I wrote the dissociation or ionization in water for each of the following acids. I just want someone to check if they are right.
a) HC3H5O2(aq)<===> H^+(aq)+ C3H5O2^-(aq)
b) (CH3)2NH2^+(aq)<===> H^+(aq)+ (CH3)2NH(aq)
c) CH3COOH(aq)<===> H^+(aq)+ CH2COOH^-(aq)
d) H2PO4^-(aq)<===> H^+(aq)+ HPO4^2-
e) [Mn(H2O)6]^2+ <===> I don't know what to do with this one
Thanks
e) [Mn(H2O)6]^2+(aq)<===> H^+(aq)+ [Mn(H2O)5]5OH^+(aq)
a) HC3H5O2(aq)<===> H^+(aq)+ C3H5O2^-(aq)
This is an odd way to write the this
a) C3H5O2H(aq)<===> H^+(aq)+ C3H5O2^-(aq)
Your answer to a) means you have shown the wrong proton dissociating here.
c) CH3COOH(aq)<===> H^+(aq)+ CH2COOH^-(aq)
should be
c) CH3COOH(aq)<===> H^+(aq)+ CH3COO^-(aq)
[It is possible to remove the proton that you have shown but not in water]
I am not clear what they are after for e) either.
They may be simple be looking for
e) [Mn(H2O)6]^2+H2O<===> H^+(aq)+ [Mn(H2O)6]OH^+(aq)
Thanks, that helped a lot
a) HC3H5O2(aq) <===> H+(aq) + C3H5O2-(aq)
The dissociation or ionization of acetic acid (HC3H5O2) in water is correct. It breaks into H+ ions and C3H5O2- ions in the aqueous solution.
b) (CH3)2NH2+(aq) <===> H+(aq) + (CH3)2NH(aq)
The dissociation or ionization of dimethylamine (CH3)2NH2+ in water is correct. It forms H+ ions and (CH3)2NH or dimethylamine in the aqueous medium.
c) CH3COOH(aq) <===> H+(aq) + CH2COOH-(aq)
The dissociation or ionization of acetic acid (CH3COOH) in water is incorrect. Acetic acid dissociates into H+ ions and CH3COO- ions, not CH2COOH- ions. The correct equation should be:
CH3COOH(aq) <===> H+(aq) + CH3COO-(aq)
d) H2PO4-(aq) <===> H+(aq) + HPO42-
The dissociation or ionization of dihydrogen phosphate (H2PO4-) in water is correct. It forms H+ ions and HPO42- ions in the aqueous medium.
e) [Mn(H2O)6]^2+ <===> I don't know what to do with this one
The compound [Mn(H2O)6]^2+ is a coordination complex. It does not readily dissociate or ionize in water to produce H+ or OH- ions. Therefore, in this case, there is no simple dissociation or ionization equation.