I have seven homework problems. I did them but I wasn't sure if I did them correctly. Did I do them correct? Thank you!
Give the reaction that describes how the hydrazine, N2H4(aq), / hydrazinium ion, N2H51+(aq), buffer reacts with a strong base such as sodium hydroxide.
N2H4(aq) + OH^1-(aq) --> N2H51+(aq) + H2O(l)
Give the reaction that describes how the sodium bicarbonate / sodium carbonate buffer reacts with a strong base such as sodium hydroxide
H2CO3(aq) + OH^1-(aq) --> HCO3^1-(aq) + H2O(l)
Give the reaction that describes how the sodium hydrogen phosphate / sodium phosphate buffer reacts with a strong base such as sodium hydroxide
HPO4^2-(aq) + OH^1-(aq) --> PO4^3-(aq) + H2O(l)
Give the reaction that describes how the trimethylamine, (CH3)3N(aq) / trimethylammonium ion, (CH3)3NH1+(aq), buffer reacts with a strong acid such as hydrochloric acid
(CH3)3NH1+(aq) + H3O^1+(aq) --> (CH3)3N(aq) + H2O(l)
Give the reaction that describes how the ethylamine, C2H5NH2(aq), / ethylammonium ion, C2H5NH31+(aq), buffer reacts with a strong acid such as hydrochloric acid
C2H5NH31+(aq) + H3O^1+(aq) --> C2H5NH2(aq) + H2O(l)
Give the reaction that describes how the hydrofluoric acid / sodium fluoride buffer reacts with a strong acid such as hydrochloric acid.
F^1-(aq) + H3O^1+(aq) --> HF(aq) + H2O(l)
Give the reaction that describes how the hydrazine, N2H4(aq), / hydrazinium ion, N2H51+(aq), buffer reacts with a strong base such as sodium hydroxide.
N2H4(aq) + OH^1-(aq) --> N2H51+(aq) + H2O(l)
I don't think so. The OH^- will react with the acid, N2H5^+, like this
N2H5^+ + OH^- ==> H2O + N2H4
Give the reaction that describes how the sodium bicarbonate / sodium carbonate buffer reacts with a strong base such as sodium hydroxide
H2CO3(aq) + OH^1-(aq) --> HCO3^1-(aq) + H2O(l)
HCO3^- is the acid in the HCO3^-/CO3^2- system. H2CO3 isn't there so you can't use that.
HCO3^- + OH^- ==> H2O + CO3^2-
Give the reaction that describes how the sodium hydrogen phosphate / sodium phosphate buffer reacts with a strong base such as sodium hydroxide
HPO4^2-(aq) + OH^1-(aq) --> PO4^3-(aq) + H2O(l)
This looks ok.
Give the reaction that describes how the trimethylamine, (CH3)3N(aq) / trimethylammonium ion, (CH3)3NH1+(aq), buffer reacts with a strong acid such as hydrochloric acid
(CH3)3NH1+(aq) + H3O^1+(aq) --> (CH3)3N(aq) + H2O(l)
The base is what reacts with the acid; therefore,
(CH3)3N(aq) + HCl ==> (CH3)3NH^+ + Cl^-
Give the reaction that describes how the ethylamine, C2H5NH2(aq), / ethylammonium ion, C2H5NH31+(aq), buffer reacts with a strong acid such as hydrochloric acid
C2H5NH31+(aq) + H3O^1+(aq) --> C2H5NH2(aq) + H2O(l)
Same comment as the trimethylamine above.
Give the reaction that describes how the hydrofluoric acid / sodium fluoride buffer reacts with a strong acid such as hydrochloric acid.
F^1-(aq) + H3O^1+(aq) --> HF(aq) + H2O(l)
This looks ok to me.
To check if you did the homework problems correctly, we can analyze each reaction and see if they follow the correct acid-base reaction principles.
For the reaction with hydrazine / hydrazinium ion buffer, the correct balanced equation is:
N2H4(aq) + OH^-(aq) → N2H5^+(aq) + H2O(l)
This is a valid acid-base reaction. The hydrazine (N2H4) acts as a base, accepting an OH^-(hydroxide ion) to form the hydrazinium ion (N2H5^+), and water is formed in the process.
For the reaction with sodium bicarbonate / sodium carbonate buffer, the correct balanced equation is:
H2CO3(aq) + OH^-(aq) → HCO3^-(aq) + H2O(l)
This is also a valid acid-base reaction. The bicarbonate ion (HCO3^-) acts as a base, accepting an OH^- to form the carbonate ion (CO3^2-), and water is formed.
For the reaction with sodium hydrogen phosphate / sodium phosphate buffer, the correct balanced equation is:
HPO4^2-(aq) + OH^-(aq) → PO4^3-(aq) + H2O(l)
Again, this is a valid acid-base reaction. The hydrogen phosphate ion (HPO4^2-) acts as a base, accepting an OH^- to form the phosphate ion (PO4^3-), and water is formed.
For the reaction with trimethylamine / trimethylammonium ion buffer, the correct balanced equation is:
(CH3)3NH^+(aq) + H3O^+(aq) → (CH3)3N(aq) + H2O(l)
This is a valid acid-base reaction. The trimethylammonium ion acts as an acid, donating an H^+ to form trimethylamine, and water is formed.
For the reaction with ethylamine / ethylammonium ion buffer, the correct balanced equation is:
C2H5NH3^+(aq) + H3O^+(aq) → C2H5NH2(aq) + H2O(l)
This is also a valid acid-base reaction. The ethylammonium ion acts as an acid, donating an H^+ to form ethylamine, and water is formed.
Finally, for the reaction with hydrofluoric acid / sodium fluoride buffer, the correct balanced equation is:
F^-(aq) + H3O^+(aq) → HF(aq) + H2O(l)
This is a valid acid-base reaction. The fluoride ion (F^-) acts as a base, accepting an H^+ to form hydrofluoric acid, and water is formed.
Based on the balanced equations provided, it seems like you did the homework problems correctly. Well done!