlorine forms oxides that react with water to form acids or salts.
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2) All alkalis are bases that dissolve in water, producing hydroxide ions, but not all bases dissolve in water.
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Sodium bicarbonate (Na+HCO3- ) is mildly alkaline.pdf
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid.
Solution
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid..
Acid base eqm and solubility equilibrium
This chapter talks about:
Acid –base equilibria
solubility equilibria
Buffer solution
Acid-base titration
Molar solubility and solubility
pH and Solubility
For more materials subscribe to channel:
https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w
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.
Ionic equilibrium part 2
The document summarizes key concepts regarding ionic equilibrium and solubility products. It discusses four types of salt hydrolysis and how they result in acidic, basic, or neutral solutions. It then defines solubility product and solubility product expressions for different types of salts. The solubility product principle is introduced, stating that precipitation will occur when the ionic product exceeds the solubility product constant.
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3) A video link about the introduction to acids and bases.
4) Definitions and examples of acids, bases, and alkalis. Chemical reactions are shown to demonstrate their properties.
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Solution
Calcium hydroxide (Ca(OH)2) is a sparingly soluble salt. The salt which is dissolved in the water is normally ionized as follows.
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- Common acids like hydrochloric acid and common bases like sodium hydroxide.
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Question 1. Dscribe the change you observed when you added 1 mL of 0.pdf
Question 1 5 pts Given the cash flow diagram below, evaluate the value of \"A\" if the \"F\"
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Solution
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Sodium, magnesium, and aluminium react with oxygen to form ionic oxides. Sodium oxide and magnesium oxide are basic due to their oxide ions and react with water to form alkaline solutions. Aluminium oxide is amphoteric as it displays both acidic and basic properties, reacting with both acids and bases. Silicon dioxide does not react with water or acids due to its covalent bonding. Phosphorus and sulphur form acidic oxides that react with water to produce acids. Chlorine forms oxides that react with water to form acids or salts.
Sulphuric acid
Sulfuric acid is a highly corrosive and toxic mineral acid that is produced industrially via the contact process. It involves burning sulfur to produce sulfur dioxide, converting the sulfur dioxide to sulfur trioxide via reaction with oxygen over a vanadium catalyst, and then reacting the sulfur trioxide with water to form sulfuric acid. Sulfuric acid is a strong acid that is widely used in industry for processes like oil refining, fertilizer production, and metal processing due to its oxidizing and dehydrating properties. It can cause severe burns upon contact with skin or tissues.
Acids, Bases and Indicators Part 3
1) Acids dissociate in water to produce hydrogen (H+) ions, while bases dissociate in water to produce hydroxide (OH-) ions.
2) All alkalis are bases that dissolve in water, producing hydroxide ions, but not all bases dissolve in water.
3) When diluting acids or bases, the substance should be slowly added to water with caution taken, as the reaction gives off heat. Water should never be added to the acid or base.
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline.pdf
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid.
Solution
Sodium bicarbonate (Na+HCO3- ) is mildly alkaline and it reacts withacids: H+ +
HCO3- =H2CO3 (carbonic acid) which is unstable inwater and breaks down into water &
Carbon Dioxide : H2CO3(aq) --> H2O(l) + CO2 (g) . Inan open container at atmospheric
pressure, the CO2 escapes, so thereaction is irreversible. Alka Seltzer must contain some
mildacid in solid form, maybe acetylsalicylic acid (aspirin). When placed in water, the acid and
bicarbonate react and fizz(CO2). Bicarbonate is useful in antacids for the same reason- stomach
acid (HCl) reacts with the bicarbonate producing waterand carbon dioxide. The carbon dioxide
leaves (burp!) andonly water remains where there once was a strong acid..
Acid base eqm and solubility equilibrium
This chapter talks about:
Acid –base equilibria
solubility equilibria
Buffer solution
Acid-base titration
Molar solubility and solubility
pH and Solubility
For more materials subscribe to channel:
https://www.youtube.com/channel/UCzXxV4xER9NIWt316gfeO1w
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.
Ionic equilibrium part 2
The document summarizes key concepts regarding ionic equilibrium and solubility products. It discusses four types of salt hydrolysis and how they result in acidic, basic, or neutral solutions. It then defines solubility product and solubility product expressions for different types of salts. The solubility product principle is introduced, stating that precipitation will occur when the ionic product exceeds the solubility product constant.
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Common ion effect
- 1. COMMON ION EFFECT MAIN POINTS ARE:
- 2. DEFINITIONS The solubility of an ionic precipitate decreases when a soluble compound containing one of the ions of the precipitate is added to the solution. Hg2Cl2 (s) Hg2+2 + 2Cl- The shifts in equilibrium that occurs because of the addition of an ion already involved in the equilibrium reaction. AgCl(s) Ag+(aq) + Cl-(aq)
- 3. Explanation of an example: ➢A saturated solution of calcium sulphate. CaSO4(s) Ca2+(S) + 2Cl- ➢ Ksp = [Ca2+] [SO42-] = 2.4 into 10-3 mol dm-6 at 298K ➢When a solution that contains the same ion is added to the saturated CaSO4 solution for e:g dilute H2SO4 : equilibrium shift to left,CaSO4 will precipitate out. ➢In presence of the additional COMMON ION (SO42-) the CaSO4 becomes less soluble. In solution ca ions are used and CaSO4 will precipitate out.
- 4. This Photo by Unknown author is licensed under CC BY-SA.
- 5. This Photo by Unknown author is licensed under CC BY-SA-NC.
- 6. PARTCIPATION OF COMMON ION EFFECT PARTICIPATION OF COMMON ION EFFECT OF CRUDE COMMON SALT: The PURIFICATION common ion effect can make insoluble substances more insoluble. An example of common ion effect is when sodium chloride is added to a solution Of HCl and water. The hydrochloric acid and water are in equilibrium with the products Being H3O+ and Cl-. Then some sodium chloride is added to the solution. HCl(g) + H2O H3O+ + Cl-
- 7. This Photo by Unknown author is licensed under CC BY-SA.
- 8. SALTING – OUT OF SOAP: The salting out process used in the manufacturing of soaps benefits from the common ion Effect. Soaps are sodium salts of fatty acids. Addition of sodium chloride reduces the solubility Of soap salts. In the presence of excess Na+ the reduced making the soap less effective. RCOONa Na+ + RCOO- NaCl Na+ + Cl-
- 9. This Photo by Unknown author is licensed under CC BY-NC-ND.