Is Sulfuric acid H2SO4 strong or weak? Is H2SO4 also act as base? Is H2SO4 lewis acid or base? What is the Conjugate base of H2SO4. The concept of conjugate acid-base pair. A very strong acid always forms a weak conjugate base. A very strong base always forms a weak conjugate acid. A very weak acid always forms a strong conjugate base.
A very weak base always forms a strong conjugate acid. Subscribe to Blog via Email Enter your email address to subscribe to this blog and receive notifications of new posts by email.
Share it Strong or Weak -…. Leave a Comment Cancel Reply Your email address will not be published. Type here.. Quick Links. Content Links. Math Chemistry Career. Connect with us. Facebook Twitter Linkedin Pinterest. All rights Reserved. Loading Comments Email Name Website. Name of Molecule. Sulfuric acid. Chemical formula. Conjugate base. HSO 4 —. All of the reactant acid is ionized into product. Weak acids do not completely dissociate into their ions in water. There are many more weak acids than strong acids.
Most organic acids are weak acids. Here is a partial list, ordered from strongest to weakest. Weak acids incompletely ionize. An example reaction is the dissociation of ethanoic acid in water to produce hydroxonium cations and ethanoate anions:. Note the reaction arrow in the chemical equation points both directions. The reaction proceeds in both directions.
The back reaction is more favorable than the forward reaction, so ions readily change back to weak acid and water. You can use the acid equilibrium constant K a or pK a to determine whether an acid is strong or weak. Strong acids have high K a or small pK a values, weak acids have very small K a values or large pK a values. Be careful not to confuse the terms strong and weak with concentrated and dilute. A concentrated acid is one that contains a low amount of water.
In other words, the acid is concentrated. 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. This convey the message that the strong acids fully dissociate in water and that the equilibrium for the dissociation lies largely to the right.
Thus, the more hydronium ions you have in solution, the larger the acid dissociation constant K a and the stronger the acid. The equilibrium constant, K a is derived when we multiply the equilibrium constant, K c by the concentration of water. As you can see, a shorter arrow points to the right, meaning only few HF molecules dissociate to produce hydronium and fluoride ions.
However, these ions easily combine to get back HF and water molecules. As a result, the equilibrium lies largely to the left, which is why we drew the reverse arrow longer than the forward arrow.
To learn more about the general properties of acids, click here.
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