Chapter 14.1 : Compounds in Aqueous Solutions
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1) Ionic compounds dissolve in water by dissociating into their constituent ions. For example, NaCl dissociates into Na+ and Cl- ions in water. 2) Aluminum sulfate, Al2(SO4)3, dissociates into 2 Al3+ and 3 SO42- ions when dissolved in water, producing a total of 5 moles of ions from 1 mole of the compound. 3) Precipitation reactions occur when opposite ions combine to form an insoluble ionic compound. For example, combining solutions of (NH4)2S and Cd(NO3)2 will produce the insoluble precipitate CdS.
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9 Aqueous Solutions
- Water is a polar solvent due to its molecular structure, with oxygen having a partial negative charge and hydrogen having partial positive charges. This allows it to dissolve ionic compounds by interacting with and separating the ions.
- Ionic compounds dissolve to varying degrees in water depending on how strongly the ions are attracted to each other versus water molecules. Solubility can be measured in g/L.
- Acids donate H+ ions in water and are classified as strong or weak based on how completely they ionize. Their strength affects pH calculations. Bases accept H+ and similarly ionize more or less completely.
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This document discusses properties of aqueous solutions and acid-base reactions. It describes how ionic compounds and electrolytes dissolve in water, forming ions that are solvated. Precipitation reactions that form insoluble products are explained. Strong and weak acids and bases are defined, and neutralization reactions that produce salts and water are covered. Some acid-base reactions evolve gas as one of the products.
Acid and base
Acids and bases can be classified based on their strength. Strong acids and bases fully dissociate in solution, while weak acids and bases only partially dissociate. The strength of an acid or base depends on factors like the polarity and stability of the conjugate ions. Acid-base reactions involve the transfer of protons between substances. The pH scale quantifies the concentration of hydrogen ions in a solution, relating acidity to the logarithm of the hydrogen ion concentration. Salts are formed by the neutralization of acids and bases.
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This document discusses acids and bases. It defines their key properties including reacting with metals, carbonates, conducting electricity, turning litmus paper colors, and neutralizing each other. It explains the theories of Arrhenius, Brønsted-Lowry, and Lewis on acids and bases. It also covers acid-base reactions, indicators, pH, titrations, strong/weak acids and bases, and acid-base stoichiometry.
Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
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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- Ionic compounds dissolve to varying degrees in water depending on how strongly the ions are attracted to each other versus water molecules. Solubility can be measured in g/L.
- Acids donate H+ ions in water and are classified as strong or weak based on how completely they ionize. Their strength affects pH calculations. Bases accept H+ and similarly ionize more or less completely.
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Theories
The document discusses several theories of acids and bases:
1. According to Arrhenius, acids are compounds that produce H+ ions in water and bases produce OH- ions. Strong acids fully dissociate while weak acids only partially dissociate.
2. Bronsted and Lowry defined acids as proton donors and bases as proton acceptors. An acid and base always work together in a proton transfer reaction. Some substances can act as both an acid and a base depending on the reaction.
3. Lewis defined acids as electron pair acceptors and bases as electron pair donors.
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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This document discusses different theories of acids and bases:
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2) Bronsted-Lowry theory defines acids as proton donors and bases as proton acceptors. Acid-base reactions involve proton transfer.
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4) pH measures hydrogen ion concentration on a logarithmic scale from 0-14.
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- Common indicators like litmus paper, phenolphthalein, and universal indicator can be used to estimate pH based on their color changes.
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3) Conjugate acid-base pairs are related - the conjugate base of an acid is its corresponding base, and vice versa.
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Acids release H+ ions in water and have sour tastes, while bases release OH- ions in water and feel slippery. Strong acids and bases completely ionize in water, while weak acids and bases only partially ionize. Common strong acids include sulfuric acid and hydrochloric acid, while strong bases include lithium hydroxide and sodium hydroxide. When acids and bases are mixed, they neutralize each other through a reaction that produces water and a salt. Indicators change color depending on whether the solution is acidic or basic, and can be used to measure the pH of a solution.
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- pH is a measure of hydrogen ion concentration in a solution on a scale from 0-14.
- A pH below 7 is acidic, above 7 is basic, and 7 is neutral.
- The pH scale is logarithmic, so each unit change in pH represents a 10-fold change in [H+].
- Common indicators like litmus paper, phenolphthalein, and universal indicator can be used to estimate pH based on their color changes.
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This document discusses acids and bases according to the Arrhenius and Brønsted-Lowry theories. It defines acids as substances that produce hydrogen ions (H+) or donate protons in water according to Arrhenius, and substances that donate protons according to Brønsted-Lowry. Bases are defined as substances that produce hydroxide ions (OH-) in water according to Arrhenius, and substances that accept protons according to Brønsted-Lowry. Examples of strong and weak acids and bases are given. The limitations of the Arrhenius theory and the concept of conjugate acid-base pairs are also outlined.
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colligative property ,made by-chinmay jagadev pattanayak
What is colligative property?
Types of colligative property
Lowering Vapour Pressure (∆P) of solutions.
Boiling point elevation.
Freezing point depression
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Chapter 14.1 : Compounds in Aqueous Solutions
- 1. Ions in aqueous solutions and Colligative properties Chapter 14.1
- 2. Objectives Write equations for the dissolution of soluble ionic compounds in water. Predict whether a precipitate will form when solutions of soluble ionic compounds are combined, and write net ionic equations for precipitation reactions Compare dissociation of ionic compounds with ionization of molecular compounds Draw the structure of the hydronium ion, and explain why it is used to represent the hydrogen ion in solution Distinguish between strong electrolytes and weak electrolytes
- 5. Precipitation Reactions Solubility Guidelines ( Table pg. 900 in text) Most sodium, potassium, and ammonium compounds are soluble in water. Mostnitrates, acetates, andchloratesare soluble. Most chlorides are soluble, except those silver, mercury(I), and lead. Lead(II) chloride is soluble in hot water. Most sulfates are soluble, except those of barium, strontium, and lead. Most carbonates, phosphates, and silicates are insoluble, except those of sodium potassium, andammonium. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, andammonium.
- 6. Will a precipitate form? (NH4)2S (s) 2 NH4+ (aq) + S2- (aq) Cd(NO3)2 (s) Cd2+ (aq) + 2 NO3- (aq) (NH4)2S (aq) + Cd(NO3)2 (aq) 2 NH4NO3 (aq) + CdS (s) Double Replacement Reaction Precipitate : Sulfides usually insoluble
- 7. Net ionic equations Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution. 2 NH4+(aq)+S2- (aq) + Cd2+(aq)+ 2 NO3-(aq) 2 NH4+ (aq)+2 NO3 -(aq) + CdS(s) Overall Ionic equation Spectator ions : Ions that do not take part in reaction They are found in solution before and after reaction Now , you have the Net Ionic Equation: Cd2+(aq)+ S2-(aq) CdS(s)
- 8. Ionization Ions are formed from solute molecules by the action of the solvent in a process Different than dissociation Molecular compounds form ions where there were none before HCl H+ (aq) + Cl- (aq) Hydronium ion H3O+ H2O(l) + HCl(g) H3O+(aq) + Cl-(aq)
- 9. Strong and Weak Electrolytes Strong electrolyte Any compound whose dilute aqueous solutions conduct electricity well; this is due to the presence of all or almost all of the dissolved compound in the form of ions. HCl, HBr, and HI completely ionize in water. H2O(l) + HCl(g) H3O+(aq) + Cl-(aq) Weak electrolyte Any compound whose dilute aqueous solutions conduct electricity poorly; this is due to the presence of a small amount of the dissolved compound in the form of ions. HF(aq) + H2O(l) H3O+(aq) + F-(aq)