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The Amphoteric Nature of Water in Acid-Base Reactions

Exploring water's amphoteric behavior, this overview highlights its ability to act as both an acid and a base in various chemical contexts. Water's role extends to Lewis acid-base chemistry, ligand chemistry, organic reactions, redox processes, and electrolysis. Its physical properties have also been pivotal in defining temperature scales, showcasing its importance in scientific advancements and industrial applications.

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1

Brønsted-Lowry acid definition

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Substance that donates a proton (H+).

2

Brønsted-Lowry base definition

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Substance that accepts a proton (H+).

3

Water's reaction with HCl

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Acts as a base, accepting a proton to form H3O+.

4

In chemistry, a substance that can accept an electron pair is known as a ______ ______.

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Lewis acid

5

Water often serves as a ______ ______, especially when it forms complexes with metal ions.

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Lewis base

6

Water molecules can stabilize ______ ions (Fe3+) by surrounding them.

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ferric

7

According to HSAB theory, water is a hard ______ and a weak hard ______.

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base acid

8

Hard species, with which water typically reacts, are characterized by small size, high ______, and low ______.

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charge polarizability

9

Water as a monodentate ligand

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Water binds to a single coordination site on a metal ion.

10

Role of water in crystal hydrates

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Water molecules integrate into crystal lattices, affecting structure and stability.

11

Hydrogen bonding in metal aquo complexes

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Water's hydrogen bonds contribute to the stability and structure of metal complexes.

12

In organic chemistry, water can initiate ______ reactions by attacking ______, resulting in the conversion of ______ to ______.

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hydration carbocations alkenes alcohols

13

Water is crucial for ______ reactions, where it helps in breaking down chemical bonds, such as during the ______ of esters.

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hydrolysis saponification

14

The involvement of water in reactions like ______ and the cleavage of ______ like proteins and carbohydrates is vital for both synthetic chemistry and ______ metabolism.

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saponification biomolecules biological

15

Oxidation states of H and O in H2O

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Hydrogen +1, Oxygen -2.

16

Water reaction with alkali metals

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Produces H2 gas and hydroxide ions.

17

Electrolysis of water

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Electric current decomposes water into H2 and O2 gases.

18

The ______ scale is defined by the triple point of water, where all three phases of water are in equilibrium.

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Kelvin

19

______'s research led to the discovery of water's composition.

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Henry Cavendish

20

The first electrolysis of water was conducted by ______ and ______.

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William Nicholson Anthony Carlisle

21

Understanding water's properties is vital for its role in ______ processes and applications in various scientific fields.

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chemical

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The Amphoteric Nature of Water in Acid-Base Reactions

Water (H2O) is an amphoteric substance, meaning it can act as both an acid and a base within the Brønsted-Lowry acid-base framework. An acid is defined as a substance that can donate a proton (H+), while a base is one that can accept a proton. When water encounters a stronger acid, such as hydrochloric acid (HCl), it acts as a Brønsted-Lowry base, accepting a proton to form the hydronium ion (H3O+). Conversely, in the presence of a stronger base like ammonia (NH3), water acts as a Brønsted-Lowry acid, donating a proton to form the hydroxide ion (OH-). This dual functionality allows water to play a central role in maintaining the acid-base balance in biological systems and in the environment.
Glass beaker with transparent liquid and drops falling from pipette, gloved hands in laboratory, blurred background with laboratory glassware.

Water as a Lewis Acid and Base in Chemical Reactions

Water also exhibits Lewis acid and base behavior, where a Lewis acid is a substance that can accept an electron pair, and a Lewis base can donate an electron pair. Water commonly acts as a Lewis base, forming coordination complexes with metal ions by donating its electron pairs. For example, water molecules can surround and stabilize ferric ions (Fe3+) in solution. According to the Hard and Soft Acids and Bases (HSAB) theory, water is classified as a hard base and a weak hard acid, typically reacting with other hard species, which are generally characterized by small size, high charge, and low polarizability.

Water's Role in Ligand Chemistry and Complex Formation

In coordination chemistry, water is a versatile ligand that can bind to metal ions, forming metal aquo complexes. These complexes are important in both biological systems and industrial applications. Water molecules can act as monodentate ligands, attaching to a single coordination site on the metal ion, or as part of the crystal lattice in solid hydrates. For instance, in the compound ferrous sulfate heptahydrate (FeSO4·7H2O), water molecules are both coordinated to the iron and incorporated into the crystal structure. Water's ability to form hydrogen bonds also influences the stability and structure of these complexes.

The Role of Water in Organic Chemistry and Hydrolysis

Water's role in organic chemistry is multifaceted. As a nucleophile, water can attack carbocations, leading to hydration reactions that transform alkenes into alcohols. Water is also essential in hydrolysis reactions, where it breaks chemical bonds, such as in the saponification of esters or the breakdown of biomolecules like proteins and carbohydrates. Furthermore, water can act as a leaving group in nucleophilic substitution and elimination reactions, the latter being known as dehydration reactions. These reactions are fundamental to synthetic chemistry and biological metabolism, underscoring water's critical role in organic transformations.

Water's Involvement in Redox Reactions and Electrolysis

Water participates in redox reactions, where it can act as both a reducing agent and an oxidizing agent. In its molecular form, water has hydrogen at an oxidation state of +1 and oxygen at −2. It can react with metals and hydrides, as seen when alkali metals are dropped into water, producing hydrogen gas and hydroxide ions. Water can also be electrolyzed, a process that uses an electric current to decompose water into hydrogen and oxygen gases. This process is essential for producing hydrogen fuel and for studying electrochemical cells.

Historical Significance of Water in Defining Temperature Scales

Water's physical properties have been instrumental in the development of temperature scales. The Celsius and Fahrenheit scales were originally based on the freezing and boiling points of water. The Kelvin scale uses the triple point of water as a fundamental reference, where water's solid, liquid, and gas phases coexist in equilibrium. The study of water's properties has been central to the advancement of chemistry, with milestones such as Henry Cavendish's discovery of its composition and the first electrolysis performed by William Nicholson and Anthony Carlisle. These contributions have been crucial in understanding water's role in chemical processes and its applications across various scientific disciplines.