Name: ammonia titration curve with hcl
Uploaded: 2025-05-22T09:06:07.000Z
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K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.6.3

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

Titration of a Weak Base with a Strong Acid

منحنى المعايرة بالتحليل الحجمي للقاعدة الضعيفة مقابل منحنى المعايرة بالتحليل الحجمي الحمضي القوي الضعيف.
تشكل الأمونيا المائية أيونات الأمونيوم والهيدروكسيد. كما تم حسابه من جدول ICE وتعبير KB ، فإن الرقم الهيدروجيني الأولي البالغ 50 مل من محلول الأمونيا 0.1 M أساسي مع 11.11 درجة حموضة.
عند إضافة 25 مل من 0.1 M حمض الهيدروكلوريك إلى محلول الأمونيا ، يحتوي المخزن المؤقت الناتج على كمية متساوية من أيونات الأمونيا والأمونيوم. يتم حساب الرقم الهيدروجيني للمخزن المؤقت عن طريق استبدال هذه القيم في معادلة هندرسون-هاسلبالش. في هذه المرحلة ، الأس الهيدروجيني يساوي pKa. 
عند نقطة التكافؤ ، يقوم 50 مل من حمض الهيدروكلوريك المضاف بتحويل كل الأمونيا لتكوين أيونات الأمونيوم. إنها تحلل مائي لإنتاج أيونات الهيدرونيوم مما يجعل المحلول حمضيا بدرجة حموضة 5.28.
بعد نقطة التكافؤ ، حيث تسود أنواع أيون الهيدرونيوم ، ينخفض الرقم الهيدروجيني إلى 1.6.
للكشف عن نقطة النهاية ، يمكن استخدام مؤشر الميثيل الأحمر.

لم يتم الإعلان عن أي تضارب في المصالح.

معايرة القاعدة الضعيفة بحمض قوي

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منحنى المعايرة لقاعدة ضعيفة مثل الأمونيا مع حمض قوي مثل حمض الهيدروكلوريك هو صورة طبق الأصل لمنحنى المعايرة لحمض ضعيف مع قاعدة قوية.

باستخدام جدول ICE واستبدال قيمة Kb، نحسب الرقم الهيدروجيني الأولي لـ 50 مل من الأمونيا 0.1 مولار ليكون 11.11. تؤدي إضافة 25 مل من حمض الهيدروكلوريك 0.1 م إلى محلول الأمونيا هذا إلى إنشاء مخزن مؤقت بتركيز متساوٍ من الأمونيا وأيونات الأمونيوم. يمكن حساب الرقم الهيدروجيني لهذا المخزن المؤقت عن طريق استبدال هذه القيم في معادلة هندرسون-هاسلبالش، والتي توضح أنه عند هذه النقطة، والمعروفة أيضًا بنقطة نصف التكافؤ، يكون الرقم الهيدروجيني يساوي pKa. إن الاستمرار في المعايرة حتى نقطة التكافؤ يعني أنه سيتم إضافة إجمالي 50 مل من حمض الهيدروكلوريك 0.1 مولار، مما يحول جميع جزيئات الأمونيا إلى أيونات الأمونيوم. عند هذه النقطة، تخضع أيونات الأمونيوم للتحلل المائي لتوليد أيونات الهيدرونيوم، مما يجعل المحلول حمضيًا، ويظهر حساب جدول ICE أن الرقم الهيدروجيني هو 5.28. بعد نقطة التكافؤ، عندما تهيمن أيونات الهيدرونيوم على المحلول، ينخفض ​​الرقم الهيدروجيني إلى 1.6. يتم الكشف عن نقطة نهاية المعايرة باستخدام مؤشر الميثيل الأحمر، الذي يُظهر تغيرًا في اللون في نطاق الرقم الهيدروجيني المطلوب.
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منحنى المعايرة بالتحليل الحجمي للقاعدة الضعيفة مقابل منحنى المعايرة بالتحليل الحجمي الحمضي القوي الضعيف.
تشكل الأمونيا المائية الأمونيوم والهيدروكسيد ...

Education

JoVE Core

Analytical Chemistry

الكيمياء التحليلية

Unit 1

الوحدة الأولى

Acid–Base Titration

معايرة الحمض والقاعدة

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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 solution becomes a buffer. A buffer is a mixture that resists pH change. At this half-equivalence point, ammonia and ammonium ions are present at equal concentration. The pH can then be found with the Henderson-Hasselbalch equation, and the pH equals pKa.

At the equivalence point, a total of 50 mL of 0.1 M hydrochloric acid has been added. All of the ammonia has been converted to ammonium ions. The ammonium ions hydrolyze to form hydronium ions, so the solution becomes acidic. An ICE table calculation gives a pH of 5.28.

Beyond the equivalence point, hydronium ions dominate the solution. The pH drops further to 1.6. The endpoint is detected with methyl red, an indicator that changes color in the needed pH range.

Ammonia Titration Curve with HCl

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

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

solution-composition-during-acidbase-titrations

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...

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

Follow the titration curve of ammonia with hydrochloric acid, from the initial pH to the buffer region, equivalence point, and methyl red endpoint.

Ammonia Titration Curve with HCl | JoVE K12

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Alabama Course of Study Science

Matter and Its Interactions

9-12.C.1.6.e

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New York State Science Learning Standards

High School

Physical Science

HS. Chemical Reactions

HS-PS1-11.

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Scientific Laws

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Radioactive Decay and Radiometric Dating

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

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The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

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Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

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PS.Chm.2.1

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Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

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Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

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

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

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Trends in Lattice Energy: Ion Size and Charge

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Covalent Bonding and Lewis Structures

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Electronegativity

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Electronegativity values of ...

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Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

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To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

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Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

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

PS.Chm.3.1

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Molecular Comparison of Gases, Liquids, and Solids

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Intermolecular vs Intramolecular Forces

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Intermolecular Forces

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Surface Tension, Capillary Action, and Viscosity

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PS.Chm.3.2

Analyze the structure of atoms and isotopes.

Ammonia Titration Curve with HCl

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