why do strong acids (that have one sided arrow bcz of the complete ionization) have equilibrium if there is no reverse reaction, since equilibrium is rate of forward reaction = to rate of reverse reaction? please expalin in detail and thank you !!!
For strong acids and bases, the reaction more or less goes to completion (the equilibrium position lies very far to the right). So much so that the reverse reaction can be said to not actually occur.
@@MSJChem Thank you, but when you say it lies so far to the right what do you mean? What is the difference when we say equilibrium on the right and equilibrium so far on the right?
Lies very right much to the right is like saying the reaction goes to completion. Which means at equilibrium the concentration of products is very high and the reactants very low. In terms of Kc, lies very much to the right would mean a very large value of Kc.
Do you have a playlist of Inorganic/Organometallic Chemistry? or Coordination Chemistry? I searched in your channel but didn't find it. If not, are you thinking of making one? Cause I really like the way of explaining in all your playlists, and everything is well organized.
Dissociate means to break apart an ionic compound into its constituent ions. The term ionise means to form ions and is mainly used for covalent compounds. However they can be used interchangeably in this topic.
@@asasiphuma Salts such as NaCl (an ionic compound) dissociate into ions (Na+ and Cl-) in solution. HCl (a covalent molecule) ionises in solution to produce H+ and Cl- ions.
why do strong acids (that have one sided arrow bcz of the complete ionization) have equilibrium if there is no reverse reaction, since equilibrium is rate of forward reaction = to rate of reverse reaction? please expalin in detail and thank you !!!
For strong acids and bases, the reaction more or less goes to completion (the equilibrium position lies very far to the right). So much so that the reverse reaction can be said to not actually occur.
@@MSJChem
Thank you, but when you say it lies so far to the right what do you mean? What is the difference when we say equilibrium on the right and equilibrium so far on the right?
Lies very right much to the right is like saying the reaction goes to completion. Which means at equilibrium the concentration of products is very high and the reactants very low. In terms of Kc, lies very much to the right would mean a very large value of Kc.
Do you have a playlist of Inorganic/Organometallic Chemistry? or Coordination Chemistry? I searched in your channel but didn't find it.
If not, are you thinking of making one? Cause I really like the way of explaining in all your playlists, and everything is well organized.
I only cover topics in the DP chemistry syllabus. Organometallic chemistry is not covered so it’s unlikely I’ll make the videos.
these videos are useful and easy to understand! :)
Glad I could help.
How did u know that it is 0.004 at 2:55
I think he is just using that as an example of how it partially dissociates - you wouldn't need to memorize that or anything
@@ButtonForest i finished IB bro 🤣🤣🤣
@@shalabi569 Damn you didn't get an answer in time 😔 At least it will help future students
For us now M23
For us now M24
do you have to remember which acids and bases are strong and which are weak?
Yes.
@@MSJChem do you also have to know the hierarchy, like, is this acid stronger than this one and whatnot?
@XenSolation. No.
Can you please explain the difference between dissociation and ionization?
Dissociate means to break apart an ionic compound into its constituent ions. The term ionise means to form ions and is mainly used for covalent compounds. However they can be used interchangeably in this topic.
@@MSJChem okay. I think I understand. Would you mind giving an example?
@@asasiphuma Salts such as NaCl (an ionic compound) dissociate into ions (Na+ and Cl-) in solution. HCl (a covalent molecule) ionises in solution to produce H+ and Cl- ions.
@@MSJChem are all ionic compounds considered salts?
According to the IUPAC definition of a salt (a chemical compound consisting of cations and anions), yes. goldbook.iupac.org/terms/view/S05447