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## Is H2CO3 a strong or weak acid? Explain. | Study.com

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• Match the search results: Acids can be defined in a number of ways based on different properties that these compounds exhibit. They can be characterized by their ability to dissociate in water to form hydronium ions. The nature by which acids dissociate in water can be used to classify them as either a strong or weak acid.

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## List of Strong and Weak Acids – ThoughtCo

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• Summary: Articles about List of Strong and Weak Acids – ThoughtCo Strong Acids · HCl – hydrochloric acid · HNO3 – nitric acid · H2SO4 – sulfuric acid (HSO4- is a weak acid) · HBr – hydrobromic acid · HI – hydroiodic …

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Strong and weak acids are important to know both for chemistry class and for use in the lab. There are very few strong acids, so one of the easiest ways to tell strong and weak acids apart is to memorize the short list of strong ones. Any other acid is considered a weak acid.

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## Table of Acid and Base Strength

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• Summary: Articles about Table of Acid and Base Strength Base. Name. Formula. Formula. Name. Large. Perchloric acid. HClO4. ClO4 -. Perchlorate ion … Carbonic acid. CO3 2-. HCO3 -. Hydrogen carbonate ion.

• Match the search results: ClO-

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## Is carbonic acid a weak acid? – Movie Cultists

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• Summary: Articles about Is carbonic acid a weak acid? – Movie Cultists No, carbonic acid is not a strong acid. H2CO3 is a weak acid that dissociates into a proton (H+ cation) and a bicarbonate ion (HCO3- anion). This compound.

• Match the search results: No, carbonic acid is not a strong acid. H2CO3 is a weak acid that dissociates into a proton (H+ cation) and a bicarbonate ion (HCO3- anion). This compound only partly dissociates in aqueous solutions. … These are the reasons why carbonic acid is classified as a weak acid rather than a strong acid.

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## 21.12: Strong and Weak Acids and Acid Ionization Constant …

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• Summary: Articles about 21.12: Strong and Weak Acids and Acid Ionization Constant … Acids are classified as either strong or weak, based on their ionization in water … Acetic acid is stronger than carbonic acid, and so on.

• Match the search results: Weak acids, like strong acids, ionize to yield the $$\ce{H^+}$$ ion and a conjugate base. Because $$\ce{HCl}$$ is a strong acid, its conjugate base $$\left( \ce{Cl^-} \right)$$ is extremely weak. The chloride ion is incapable of accepting the $$\ce{H^+}$$ ion and becoming $$\ce{HCl}$$ again. In gene…

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## carbonic acid is a mineral acid then why we considered it …

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• Summary: Articles about carbonic acid is a mineral acid then why we considered it … When we talk about acids, It is a general case that organic acids are weak and mineral acids are strong. But it is not true for all case.

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## which is stronger acid dilhcl or conc carbonic acid h2co3 also …

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• Summary: Articles about which is stronger acid dilhcl or conc carbonic acid h2co3 also … Strong and weak acid refer to the degrees of dissociation. HCl acid ionises completely to H+ and Cl- ions (that is, about 100 out of 100 …

• Match the search results: Which is stronger acid- dil.HCl or conc. carbonic acid (H2CO3)? Also give reasons for the same.

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## Classifying Electrolytes – St. Olaf College

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• Summary: Articles about Classifying Electrolytes – St. Olaf College Strong Electrolytes · salts, NaCl, KBr, MgCl2, and many, many more ; Weak Electrolytes ; Weak Electrolytes. weak acids, HF, HC2H3O2 (acetic acid), H2CO3 (carbonic …

• Match the search results: Strong electrolytes fall into three categories: strong acids,
strong bases, and salts.
(Salts are sometimes also called ionic compounds, but really strong
bases are ionic compounds as well.) The weak electrolytes include weak acids and weak bases.

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## carbonic acid | Formula, Uses, & Facts – Encyclopedia Britannica

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• Summary: Articles about carbonic acid | Formula, Uses, & Facts – Encyclopedia Britannica carbonic acid, (H2CO3), a compound of the elements hydrogen, carbon, and oxygen. It is formed in small amounts when its anhydride, carbon dioxide (CO2), …

• Match the search results: Carbonic acid is important in the transport of carbon dioxide in the blood. Carbon dioxide enters blood in the tissues because its local partial pressure is greater than its partial pressure in blood flowing through the tissues. As carbon dioxide enters the blood, it combines with water to form&nbsp…

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## Acid strength – Wikipedia

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• Summary: Articles about Acid strength – Wikipedia For example, hydrogen chloride is a strong acid in aqueous solution, but is a weak acid when dissolved in glacial acetic acid. Contents. 1 …

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p

K

a

{\displaystyle \mathrm {p} K_{{\ce {a}}}}

value measures the tendency of an acidic solute to transfer a proton to a standard solve…

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## Carbonic acid – Wikipedia

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• Summary: Articles about Carbonic acid – Wikipedia Equilibrium constant values. Bjerrum plot for carbonate speciation in seawater (ionic strength 0.7 mol dm−3).

• Match the search results: The fact that the carbonic acid may form by irradiating a solid H2O + CO2 mixture or even by proton-implantation of dry ice alone[16] has given rise to suggestions that H2CO3 might be found in outer space or on Mars, where frozen ices of H2O and CO2 are found, as well as cosmic rays.[13&…

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## Q & A: Acids and Other Materials | Department of Physics

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• Summary: Articles about Q & A: Acids and Other Materials | Department of Physics OH- and H+ react to form water. Carbonates (CO3–) are actually weak bases. Carbonic Acid (H2CO3) breaks apart to form H+ and HCO3- or to make …

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## Why HNO2 stronger acid than H2CO3 – Laurence Lavelle

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• Summary: Articles about Why HNO2 stronger acid than H2CO3 – Laurence Lavelle Would HNO2 and H2CO3 act like strong acids when each is dissolved in CH3COOH … the conjugate base CH3COO-, so H2CO3 would act like a weak acid in CH3COOH.

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## Acid and Base Chart — Table of Acids & Bases – Sigma-Aldrich

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• Summary: Articles about Acid and Base Chart — Table of Acids & Bases – Sigma-Aldrich Xem thêm 29 hàng

• Match the search results: Use this acids and bases chart to find the relative strength of the most common acids and bases. This acid-base chart includes the Ka value for reference along with the chemical’s formula and the acid’s conjugate base. The acid and base chart is a reference table designed to make determining the str…

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## Strong and Weak Acids – Chemistry – Cliffs Notes

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• Summary: Articles about Strong and Weak Acids – Chemistry – Cliffs Notes The sodium carbonate is a strong electrolyte, and each formula unit dissociates … assume that x is so much less than 1 (carbonic acid is weak and only …

• Match the search results: where K a is the acid ionization constant (or merely acid constant). Different acids have different K a values—the higher the value, the greater the degree of ionization of the acid in solution. Strong acids, therefore, have larger K a than do weak acids.

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## Acid-Base Reactions | Boundless Chemistry – Lumen …

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• Summary: Articles about Acid-Base Reactions | Boundless Chemistry – Lumen … Similarly, excess carbonic acid can be converted into carbon dioxide gas and … Titration of a weak acid by a strong base: The pH of a weak acid solution …

• Match the search results: Acid-base titration: The solution in the flask contains an unknown number of equivalents of base (or acid). The burette is calibrated to show volume to the nearest 0.001 cm3. It is filled with a solution of strong acid (or base) of known concentration. Small increments are added from the burette unt…

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## Metabolic Acidosis: Practice Essentials, Background, Etiology

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• Summary: Articles about Metabolic Acidosis: Practice Essentials, Background, Etiology Hydrochloric acid (HCl) is considered a strong acid because it is present … whereas carbonic acid (H2 CO3) is a weak acid because it is …

• Match the search results: Free fatty acids released from adipose tissue have 2 principal fates. In the major pathway, triglycerides are synthesized in the cytosol of the liver. In the less common pathway, fatty acids enter mitochondria and are metabolized to ketoacids (acetoacetic acid and beta-hydroxybutyric acid) by the be…

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Multi-read content h2co3 strong or weak acid

Carbonic acid is a diprotic acid with the formula H2CO3. It is a hydride of carbon dioxide and decomposes at temperatures above -80°C.

As a diprotic, it is responsible for two salts, viz. Hydrogen carbonate salts (HCO3-) and carbonate salts (CO3-2).

Many students wonder about the acidity of H2CO3 (carbonic acid), is it a strong acid or a weak acid.

So, in this post, we will examine the acidity of H2CO3 and tell you all the basic principles.

So is carbonic acid a strong acid?No, H2CO3 is not a strong acid as it does not fully dissociate in aqueous solution. The carbonic acid molecule is missing two hydrogen atoms, meaning it is a diprotic acid and therefore has two acid dissociation constants, Ka. The value of the acid dissociation constant reflects the strength of the acid. A higher Ka value indicates higher acidity.

The reaction equations along with their Ka values ​​are given below:

H2CO3 (aqueous) <=====> HCO3- H Ka1 = 4.3 X 10−7 mol/L; pKa1 = 6.36 at 25°C

HCO3- <=====> CO3-2 H Ka2 = 4.8 X 10−11 mol/L; pKa2 = 10.25 at 25°C

From the above equations, it can be seen that the value of the acid dissociation constant is very low, while the logarithmic constant of carbonic acid is higher than that of a strong acid.

For strong acids, the value of Ka is expected to become infinity, while the value of pKa should be less than 2.

Therefore, carbonic acid is not a strong acid. The pH of 0.1 M carbonic acid is 3.68.

contents

show

Why is carbonic acid a weak acid?

Which substance is more acidic than H2CO3 or CH3COOH?

pH of carbonic acid

what is acid

Conjugated acid-base pairs

How is carbonic acid formed?

Is carbonic acid an organic or an inorganic acid?

Properties of carbonic acid

use of carbon dioxide

inference

Why is carbonic acid a weak acid?

As discussed in the previous section, carbonic acid first ionizes to bicarbonate and proton when dissolved in an aqueous solution.

This means that the bicarbonate ion acts as a conjugate base for the carbonic acid in this reaction.

Likewise,It is well known that the bicarbonate ion is a strong conjugate base and therefore tends to remain bound to its proton, which is why the acid molecules only partially ionize in aqueous solution.

Which substance is more acidic than H2CO3 or CH3COOH?

Both carbonic acid and acetic acid are weak acids and do not ionize completely in aqueous solution.

However,The Ka value of carbonic acid is 4.3 x 10-7 mol/L, while that of acetic acid is 1.8 x 10-5 mol/L.

Likewise,the pKa of carbonic acid is 6.36 for the first dissociation equation, while that of acetic acid is 4.76.

These values ​​show that acetic acid is stronger than carbonic acid.

Now let’s try to figure out why acetic acid is stronger than carbonic acid. Start by writing dissociation equations for both acids:

for carbonic acid,H2CO3 (aqueous) <====> HCO3- H

For acetic acid,CH3COOH (aqueous) <====> CH3COO-H

According to the equations above, the conjugate base of carbonic acid is the bicarbonate ion, while for acetic acid, the acetate ion acts as the conjugate base.

Check out the detailed article I wroteAcetic acid a strong acid.

We can leave the second dissociation equation of carbonic acid for the time being, since the strength is only measured via the first proton released.

Now we need to analyze the strength of conjugate bases as stronger conjugate base means weaker acid and vice versa.

The acetate ion is a stronger conjugate base than the bicarbonate ion due to the resonance effect of the carboxyl ion.

Another factor is the instability of the carbonic acid, which is mostly broken down into water and carbon dioxide molecules, leaving a very small amount of carbonic acid in solution, so the acidity automatically decreases.

If you also want to know the chemical structure of carbonic acid. Read the article aboveLewis structure of carbonic acid.

pH of carbonic acid

The pH scale is a scale used to express the acidity or basicity of a substance in an aqueous solution.

Values ​​on the pH scale range from 1 to 14. All acids have a pH below 7 while all bases have a pH above 7.

Neutral solutions like pure water have a pH of 7.

Now, when calculating the pH value of carbonic acid, we have to bear in mind that it is a polyprotic acid, i.e. it dissociates several times in a solution and thus releases different ions when it dissolves.

Therefore, the steps to calculate the pH of 0.1 M carbonic acid are different from other simple acids.

First, let’s start with the first dissociation equation, which leads to the release of bicarbonate ions along with protons.

The chemical equation is given below:

H2CO3 (aqueous) <====> HCO3- H

Now calculate the hydrogen ion concentration of this equation, knowing that the Ka1 value is 4.3 x 10−7 mol/L.

The equation is written below:

Ka = ([HCO3-][H]) / H2CO3

We calculate the pH for a 0.1 M solution, so the initial concentration of H2CO3 is assumed to be 0.1. Assuming that x protons and x bicarbonate ions are eventually formed, the above equation can be written as:

4.3 X 10^−7 = x^2/1-x

x = 2.1 x 10^-4

Looking now at the second dissociation equation, the value of Ka2 is 4.8 x 10−11 mol/L. The equation is written as follows:

HCO3- <====> CO3-2 H

Once again,Ka2 = ([CO3-2] [H]) / [HCO3-]

According to the calculation in the equation above, the concentration of HCO3- is 2.1 x 10-4. Now insert the values ​​into the above equation, assuming that y protons and y CO3-2 ions are formed,

4.8 X 10^−11 = (2.1 X 10^-4y)y / 2.1 X 10^-4 – y

y = 4.8 X 10^−11

In the case of carbonic acid, the effect of the second proton release is completely negligible and the pH is derived from the first equation, i.e. H. the value of Ka1.

So,pH = -log [H]

= -log[2.1 X 10^-4]

= 3.68

what is acid

A substance that readily donates a proton when dissolved in water is called an acid. These are acidic substances, pH below 7, that turn red litmus blue to red and form salts with alkali.

Acids are divided into strong acids and weak acids according to their degree of dissociation in aqueous solution.

Acids that ionize completely are called strong acids, and those that don’t completely dissociate in aqueous solution are called weak acids.

Three theories are said to have correctly determined the properties of acids.

Bronsted-LowryThe theory defines an acid as a proton donor in aqueous solution or a proton donor.

Arrhenius theorysay that acids in water produce hydrogen ions.

Lewis theorydefines an acid as an electron acceptor.

When a substance is said to have any or all of the properties listed above, it can be said to be an acid.

Conjugated acid-base pairs

According to the Bronsted-Lowry theory of acids and bases, a substance that donates its proton is an acid, while a proton acceptor is a base.

For example, in the case of carbonic acid, the dissociation equation is written as follows:

H2CO3 H2O <====> HCO3- (conjugate base) H3O (conjugate acid)

H2CO3 releases a proton and is therefore an acid, while water accepts a proton and thus acts as a base in this reaction.

However, the theory adds that due to this loss and gain of protons, a conjugate base and conjugate acid are formed, with the acid and the base participating respectively as reactants.

In the example aboveHCO3- is the conjugate radical of carbonic acid while H3O is the conjugate acid of water molecule.

A strong conjugate base shows a weak acid and vice versa. Likewise, a strong conjugate acid shows a weak base and vice versa. Therefore, they help in estimating the strength of acids and bases.

How is carbonic acid formed?

Carbonic acid is made by dissolving carbon dioxide in water.

The carbon dioxide molecule acts as the anhydride of carbonic acid and easily takes on a water molecule to form carbonic acid.

The reaction equation is written as follows:

CO2 H2O <====> H2CO3

It is unstable and weak, so it easily dissociates into bicarbonate and hydrogen ions.

Is carbonic acid an organic or an inorganic acid?

Compounds that contain carbon and hydrogen atoms are called organic compounds. There is a special branch of chemistry that deals with the properties and reactivity of these compounds.

Although carbonic acid contains both carbon and hydrogen, it is still not considered an organic compound.

Similar to carbon dioxide, carbonic acid is also an inorganic or mineral acid.

The reason for this behavior can be understood by looking at the structure of the carbonic acid molecule, which consists of one carbon-oxygen double bond and two carbon-oxygen single bonds.

Properties of carbonic acid

Carbonic acid is an unstable and weak base or diprotic acid. It also occurs naturally in the human body.

Some important properties of carbonic acid are listed in the table below:

 chemical name carbonic acid Appear Light gray white chemical formula H2CO3 molecular mass 62.024 g/mol degree of melting 210 degrees boiling point -78℃ density 1.668 g/cm3 Odor Odorless Ca1 4.3 x 10-7 mol/l pKa1 6.35 toxicity non-toxic

use of carbon dioxide

Some of the important uses of carbonic acid are listed below:

• It is used to make salt.

• In our body, the conjugate base of carbonic acid and bicarbonate is used to transport CO2 outside through respiratory exchange.

• Also helps to protonate nitrogenous bases in serum.

• It also acts as a buffer in our body and is broken down into carbon dioxide by carbonic anhydrase activity.

• It is used to prepare carbonated drinks, carbonated wine and carbonated water.

• It is also an ingredient in mouthwash and vaginal douches.

• Carbonic acid is used as a contact lens cleaner.

• It is also used in the cosmetics and food industries.

• It helps hydrolyze starch.

inference

Carbonic acid is a weak acid because it does not completely dissociate in aqueous solution.

A high value of the acid dissociation constant and a lower value of the logarithmic constant for carbonic acid also indicate that it is a weak acid.

Under carbonic acid and acetic acid, H2CO3 is weaker than its conjugate base due to the higher stability of the conjugate base. In addition, it tends to separate its constituents, i. H. Water and carbon dioxide, to reformulate.

The conjugate radical of carbonic acid is HCO3-.

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Video tutorials about h2co3 strong or weak acid

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Learn the basics about strong and weak acids, and how they differ.

Strong acids are often used in School Science labs for experimentation but they have important uses in industry and the everyday world.

Sulphuric acid for example is found in car batteries but industry uses 200 million tonnes annually for the chemical industry. Hydrochloric acid found in your stomach and nitric acid are also examples of strong acids.

Acids react with water to produce hydrogen ions, or more strictly hydroxonium ions: Strong acids dissociate fully into their ions.

Most acids are weak, and remain largely as molecules in solution. Acids can be identified by using full-range indicator from 0 to 7 on the pH scale. pH is a measure of the concentration of hydrogen ions.

If you dissolve 1 mole of a strong acid, like HCl in water to make 1litre of solution it dissociates completely into ions so you also get 1 mole per litre of H+ ions, and a pH of 0. To get a solution of pH 4 you have to dilute this with 10,000 times its volume of water. We still have a STRONG acid but it is VERY dilute!

However, if you dissolve 1 mole of a weak acid, like ethanoic acid (also called acetic acid) to make a litre of solution it remains mostly as undissociated molecules.

If an acid is only 0.01% dissociated – so only one molecule in 10,000 are split into ions. Although the concentration of acid is 1 Mole, the concentration of hydrogen ions is only 0.0001 moles per litre, that is 10 to the power negative 4, making the pH 4. So here is an example of a fairly concentrated acid which is weak.

So acids cab be both concentrated and fully dissociated so STRONG, concentrated but not fully dissociated so WEAK, dilute but STRONG because fully dissociated or finally dilute and weak.

A weak acid can be concentrated and a strong acid can be dilute. Most acids are commonly occurring organic acids such as you find in lemons or vinegar – which are all WEAK so remain mostly as molecules and often have a smell. There are only a few STRONG acids, mostly non-metal oxides dissolved in water like sulfuric and nitric acids, but there is also Hydrochloric acid – found in your stomach to aid digestion!

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Learn how to classify an acid as strong or weak, write ionization and dissociation reactions, the list of strong acids, and modeling of the strong vs weak acids.

#StrongAcid #WeakAcid #SchmidtChemist

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8.3.1 Distinguish between strong and weak acids and bases in terms of the extent of dissociation, reaction with water and electrical conductivity.

8.3.2 State whether a given acid or base is strong or weak.

8.3.3 Distinguish between strong and weak acids and bases, and determine the relative strengths of acids and bases, using experimental data.

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