OTP has been re-sent. OTP has been sent to your mobile. Finding exercises tough? Install the app to watch our videos and get a crystal clear understanding of concepts Install Now. Rohit Kumar Nov 20, Give a reason why sulphuric acid is considered a strong acid while acetic a weak acid? Arun prakash Puthanviddu. Recommend 0 Comment 0. A dilute acid is an acidic solution that contains a lot of solvent. If you have 12 M acetic acid, it's concentrated, yet still a weak acid.
No matter how much water you remove, that will be true. On the flip side, a 0. You can drink diluted acetic acid the acid found in vinegar , yet drinking the same concentration of sulfuric acid would give you a chemical burn.
The reason is that sulfuric acid is highly corrosive, while acetic acid is not as active. While acids tend to be corrosive, the strongest superacids carboranes are actually not corrosive and could be held in your hand. Hydrofluoric acid, while a weak acid, would pass through your hand and attack your bones.
Actively scan device characteristics for identification. Use precise geolocation data. Select personalised content. Create a personalised content profile. Measure ad performance. Select basic ads. Create a personalised ads profile. Select personalised ads. Apply market research to generate audience insights. Due to the complete dissociation of strong acids in aqueous solution, the concentration of hydronium ions in the water is equal to the total concentration ionized and un-ionized of the acid introduced to solution:.
Strong acids can accelerate the rate of certain reactions. For instance, strong acids can accelerate the synthesis and hydrolysis of carbonyl compounds.
With carbonyl compounds such as esters, synthesis and hydrolysis go through a tetrahedral transition state, where the central carbon has an oxygen, an alcohol group, and the original alkyl group. Strong acids protonate the carbonyl, which makes the oxygen positively charged so that it can easily receive the double-bond electrons when the alcohol attacks the carbonyl carbon; this enables ester synthesis and hydrolysis. Weak acids have very small values for K a and therefore higher values for pK a compared to strong acids, which have very large K a values and slightly negative pK a values.
The majority of acids are weak. On average, only about 1 percent of a weak acid solution dissociates in water in a 0.
Vinegars : All vinegars contain acetic acid, a common weak acid. Weak acids ionize in a water solution only to a very moderate extent. The generalized dissociation reaction is given by:.
The strength of a weak acid is represented as either an equilibrium constant or a percent dissociation. The equilibrium concentrations of reactants and products are related by the acid dissociation constant expression, K a :.
The K a of weak acids varies between 1. Acids with a K a less than 1. If acids are polyprotic, each proton will have a unique K a. To further understand Why H 2 SO 4 is a strong acid? And this reaction is irreversible means, it strongly favors the right side.
In the second reaction, HSO 4 — as a weak acid that also partially dissociate and release the one proton and forms SO 4 The double arrow in the second reaction shows that both backward and forward reactions will occur at equilibrium. Hence, this is why H 2 SO 4 is a strong acid in nature as it fully dissociates into ions in one shot.
Also check:- How to know if acid or base is strong or weak? Yes, sometimes H 2 SO 4 can also act as a base if it reacts with superacids. A compound is said to be base when it accepts the proton or donates the OH — in an aqueous solution. So, when sulfuric acid reacts with superacids then it will accept the proton from super acid, hence, act as a base.
Also check:- How to tell if something is acid or base or salt? Lewis acid is a compound that accepts the pair of electrons and lewis base which donates the pair of electrons to other compounds. So, Is H 2 SO 4 lewis acid or base?
To be a Lewis acid, the atom needs an empty orbital in its valence shell. Note: Lewis acid is a superset of Bronsted-Lowry acids that means every compound that falls into the category of Bronsted-Lowry acid is Lewis acids.
The acid will have both of these characteristics. Conjugate acid is always formed by base and conjugate base is formed by acid. So, H 2 SO 4 is a very strong acid that makes a weak conjugate base according to the concept of conjugate acid-base pair. It is because greater oxidation numbers attract more electrons towards itself, therefore, expanding the acidity which helps in stabilizing the conjugate base of the compound.
Clearly, sulfuric acid has high oxidation number than sulfurous acid. So, H 2 SO 4 central atom pulls out more electron density from the acidic proton.
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