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The document provides a chemistry problem set involving calculations of hydrogen ion (H+) and hydroxide ion (OH-) concentrations in solution, definitions and calculations of pH and pOH, and properties of strong acids, weak acids, and weak bases. It asks students to calculate pH and concentrations of H+ given OH- concentrations and vice versa. It also asks students to list strong acids and bases, properties of strong and weak acids, what weak acids and bases have in common, and why HCl is a strong acid but weak base.
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![GENERAL CHEMISTRY-II (1412)
S.I. # 20
1. Calculate the concentration of H+ (aq) in (a) a solution in which [OH-] is 0.010 M,
(b) a solution in which [OH-] is 1.8x10-9 M.
2. Define pH and give the formula by which it is calculated.
3. Calculate the pH of a solution when the value of [H+] is 1.0 x 10-7M and when [H+]
is 1.0 x 10-3M.
4. Give the pH of a solution when the value of [OH-] is 2.0 x 10-3M.
5. Determine [H+] if the pH of a sample is 3.76.](https://image.slidesharecdn.com/chem-ii-si-20-1272476774-phpapp01/85/20-1-320.jpg)
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#20 Key
The document provides information about acid-base chemistry including:
1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions.
2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values.
3) Relating pH and pOH through the equation pH + pOH = 14.
4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.
Tabla de Ka y pKa
Tabla de Ka y pKa nos muestra acidos con sus respectivas constantes de acides y pka's. En la tabla se ve el nombre del acido, su formula quimica, su acido conjugado su base conjugada, y la fuerza de estos.
Ab Lec1
Acids and bases can be defined operationally based on experimental observations or conceptually based on theories. Operationally, acids are sour electrolytes that turn litmus red and react with metals, while bases are bitter electrolytes that turn litmus blue. Conceptually, acids are proton donors according to Arrhenius and Bronsted-Lowry, or electron pair acceptors according to Lewis. Conjugate acid-base pairs involve the transfer of a proton between an acid and its conjugate base. The strength of an acid or base depends on its tendency to donate or accept protons.
#19 Key
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
How do we measure acids and bases
This document discusses pH and how it is used to measure the acidity or basicity of solutions. It explains that pH is determined by measuring the concentration of hydrogen ions [H+] or hydronium ions [H3O+] in a solution. The pH scale ranges from 0 to 14, with acids having a pH below 7, bases above 7, and neutrals at 7. It also provides examples of calculating the pH of acid and base solutions given their concentrations.
Ionic Equilibria - Acid & Base
This document discusses ionic equilibria, specifically acid-base and solubility equilibria. It provides information on acid-base titration curves and indicators. Key points covered include:
- The definitions and reactions of strong/weak acids and bases, and how to determine if a salt is acidic, basic, or neutral based on the ions.
- How to calculate pH for solutions containing acids, bases, salts, and buffers using the relevant equilibrium expressions.
- The three important points on a titration curve and what parameters can be determined at each point.
- The step-by-step approach for solving acid-base equilibrium problems.
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The document provides 10 questions related to general chemistry concepts including:
1) Defining the common ion effect and buffer capacity
2) Providing the Henderson-Hasselbalch equation
3) Calculating the pH of different buffer solutions
#25 Key
1. The common ion effect decreases the ionization of a weak electrolyte when a strong electrolyte with a common ion is added to the solution.
2. Buffer capacity refers to how much acid or base can be neutralized before the pH begins to change significantly.
3. A buffer solution contains a weak acid or base and its salt. It has the ability to resist changes in pH.
4. The pH range of a buffer depends on the acid's Ka value and the relative concentrations of the acid and base in the buffer solution. It is the range over which the buffer acts effectively.
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#20 Key
The document provides information about acid-base chemistry including:
1) Calculating the concentration of H+ ions and determining if solutions are acidic or basic based on the relative concentrations of H+ and OH- ions.
2) Defining pH as the negative logarithm of the H+ ion concentration and calculating pH values from given [H+] values.
3) Relating pH and pOH through the equation pH + pOH = 14.
4) Listing the 7 strong acids and their formulas as well as the 7 strong bases and their formulas.
Tabla de Ka y pKa
Tabla de Ka y pKa nos muestra acidos con sus respectivas constantes de acides y pka's. En la tabla se ve el nombre del acido, su formula quimica, su acido conjugado su base conjugada, y la fuerza de estos.
Ab Lec1
Acids and bases can be defined operationally based on experimental observations or conceptually based on theories. Operationally, acids are sour electrolytes that turn litmus red and react with metals, while bases are bitter electrolytes that turn litmus blue. Conceptually, acids are proton donors according to Arrhenius and Bronsted-Lowry, or electron pair acceptors according to Lewis. Conjugate acid-base pairs involve the transfer of a proton between an acid and its conjugate base. The strength of an acid or base depends on its tendency to donate or accept protons.
#19 Key
This document discusses Bronsted-Lowry acid-base chemistry. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. It explains that conjugate acids are formed by adding a proton to a base and conjugate bases are formed by removing a proton from an acid. Several examples of conjugate acid-base pairs are given. The document also states that the stronger the acid, the weaker its conjugate base, and the stronger the base, the weaker its conjugate acid. It describes how the position of equilibrium favors transfer of a proton to the stronger base. Finally, it provides the autoionization reaction of water and defines the ion product constant, Kw, for water.
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This document discusses pH and how it is used to measure the acidity or basicity of solutions. It explains that pH is determined by measuring the concentration of hydrogen ions [H+] or hydronium ions [H3O+] in a solution. The pH scale ranges from 0 to 14, with acids having a pH below 7, bases above 7, and neutrals at 7. It also provides examples of calculating the pH of acid and base solutions given their concentrations.
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This document discusses ionic equilibria, specifically acid-base and solubility equilibria. It provides information on acid-base titration curves and indicators. Key points covered include:
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- How to calculate pH for solutions containing acids, bases, salts, and buffers using the relevant equilibrium expressions.
- The three important points on a titration curve and what parameters can be determined at each point.
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2. Buffer capacity refers to how much acid or base can be neutralized before the pH begins to change significantly.
3. A buffer solution contains a weak acid or base and its salt. It has the ability to resist changes in pH.
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This document covers Bronsted-Lowry acids and bases, conjugate acids and bases, and acid-base equilibrium. It defines Bronsted-Lowry acids as proton donors and bases as proton acceptors. Conjugate acids are formed when a base gains a proton, and conjugate bases are formed when an acid loses a proton. Several examples of conjugate acid-base pairs are given. The document also discusses how the strength of an acid or base determines the position of acid-base equilibrium and the autoionization process and ion product constant for water.
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The document provides instructions to name and write formulas for various acids and bases. It lists 20 acids and bases and asks the reader to provide their names or formulas. The acids and bases include sulfuric acid, sulfurous acid, hydrogen sulfide, phosphoric acid, nitric acid, hydrocyanic acid, hydrofluoric acid, carbonic acid, nitrous acid, acetic acid, perchloric acid, chloric acid, hydrobromic acid, oxalic acid, boric acid, bromic acid, and phosphorous acid.
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This document summarizes acids and bases according to two theories - Arrhenius and Bronsted-Lowry. According to Arrhenius, an acid is a substance that ionizes in water to produce hydrogen ions, while a base produces hydroxide ions. Bronsted-Lowry defined acids as proton donors and bases as proton acceptors, with no requirement for aqueous solutions. Conjugate acid-base pairs are also discussed, where a conjugate acid is a base that accepts a proton, and a conjugate base is an acid that donates a proton.
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The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
- Lewis in 1923 expanded the definition to electron pair transfers between any acids and bases, not just involving hydrogen.
- Other theories such as Lux-Flood's oxygen theory of 1939 and Pearson's hard/soft acid base principle
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This document provides an overview of acid-base theories and key concepts such as:
[1] Arrhenius and Brønsted-Lowry definitions of acids and bases. Acids donate protons while bases accept protons.
[2] Water can act as both an acid and a base in different reactions due to its amphiprotic nature.
[3] Equilibria involving proton transfers favor the reaction where the proton moves to the stronger base. The position of equilibrium is determined by relative acid and base strengths.
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This document provides an overview of acids and bases, including:
- Water can act as both an acid and a base in chemical reactions.
- The autoionization of water establishes an equilibrium expression relating [H3O+] and [OH-].
- Adding acids or bases shifts the equilibrium by changing [H3O+] or [OH-] while maintaining the same Kw expression.
- pH is a measure of acidity and is defined as -log[H3O+], with lower pH indicating higher acidity.
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Sandrogreco Tabela De P Ka
This document contains tables summarizing pKa values for various inorganic acids, organic acids, alcohols, amines, and other compounds. The tables include the substrate, its pKa values in both water and DMSO as a solvent, and are organized by functional groups including carboxylic acids, alcohols, amines, heterocycles, and carbonyl compounds. This comprehensive compilation of pKa data from multiple tables provides chemists with a reference for the acidity of different functional groups in aqueous and non-aqueous solutions.
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1) Water can act as both an acid and a base, donating or accepting protons in chemical reactions.
2) Water undergoes autoionization, reacting with itself to form hydronium and hydroxide ions. The equilibrium constant for this reaction is known as Kw.
3) In pure water at 25°C, Kw equals 1.0 × 10-14, meaning the concentrations of hydronium and hydroxide ions are both 1.0 × 10-7.
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This document discusses autoionization of water and concepts related to acid-base chemistry including:
- In neutral solutions, the concentrations of H3O+ and OH- are equal to each other based on the water ion product constant.
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- Strong acids and bases completely ionize in solution, allowing their concentrations to determine H3O+ or OH- concentrations.
- Weak acids and bases only partially ionize in solution, with their extent of dissociation determined by their acid or base ionization constant (Ka or Kb).
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2. It explains the ion product constant of water (Kw) and how pH and pOH scales are used to measure hydrogen and hydroxide ion concentrations.
3. Weak acids and bases only partially dissociate in water and their equilibria are expressed using acid (Ka) and base (Kb) dissociation constants.
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This document discusses acids and bases, including:
- The Arrhenius definition of acids and bases as substances that increase H+ or OH- ions in water.
- The Brønsted-Lowry definition of acids as proton donors and bases as proton acceptors.
- Conjugate acid-base pairs that differ by the presence or absence of a proton.
- Amphoteric substances that can act as both acids and bases, such as water.
- The pH scale for measuring the concentration of hydrogen ions in a solution.
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asam dan basa
This document provides an overview of acid-base concepts including definitions, examples, and calculations. It defines acids as producing H+ ions and bases as producing OH- ions. Strong acids and bases fully dissociate in water while weak acids and bases partially dissociate. Acids are proton donors and bases are proton acceptors. The document also discusses using pH and pOH scales to calculate hydrogen and hydroxide ion concentrations in solutions and determine whether they are acidic or basic.
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The document provides instructions to name and write formulas for various acids and bases. It lists 20 acids and bases and asks the reader to provide their names or formulas. The acids and bases include sulfuric acid, sulfurous acid, hydrogen sulfide, phosphoric acid, nitric acid, hydrocyanic acid, hydrofluoric acid, carbonic acid, nitrous acid, acetic acid, perchloric acid, chloric acid, hydrobromic acid, oxalic acid, boric acid, bromic acid, and phosphorous acid.
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1) The common ion effect where adding a strong electrolyte containing a common ion with a weak electrolyte decreases the ionization of the weak electrolyte.
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3) Solubility products (Ksp) and how solubility is affected by factors like common ions, pH, and complex ion formation.
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The document discusses weak acids and bases. It defines them as substances that are only partially ionized in solution, with a degree of ionization (α) less than 1. Examples of weak acids given are H2C2O4, HNO2, CH3COOH, H3PO4, and HF. Examples of weak bases include NH4OH, Be(OH)2, AgOH, and Zn(OH)2. Formulas are provided for calculating the concentration of H+ ions in weak acids or OH- ions in weak bases based on the acid or base concentration and equilibrium constant. The pH of solutions is also explained in relation to weak acids and bases.
Mofppb3 slides presentation on acids & bases
This document summarizes acids and bases according to two theories - Arrhenius and Bronsted-Lowry. According to Arrhenius, an acid is a substance that ionizes in water to produce hydrogen ions, while a base produces hydroxide ions. Bronsted-Lowry defined acids as proton donors and bases as proton acceptors, with no requirement for aqueous solutions. Conjugate acid-base pairs are also discussed, where a conjugate acid is a base that accepts a proton, and a conjugate base is an acid that donates a proton.
Acid and base
The document discusses several theories of acids and bases that developed over time:
- Lavoisier's original oxygen theory defined acids as containing oxygen (1776). This was disproven by Davy in 1810.
- Liebig proposed in 1838 that acids contain replaceable hydrogen.
- Arrhenius' 1884 definition defined acids as producing hydrogen ions (H+) and bases as producing hydroxide ions (OH-) in aqueous solutions, which became the standard definition.
- Lewis in 1923 expanded the definition to electron pair transfers between any acids and bases, not just involving hydrogen.
- Other theories such as Lux-Flood's oxygen theory of 1939 and Pearson's hard/soft acid base principle
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1. The document discusses key concepts from general chemistry including:
- The van der Waals equation accounting for non-zero particle volumes and interparticle interactions.
- Using the ideal gas law to calculate changes in volume with temperature changes.
- The value of the gas constant R at standard temperature and pressure.
- Conversions between various pressure and volume units.
- Calculating moles, pressure, volume, and number of molecules using the ideal gas law.
#18
This document contains 6 chemistry problems involving gas phase chemical equilibria. Problem 1 involves calculating the equilibrium partial pressure and equilibrium constant for the reaction N2O4(g) ⇌ 2NO2(g). Problem 2 involves calculating equilibrium concentrations and the equilibrium constant for the reaction H2(g) + Br2(g) ⇌ 2HBr(g). Problem 3 asks to calculate the equilibrium constant for the reaction SO2(g) + Cl2(g) ⇌ SO2Cl2(g) given the value of Kp at a specific temperature.
Key SI #6
Intermolecular forces exist between molecules, while intramolecular forces exist within molecules. Melting points increase as intermolecular forces strengthen. Polar molecules have partial charges and can form ion-dipole attractions. The main intermolecular forces are London dispersion, dipole-dipole, and hydrogen bonding. Ionic and covalent bonds are stronger than any intermolecular force within a molecule. A flow chart determines the dominant intermolecular force based on whether ions or polar molecules are present.
SI #10
This document contains 11 multiple choice and short answer questions about concepts in general chemistry including: solvent-solute interactions, hydration, enthalpy of solution, colligative properties, molality calculations, definitions of colloid and miscibility, concentration calculations involving mass percent and ppm, and molality calculations for solutions.
Si #15
The document discusses reaction rates and kinetics. It defines reaction rate and states that the concentration of reactants is proportional to the rate of reaction. It also defines the rate constant and rate law formula. A catalyst affects the reaction rate by lowering the activation energy, increasing the frequency of collisions, and increasing the probability of successful collisions. Enzymes are biological catalysts and the collision theory states that for a reaction to occur, reactant particles must collide with adequate energy.
SI #9
The document is a practice exam for general chemistry II that contains 10 multiple choice questions testing knowledge of intermolecular forces, phase changes, concentrations, vapor pressure, and nomenclature. It asks about the forces between molecules, which substance experiences only dispersion forces, the process of molecules sticking to a surface, the energy required to expand a liquid's surface area, the vapor pressure at the normal boiling point, the concentration of nitrate ions in a solution, the direct change of a solid to a gas, and the phase changes of water freezing and drying and frost forming. It concludes by listing the names and symbols of 10 chemical substances and compounds.
SI #11
The document contains 10 chemistry problems related to calculating molarity and percent composition of solutions, osmotic pressure, boiling points of solutions, definitions of hydrophilic and hydrophobic colloids, and identifying examples of each. It also contains 10 chemistry nomenclature problems to identify chemical formulas and names.
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The document summarizes key concepts about acids and bases from an introductory chemistry textbook. It defines acids and bases according to the Arrhenius, Brønsted-Lowry, and Lewis theories. It also discusses acid-base properties and reactions, pH and pOH scales, strong vs. weak acids/bases, and calculating pH for acid/base solutions.
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The document discusses acid-base titrations and pH. It defines pH as the negative logarithm of hydronium ion concentration and explains how to calculate pH from [H3O+] and vice versa. It also describes how to perform and calculate molarity from a titration experiment by determining moles of acid/base reacted using volume and molarity of the titrant. Sample titration problems are worked through demonstrating these concepts.
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This document discusses acid-base equilibria and the key concepts of acids, bases, pH and pOH. It begins with a review of the Arrhenius and Brønsted-Lowry definitions of acids and bases. Key points covered include: water can act as both an acid and a base; conjugate acid-base pairs are formed in acid-base reactions; and the pH scale relates hydrogen ion concentration to acidity. Strong acids and bases are defined as completely dissociating in water.
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This document provides an overview of acids and bases, including:
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acids and bases
The document discusses key concepts regarding acids and bases including: Bronsted-Lowery acids and bases, conjugate acid-base pairs, the pH scale, strong and weak acids and bases, acid-base properties of salts, and Lewis acids and bases. Key equations discussed include the ionization of water and the autoionization constant Kw. Sample problems are provided for calculating pH, percentage of ionization, and acid and base dissociation constants.
AP Chemistry Chapter 16 Sample Exercises
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This document provides an introduction to principles of chemistry lab II, covering acids and bases, pH, buffers, and hydrolysis. Key points include:
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Apchemunit15presentation 120311192458-phpapp01
1. This unit covers acid-base chemistry including solutions containing a common ion, buffered solutions, and titrations.
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3. Titration curves are generated by plotting pH versus volume of titrant added. The pH changes slowly until near the equivalence point, where a small change in titrant produces a large pH change as the ratio of [H+]/[OH-] changes dramatically.
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The document discusses acids, bases, and salts. It provides information on the Arrhenius and Bronsted-Lowry theories of acids and bases. Key points include: Arrhenius acids contain H+ ions and bases contain OH- ions. Bronsted-Lowry defined acids as proton donors and bases as proton acceptors. Acids have a pH below 7 while bases are above 7. Neutralization reactions involve acids and bases reacting to form water and a salt. Titration can be used to determine the concentration of an unknown acid or base solution.
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Chapter 5&6
analytical Chemistry just the basic one. consists of compleximetric titration and the principle titration
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This document provides definitions and information about acids and bases:
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ModuleAnalytical MeasurementTutorCodeICAExcel si.docx
Module
Analytical Measurement
Tutor
Code
ICA
Excel simulation of a titration involving strong acid and a weak base (or v.v.)
2nd Marker
Weight
50%
Type
Online submission
Produce an Excel spreadsheet based on simulation to illustrate the variation of the pH of the solution that occurs when strong acid is added to a weak base (or strong alkali and weak acid). The spreadsheet should demonstrate the change in the pH of the mixture as the titrant is added for a range of concentration of both components. Particular attention should be paid to the behaviour close to the end point (or equivalence point). Graphs should be generated on a range of scales showing in detail the likely behaviour around the end point.
The exact calculations for all situations can be quite involved so it may be useful to divide the titration into various segments in which various equations and approximations are valid and then stitch these together.
Write a report explaining the design of your spreadsheet and describe the graphs, which you should import.
Write a short description of the theory of buffer solutions and give examples of their applications.
The report should be a word document and an Excel spreadsheet. Describe the background theory and the methodology behind the construction of the simulation, and include the realisation of the system equations in Excel formulae. Graphs of pH against added solution over various ranges and around particular key points – such as the equivalence point or “end point”.
[60 marks]
The report should also include a discussion of the concept of buffer solutions and give examples of their use either in industrial processes or naturally occurring phenomena. Any sources should be appropriately referenced (Harvard).
[40 marks]
assignhints(1).pptx
Hints for the Assignment Weak Monoprotic AcidsNameFormulaValue of KaMonochloracetic acid
Hydrofluoric acid
Nitrous acid
Formic acid
Lactic acid
Benzoic acid
Acetic acid
Hydrated aluminum(III) ion
Propanoic acid
Hypochlorous acid
Hypobromous acid
Hvdrocyanic aid
Boric acid
Ammonium ion
Phenol HC2H3ClO2
HF
HNO2
HCO2H
HC3H5O3
HC7H502
HC2H3O2
[Al (H20)6]3+
HC3H5O2
HOCl
HOBr
HCN
H3BO3
NH4+
HOC6H5
HOI 1.35 x 10 -3
7.2 x 10-4
4.0 x 10-4
1.8 x 10-4
1.38 x 10-4
6.4 x 10-5
1.8 x 10-5
1.4 x 10-5
1.3 x 10-5
3.5 x 10-8
2 x 10-9
6.2 x 10-10
5.8 x 10-10
5.6 x 10-10
1.6 x 10-10
2 x 10-11
Weak Alkalis or BasesFormulaNameKbNH3ammonia
1.8 x 10 -5CH3NH2methylamine
4.4 x 10 -4C5H5Npyridine
1.5 x 10 -9C6H5NH2aniline4.3 x 10 -10
It is possible to set up a simulated titration between a weak acid and a strong base.
It is easier to work backwards from pH to the added volume of titrant using the equations below as [H+] = 10(-pH)
It is possible to generate the curve with just one formula going backwards.
However we know by working forwards from added volume to pH that there are certain key points of interest, namely where φ = 0, 0.5, 1 and >1.
...
Ap chem unit 15 presentation
Here are the ratios [HA]/[A-] required for each system to yield a pH of 4.30:
Acetic acid (pKa = 4.76): [HA]/[A-] = 1
Benzoic acid (pKa = 4.19): [HA]/[A-] = 1
Phthalic acid (pKa = 2.89): [HA]/[A-] is not possible since the pKa is too low.
The optimal system is acetic acid/sodium acetate since it has a pKa closest to the desired pH of 4.30. This system allows a ratio of [HA]/[A-] = 1, which provides maximum buffering
Ch14 z5e acid base
The document discusses different definitions of acids and bases, including:
1) Arrhenius definitions - acids produce H+ ions in water, bases produce OH- ions. Limited to aqueous solutions.
2) Bronsted-Lowry definitions - acids are H+ donors, bases are H+ acceptors. Acids and bases always come in pairs when reacting.
3) pH scale is used to express acidity because [H+] is usually very small. pH decreases as [H+] increases exponentially. Common substances are classified as acidic, basic, or neutral based on their pH.
Acid-Base-Equilibria.ppt
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Acids-Bases-pH-PPT-2018.ppt.organic-chemistry
This document discusses the chemistry of acids and bases. It defines acids as substances that produce hydrogen ions (H+) or hydronium ions (H3O+) in water, and bases as substances that produce hydroxide ions (OH-). It provides examples of common acids and bases and discusses their properties. Key topics covered include the Arrhenius, Brønsted-Lowry, and Lewis definitions of acids and bases; acid-base reactions; pH and pOH scales; strong and weak acids and bases; and acid-base equilibria.
AP Chemistry Chapter 16 Outline
This document provides an overview of acids and bases including:
- Definitions of acids and bases according to Arrhenius, Brønsted-Lowry, and Lewis theories
- How acids and bases react in water, forming conjugates
- Factors that influence acid and base strength such as polarity, resonance, and electronegativity
- Calculations involving acid and base dissociation constants (Ka and Kb) to determine pH
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Chem 132 principles of chemistry lab ii montgomery
Chem 132 principles of chemistry lab ii montgomery
ModuleAnalytical MeasurementTutorCodeICAExcel si.docx
ModuleAnalytical MeasurementTutorCodeICAExcel si.docx
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This document contains questions about oxidation-reduction reactions and voltaic cells. It asks the student to identify oxidizing and reducing agents, write half reactions, identify anodes and cathodes, and determine the direction of electron and ion flow. It also contains questions about standard cell potentials, units of electrical potential, and a half reaction for a hydrogen electrode.
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1. The document provides steps to convert between solubility in grams per liter, molar solubility in mol/L, molar concentrations of ions, and Ksp.
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This document provides examples of calculating the pH of various strong acid solutions, including nitric acid, perchloric acid, hydrochloric acid, a mixture of hydrochloric acid and hydroiodic acid, and a solution of bromoacetic acid that is partially ionized. It also asks questions about weak acids, Lewis acids, and which compounds form more acidic solutions based on cation properties.
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1. The document provides 7 chemistry problems involving calculations of pH, concentrations of products and reactants from acid-base reactions involving strong acids and bases, and identification of types of acids.
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The document contains 6 chemistry problems involving gas phase chemical equilibria calculations:
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1. The document contains 7 chemistry problems involving calculation of equilibrium constants (Keq and Kc) for various chemical reactions.
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This document contains 7 questions regarding chemical equilibrium calculations. The questions involve writing equilibrium constants, calculating equilibrium constants based on given partial pressures or concentrations at equilibrium, and determining unknown values at equilibrium given some known values. Specifically, it asks the student to:
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This document contains information about several chemistry concepts and example calculations:
1) It provides calculations to determine the amount of N2O5 remaining and reaction time for its decomposition reaction at 70°C.
2) It discusses how reaction rates change with changes in reactant concentrations for a reaction following a rate law.
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Si #12 Key
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The document contains a chemistry problem set with 10 questions:
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