Strong Acid
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 29
- Joined: Fri Apr 06, 2018 11:01 am
-
- Posts: 31
- Joined: Fri Apr 06, 2018 11:03 am
Re: Strong Acid
It completely dissociates in water and increases the [H3O^+] concentration thus decreasing pH.
-
- Posts: 30
- Joined: Fri Apr 06, 2018 11:02 am
- Been upvoted: 1 time
Re: Strong Acid
A strong acid is based on the bond between the H+ part of the molecule, and the negative ion. So HCl is totally fine separating into H+ and Cl- which makes it a strong acid.
When we measure pH, we are talking about the amount of H+/H3O+ (which is H+ + H2O -> H3O+). The greater a concentration of H3O+, the more acidic.
Molecules like H2CO3, are much less likely to dissociate in water (of course there will be a little, but that is what makes it weak).
When we measure pH, we are talking about the amount of H+/H3O+ (which is H+ + H2O -> H3O+). The greater a concentration of H3O+, the more acidic.
Molecules like H2CO3, are much less likely to dissociate in water (of course there will be a little, but that is what makes it weak).
-
- Posts: 30
- Joined: Fri Apr 06, 2018 11:01 am
Re: Strong Acid
Acid solutions contain hydrogen ions. The higher the concentration of hydrogen ions, the lower the pH. A strong acid also completely dissociates in water.
-
- Posts: 31
- Joined: Fri Apr 06, 2018 11:04 am
Re: Strong Acid
A strong acid can completely disassociate in water. As they have hydrogen ions, the higher the hydrogen concentration, the lower the pH is. In a compound it is dependent on the H bond and the negative ion.
-
- Posts: 67
- Joined: Fri Sep 28, 2018 12:24 am
Re: Strong Acid
When a strong acid dissociates, this yields a high concentration of H+ ions. Using the equation pH=-log[H+], you will find that the pH is very low which correlates to a strong acid.
-
- Posts: 62
- Joined: Fri Sep 28, 2018 12:28 am
Re: Strong Acid
They dissociate completely in water to form hydronium ions. Examples would be HCl, HBr, HNO3 etc.
Return to “Lewis Acids & Bases”
Who is online
Users browsing this forum: No registered users and 0 guests