Name: acetic acid buffer changes in titration
Uploaded: 2024-04-04T10:51:19.000Z
Duration: 1 min 17 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

solution-composition-during-acidbase-titrations

Solution Composition During Acid/Base Titrations

Przypomnijmy, że miareczkowanie kwasu octowego wodorotlenkiem sodu wytwarza octan sodu i wodę, w wyniku czego powstaje bufor.
Względne stężenie różnych gatunków w roztworze buforowym w różnych punktach miareczkowania jest wskazywane przez wartości alfa.
Podczas gdy linia zakrzywiona reprezentuje miareczkowanie kwasu octowego i wodorotlenku sodu, linie proste oznaczone jako węzeł alfa i alfa-on oznaczają odpowiednio względne stężenie równowagowe kwasu octowego i jonów octanowych.
Początkowo wartość węzła alfa wynosząca 0,987 sugeruje, że 98,7% kwasu octowego jest niezdysocjowane, a pozostałe 1,3% to jony octanowe.
W punkcie przecięcia lub w punkcie połówkowym równoważnikowym pH jest równe pKa. W związku z tym roztwór ma równe stężenie kwasu octowego i jonów octanowych.
W miarę postępu miareczkowania stężenie kwasu octowego, węzła alfa, spada prawie do zera w punkcie równoważnikowym. Alternatywnie, stężenie jonów octanu, alfa-onu, wzrasta i zbliża się do jedności.

skład roztworu podczas miareczkowania monoprotonowych kwasów/zasad

Miareczkowanie słabego kwasu mocną zasadą powoduje utworzenie wody i sprzężonej zasady kwasu. Na przykład miareczkowanie kwasu octowego wodorotlenkiem sodu prowadzi do powstania wody i octanu sodu. Roztwór kwasu octowego i octanu sodu stanowi bufor, którego względne stężenie na różnych etapach miareczkowania jest oznaczone wartościami α, które reprezentują procent słabego kwasu i jego sprzężonej zasady.

Wartości α0 i α1 reprezentują względne równowagowe stężenie odpowiednio jonów kwasu octowego i octanu. Przed dodaniem zasady wartości α0 i α1 wynoszą odpowiednio 0,987 i 0,013. Sugeruje to, że roztwór zawiera 98,7% kwasu octowego i 1,3% jonów octanowych. Po dodaniu wodorotlenku sodu podczas miareczkowania, α0 maleje, podczas gdy α1 wzrasta. W punkcie półrównoważności, gdzie pH jest równe pKa kwasu octowego, wartość α0 jest równa α1. Roztworem na tym etapie jest mieszanina 50% kwasu octowego i 50% jonów octanowych. W miarę postępu miareczkowania α0 maleje, a jego wartość spada do zera w punkcie równoważności. Wręcz przeciwnie, wartość α1 staje się jednością.

Skład roztworu podczas miareczkowania monoprotonowych kwasów/zasad

Przypomnijmy, że miareczkowanie kwasu octowego wodorotlenkiem sodu wytwarza octan sodu i wodę, w wyniku czego powstaje bufor.
Względne stężenie ...

Education

JoVE Core

Analytical Chemistry

Chemia analityczna

Unit 1

Jednostka 1

Acid–Base Titration

Miareczkowanie kwasowo-zasadowe

KEY TERMS AND CONCEPTS

KLUCZOWE POJĘCIA I KONCEPCJE

acetic acid buffer changes in titration

Acetic acid buffer changes during a weak acid–strong base titration. When acetic acid is titrated with sodium hydroxide, the reaction forms water and the conjugate base of the acid, sodium acetate. The mixture of acetic acid and sodium acetate acts as a buffer, which helps show how solution makeup shifts during the titration.

The relative amounts of acetic acid and acetate ions are tracked with α values. Here, α0 represents the equilibrium concentration of acetic acid, and α1 represents the equilibrium concentration of acetate ions. Before base is added, α0 is 0.987 and α1 is 0.013. That means the solution is about 98.7% acetic acid and 1.3% acetate ions.

As sodium hydroxide is added, α0 goes down and α1 goes up. At the half-equivalence point, the pH equals the pKa of acetic acid. At that stage, α0 and α1 are equal, so the solution contains 50% acetic acid and 50% acetate ions. As the titration continues to the equivalence point, α0 drops to zero and α1 becomes unity.

Acetic Acid Buffer Changes in Titration

acid&#8211;base titration: overview

Titration Curves and pH Changes

Acid-base titration uses a known acid or base to find the concentration of an unknown solution. A base can titrate an acid, or an acid can titrate a base. As titrant is added little by little, the pH changes in a predictable way. The pH change is shown on a titration curve. A titration curve plots how the pH of the solution changes as more titrant is added. Scientists use this curve to follow the progress of the titration and to identify the endpoint, which is the point used to stop the...

titration of a strong acid with a strong base

titration-of-a-strong-acid-with-a-strong-base

pH Changes in Strong Acid-Base Titration

pH changes in a strong acid-strong base titration depend on the amount of leftover hydronium or hydroxide ions. A strong acid such as hydrochloric acid fully dissociates in water. That gives the solution hydronium ions and chloride ions, so the starting pH is low. When sodium hydroxide is added, it neutralizes hydronium ions. As more base is added, the concentration of hydronium ions falls and the pH rises. At the equivalence point, the hydronium ions have been neutralized and the solution is...

titration of a weak acid with a strong base

titration-of-a-weak-acid-with-a-strong-base

Weak Acid Titration Curve and pH Stages

Weak acid titration with a strong base changes pH in clear stages. The acid in this example is acetic acid, and the base is sodium hydroxide. Each stage uses a different pH calculation method. At the start, the pH of the weak acid is found with its dissociation constant, Ka, and an ICE table. An ICE table tracks the initial, change, and equilibrium amounts of the acid. This step describes the acid before much base is added. As sodium hydroxide is added, a buffer forms. A buffer is a solution...

titration of a weak base with a strong acid

titration-of-a-weak-base-with-a-strong-acid

Ammonia Titration Curve with HCl

Ammonia titration with hydrochloric acid shows how a weak base behaves as acid is added. The curve is the mirror image of a weak acid titrated with a strong base. In this case, ammonia acts as the weak base, and hydrochloric acid acts as the strong acid. The starting pH of 50 mL of 0.1 M ammonia is found with an ICE table and the Kb value. That calculation gives an initial pH of 11.11. As hydrochloric acid is added, the pH begins to fall. After 25 mL of 0.1 M hydrochloric acid is added, the...

titration of a weak acid with a weak base

titration-of-a-weak-acid-with-a-weak-base

Finding the Endpoint in Weak Acid–Base Titration

Weak acid and weak base titration is used to follow how pH changes as base is added. In this kind of titration, both the acid and the base dissociate only partly. The titration curve shows a slow, gradual pH change instead of a sharp jump. A common example is the titration of acetic acid with ammonia. During the reaction, these two species form ammonium acetate and water. Because the pH changes so gradually, there is no simple indicator that shifts color sharply at the equivalence point. One...

solution composition during acid/base titrations

Acetic acid buffer changes during a weak acid–strong base titration. When acetic acid is titrated with sodium hydroxide, the reaction forms water and the conjugate base of the acid, sodium acetate. The mixture of acetic acid and sodium acetate acts as a buffer, which helps show how solution makeup shifts during the titration. The relative amounts of acetic acid and acetate ions are tracked with α values. Here, α0 represents the equilibrium concentration of acetic acid, and α1 represents the...

mixtures of acids

Finding pH in Acid Mixtures

Finding pH in acid mixtures depends on the acids present and their dissociation constants. When a solution contains two acids, the pH can be found by choosing the method that matches their relative strengths. The key idea is that the stronger acid often controls the hydronium ion level, which is the amount of H3O+ in solution. In a mixture of a strong acid and a weak acid, the strong acid dissociates completely. It becomes the main source of hydronium ions in the solution. The weak acid...

titration in nonaqueous solvents

Nonaqueous Solvents for Sharper Titration Endpoints

Nonaqueous solvents can make acid-base titrations easier to read by giving sharper endpoints. Most acid-base titrations are done in water, but water can compete with weak acids or bases for proton donation or acceptance. That competition can blur the titration curve and make the endpoint less clear. Water also changes the partial ionization of weak acids and bases. For example, water can accept a proton from acetic acid to form hydronium and acetate ions. The hydronium ion is a stronger acid...

titration of polyprotic base with a strong acid

titration-of-polyprotic-base-with-a-strong-acid

Carbonate Buffering in Acid Titration

The titration of sodium carbonate with hydrochloric acid shows how a polyprotic base reacts in stages. A polyprotic base can accept more than one proton, so its titration curve has two equivalence points. These points mark where one form has been fully changed into the next. At the first equivalence point, carbonate ions are completely converted to bicarbonate ions. The region before this point is the carbonate/bicarbonate buffer. In this buffer region, both forms are present in the solution. <br...

titration of polyprotic acids with a strong base

titration-of-polyprotic-acids-with-a-strong-base

Polyprotic Acid Titration Curve Features

Polyprotic acid titration curves show how acids with more than one ionizable proton react with a strong base. Each proton is released in a separate step. Each step has its own dissociation constant, or Ka, and each later Ka is weaker than the one before it. When a polyprotic acid such as sulfurous acid is titrated with sodium hydroxide, the base first neutralizes the first ionizable proton. This forms an intermediate species, such as hydrogen sulfite ions. The first part of the curve looks...

composition of polyprotic acid solutions as a function of ph

composition-of-polyprotic-acid-solutions-as-a-function-of-ph

Polyprotic Acid Titration Fractions at Each pH

Polyprotic acid titration shows how the main species in solution change as pH changes. In a compound of the form H2M, there are two ionizable protons. That means the titration with a base produces two equivalence points on the curve. As base is added, three species can be present in the solution: H2M, HM−, and M2−. Their amounts are shown as fractions called α0, α1, and α2. These alpha values track how much of each form is present at different stages of the titration. At the start of the...

buffers: overview

Buffers and pH Stability

Buffers help keep the pH of a solution stable when small amounts of acid or base are added. They are made from a weak acid and its conjugate base, or from a weak base and its conjugate acid. This balance lets the solution resist large pH changes until the buffer capacity is exceeded. One common buffer uses acetic acid and sodium acetate. Here, CH3COOH acts as the weak acid and CH3COONa provides its salt. Another buffer uses ammonia and ammonium chloride, written as NH3 and NH4Cl. These...

buffers: buffer capacity

Buffer Capacity and pH Resistance

Buffer capacity describes how well a buffer resists changes in pH. It is a quantitative measure, so it tells how much acid or base a one-liter buffer solution can take before its pH shifts by 1 unit. In the equation, beta is the buffer capacity, while Ca and Cb represent the moles of acid and base added. The term dpH means the change in pH. A graph of pH versus the moles of base added to a weak acid with a pKa of 5 shows how buffering works as more base is added. Taking the derivative of that...

leveling effect

How Solvents Limit Acid and Base Strength

The leveling effect explains how a solvent can limit acid and base strength in solution. In acid-base chemistry, the solvent sets a ceiling on how strong an acid or base can act. Stronger acids or bases may react with the solvent itself instead of with the intended compound. When a base is stronger than the conjugate base of the solvent, it deprotonates the solvent first. A conjugate base is the species left after an acid loses a proton. This reaction keeps going until the stronger base is...

key terms and concepts

See how acetic acid and sodium acetate change during a titration, including α values, the half-equivalence point, and the equivalence point.

Acetic Acid Buffer Changes in Titration | JoVE K12

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Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6.e

Scientific Laws and Theories

Scientific Laws

In science, a law is defined as a concise, verbal or mathematical, statement that summarizes a vast number of experimental observations. ...

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The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

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Elements: Chemical Symbols and Isotopes

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Use models to explain how the scientific understanding of atomic structure has evolved.

PS.Chm.1.1

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Nuclear Fission

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Nuclear Power

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Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

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Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

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The Energies of Atomic Orbitals

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PS.Chm.1.3

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Atomic Mass

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Molar Mass

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PS.Chm.2.1

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Ionic Radii

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Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

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	...

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Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

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Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

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Analyze the structure of atoms and isotopes.

Acetic Acid Buffer Changes in Titration

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