Name: water as a biological solvent
Uploaded: 2019-03-11T09:21:00.000Z
Duration: 1 min 12 s
Channel: JoVE

K12 Standards

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North Carolina K-12 Science Standard Course of Study

9-12

Earth and Environmental Science

Earth's Systems

ESS.EES.3.1

Solvents

Um solvente é qualquer substância que dissolva outras moléculas conhecidas como solutos, o que está sendo dissolvido. Por exemplo, a água abundante dentro do citoplasma da célula dissolve e entrega muitos nutrientes necessários para sobrevivência. A química celular é possível devido à polaridade da água.As cargas positivas parciais nos átomos de hidrogénio e uma leve carga negativa no oxigénio. Quando um composto iónico como o sal ou cloreto de sódio está presente, os iões individuais são mais atraídos para a água do que uns ao outros formando ligações de hidrogénio. Agora a água envolve as partículas, criando uma concha.Uma esfera de hidratação que mantém os solutos dispersos em uma mistura homogênea chamado de solução.

solventes

Um solvente é uma substância, na maioria das vezes um líquido, que pode dissolver outras substâncias. Aqui, a substância que está a ser dissolvida é chamada de soluto. Quando um solvente e um soluto se combinam, formam uma solução que, a nível molecular, é uma mistura homogénea tanto do solvente como do soluto. A água é um solvente biológico universal. A sua estrutura polar permite dissolver muitos outros compostos polares. A capacidade de dissolução da água é regida por um equilíbrio entre moléculas de água que se ligam umas às outras e que se ligam ao soluto.
 
 Uma solução saturada contém a quantidade máxima de soluto dissolvível. Por exemplo, o sal (NaCl) é facilmente dissolvido em água para criar água salgada, ou solução salina. Dissolve-se porque o sal dissocia-se nos seus respectivos iões de sódio (Na+) e cloreto (Cl-). A água é polar, então o seu átomo de oxigénio, sendo ligeiramente negativo, é atraído pelos iões de sódio positivos. Várias moléculas de água podem ligar-se a um único ião de sódio, criando uma esfera de hidratação. Da mesma forma, os átomos de hidrogénio da água são ligeiramente positivos e são atraídos pelos iões cloreto negativos, criando novamente uma esfera de hidratação em torno dos iões cloreto. Essas esferas de hidratação mantêm as partículas de soluto separadas e dispersas, criando uma solução.
 
 Uma solução saturada de água salgada (à temperatura ambiente) contém cerca de 26% de cloreto de sódio. Se mais sal for adicionado, o excesso não pode ser dissolvido na solução e torna-se um precipitado no fundo. O teor de sal do Grande Lago Salgado em Utah (EUA) varia de 5 a 27%. O Mar Morto, que faz fronteira com Israel, Jordânia e Cisjordânia, tem um teor de sal de ~34%. Isto é substancialmente maior do que o nível de saturação de sal na água. O excesso de sal precipita, criando formações extraordinárias de cristais de sal.
 
 A solubilidade de um soluto, ou capacidade de se dissolver na água, é crucial para as funções biológicas. Por exemplo, proteínas e aminoácidos devem ser dissolvidos para terem acesso às células. Da mesma forma, iões de sódio, cloreto, potássio e cálcio (entre outros) são necessários para a função celular. Proteínas, iões e outros nutrientes são dissolvidos no sangue, que é ~79% água. Os rins ajudam a manter os níveis adequados desses solutos dissolvidos no sangue, removendo-os ou adicionando-os durante a filtragem, um processo chamado de osmoregulação.

Solventes

Um solvente é uma substância, na maioria das vezes um líquido, que pode dissolver outras substâncias. Aqui, a substância que está sendo dissolvida é chamada de soluto. Quando um solvente ...

Education

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Biology

Biologia

Fundamentals

Fundamentos

Chemistry of Life

Química da Vida

KEY TERMS AND CONCEPTS

TERMOS-CHAVE E CONCEITOS

water as a biological solvent

Water acts as a biological solvent in many living systems. A solvent is a substance, usually a liquid, that dissolves another substance called a solute. When a solvent and a solute mix, they form a solution, which is a uniform mixture of both parts.

Water is called a universal biological solvent because its polar structure helps it dissolve many other polar compounds. Polarity means that one side of the molecule has a slight positive charge and the other side has a slight negative charge. Water’s ability to dissolve substances depends on a balance between water molecules sticking to each other and sticking to the solute.

A saturated solution holds the maximum amount of solute that can dissolve. Table salt, or sodium chloride (NaCl), dissolves readily in water to make salt water, also called saline. When salt dissolves, it breaks apart into sodium ions (Na+) and chloride ions (Cl-).

Water molecules then surround these ions. The oxygen atom in water is slightly negative, so it is attracted to sodium ions. The hydrogen atoms are slightly positive, so they are attracted to chloride ions. Several water molecules can cluster around each ion and form a sphere of hydration. These hydration shells keep the particles separated and dispersed, which allows a solution to form.

At room temperature, saturated salt water contains about 26% sodium chloride. If more salt is added, the extra salt cannot dissolve. It settles out as a precipitate at the bottom. The Great Salt Lake in Utah has a salt content that ranges from 5% to 27%. The Dead Sea, bordered by Israel, Jordan, and the West Bank, has about 34% salt. That is well above the saturation level of salt in water, so excess salt precipitates and forms striking salt crystals.

Solubility is important for biology because many molecules must stay dissolved to work in the body. Proteins and amino acids need to be dissolved to reach cells. Ions such as sodium, chloride, potassium, and calcium are also needed for cell function. Proteins, ions, and other nutrients stay dissolved in the blood. The kidneys help control the right levels of these dissolved solutes by removing or adding them during filtration. This process is called osmoregulation.

Water as a Biological Solvent

the periodic table and organismal elements

the-periodic-table-and-organismal-elements

Periodic Table Basics for Living Things

The periodic table helps explain which elements living things need and how those elements are related. Elements are the smallest units of matter that cannot be broken down further by chemical processes. There are 118 known elements, but not all occur naturally, and even fewer are essential for life. Living matter is made mostly of carbon, nitrogen, hydrogen, and oxygen. Together, these elements make up most of the human body and are also found in all life on Earth. Smaller amounts of calcium,...

atomic structure

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Atoms are the smallest units of elements, and they make up all matter. Each atom contains three subatomic particles: protons, neutrons, and electrons. These particles give an atom its mass and its charge. The idea that matter is made of tiny particles goes back to Democritus, a Greek philosopher around 450 B.C. He used the word atomos, which means “indivisible.” The idea was not accepted at the time, but it returned many centuries later. In the 19th century, John Dalton proposed an atomic...

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electron behavior

Electron Shells and Valence Electrons

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electron orbital model

Electron Orbitals and Energy Levels

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covalent bonds

Electronegativity and Covalent Bond Polarity

Covalent bonds form when two atoms share electrons to fill their valence shells. The way those shared electrons are pulled depends on electronegativity, which is an atom’s ability to attract electrons in a bond. When atoms have similar electronegativities, they form nonpolar covalent bonds. When their electronegativities differ, the bond is polar because the electrons are shared unevenly. The number of covalent bonds an atom can make depends on its valence electrons. Oxygen has six valence...

ionic bonds

Ionic Compounds and Electrolytes

Ionic compounds form when atoms gain or lose electrons to reach a more stable electron configuration. The charged particles that result are called ions. Ionic bonds are electrostatic attractions between oppositely charged ions. The most reactive elements include those with one valence electron, such as potassium, and those that need one more valence electron, such as chlorine. Ions that lose electrons become positive cations. Ions that gain electrons become negative anions. Cations and anions...

hydrogen bonds

Hydrogen Bonds in Water

Hydrogen bonds in water are weak attractions between atoms that are already part of other chemical bonds. One atom is electronegative, such as oxygen, and carries a partial negative charge. The other is a hydrogen atom that is bonded to another electronegative atom and has a partial positive charge. These attractions form because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom like oxygen or nitrogen. The electrons in that bond are shared unequally.

van der waals interactions

Intermolecular Forces in Polar Solutions

Intermolecular forces are the attractions and repulsions that act between atoms and molecules. These electrostatic forces come from particles with permanent, partial, or temporary charges. For neutral atoms and molecules, the main types are ion-dipole, dipole-dipole, and dispersion forces, which are together called van der Waals forces. Polar molecules have a partial positive end and a partial negative end. That separation of charge creates a dipole. In water, oxygen is more electronegative...

elements and compounds

Elements, Compounds, and Bonding

Elements and compounds are the two main kinds of pure substances. A pure substance contains only one kind of matter. An element contains only one type of atom. A compound contains two or more types of atoms joined by a chemical bond. Elements can be atomic or molecular, depending on their basic units. They are unique forms of matter with specific chemical and physical properties. Ordinary chemical reactions cannot break an element into a smaller substance. There are 118 elements, but only 98...

molecular shapes

Electron Geometry and Lone Pairs

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pH Scale in Everyday Solutions

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chemical reactions

Atoms, Bonds, and Chemical Reactions

Chemical reactions rearrange atoms to form new substances. In a reaction, the starting materials are called reactants, and the new substances are called products. The atoms stay the same type and number, but their bonds change, so the substances become different compounds. During a chemical reaction, bonds between atoms break and form again. This means the shared electrons are rearranged. Some reactions happen on their own, while others need an energy source such as heat or light. In biology,...

redox reactions

Electron Transfer in Redox

Redox reactions are chemical reactions that involve electron transfer between atoms or molecules. When one particle gains electrons, another must lose them at the same time. That is why oxidation and reduction always happen together. The two roles in a redox reaction are linked. The atom that is oxidized acts as the reducing agent, or reductant. The atom that is reduced acts as the oxidizing agent, or oxidant. A simple way to remember the ideas is OIL-RIG, which means oxidation is losing...

cohesion

Water Molecules and Surface Tension

Water molecules stick to each other through cohesion. Water is neutral overall, but it is a polar molecule. The oxygen atom in one water molecule has a partial negative charge, and it can bind with a hydrogen atom that has a partial positive charge in another water molecule. This forms a hydrogen bond. Each water molecule can form up to four hydrogen bonds with other water molecules, and these bonds give water its cohesive nature. Cohesion helps water form droplets on a surface. Water does not...

adhesion

Water Climbing by Adhesion

Water can climb or stick to surfaces because of adhesion, which is the attraction between different kinds of molecules. In water, this is easy to see on polar surfaces such as glass or cellulose in plants. The positive hydrogen side of water is more attracted to the negative oxygen in silica than to nearby water molecules. This attraction helps explain capillary action. If a narrow glass tube is placed in a beaker of water, water molecules attach to the tube’s surface and the water level rises.

states of water

Water Phase Changes and Ice Density

Water changes between solid, liquid, and gas states as temperature and molecular motion change. In this lesson, the focus is on how water freezes, melts, vaporizes, and returns to liquid or solid form. The balance between intermolecular forces, which pull molecules together, and kinetic energy, which pushes them apart, controls each state. Water freezes when intermolecular forces become stronger than kinetic energy. Unlike most substances, ice is less dense than liquid water. This happens...

specific heat

How Specific Heat Affects Temperature

Specific heat capacity describes how much energy a substance needs to rise by 1 degree Celsius for each gram. It is often written with calories, grams, and degrees Celsius, but it can also be shown in joules, kilograms, and Kelvin. For water, 1 gram needs 1 calorie to increase by 1°C, which is also written as 1 cal/g-°C or 4186 J/kg/K. Water has a high specific heat capacity, so it takes in a large amount of heat before its temperature changes much. It also gives off a lot of heat when it...

vaporization

Vaporization, Boiling, and Evaporation

Vaporization changes a liquid into vapor when temperature adds enough kinetic energy to overcome intermolecular forces. It is a surface phenomenon, which means it starts at the liquid’s surface. The energy needed to vaporize a set amount of liquid at a given pressure and constant temperature is called the heat of vaporization. Water shows this process clearly. When liquid water is vaporized, it becomes steam. One way this happens is boiling, which occurs when vapor bubbles form beneath the...

solvents

Water acts as a biological solvent in many living systems. A solvent is a substance, usually a liquid, that dissolves another substance called a solute. When a solvent and a solute mix, they form a solution, which is a uniform mixture of both parts. Water is called a universal biological solvent because its polar structure helps it dissolve many other polar compounds. Polarity means that one side of the molecule has a slight positive charge and the other side has a slight negative charge.

key terms and concepts

Explore how water dissolves salt, forms hydration shells, and reaches saturation. Learn why dissolved ions matter for cells, blood, and kidney regulation.

Water as a Biological Solvent | JoVE K12

JoVE Core series brings biology to life through over 300 concise and easy-to-understand animated video lessons that explain key concepts in biology, plus more than 150 scientist-in-action videos that show actual research experiments conducted in today’s laboratories.

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A coleção JoVE Core dá vida à biologia através de mais de 300 vídeos de animação concisos e fáceis de entender que explicam conceitos-chave de biologia, além de mais de 150 vídeos de Cientistas em ação que mostram experimentos reais em pesquisa realizados nos laboratórios atualmente.

Pennsylvania State Academic Standards

Earth and Space Science

3.3.9-12.K

Alabama Course of Study Science

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From Molecules to Organisms: Structures and Processes

9-12.B.1.4.b

Florida Department of Education

High School

Life Science

SC.912.L.18

SC.912.L.18.12

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South Carolina College and Career Ready Science Standards

Earth and Space Science (ESS)

Earth’s Systems

E-ESS2-5.

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Water as a Biological Solvent

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