Which compounds are the Bronsted-Lowry bases in this equilibrium: $HC_2O_4^- + H_2BO_3^(-) rightleftharpoons H_3BO_3 + C_2O_4^(2-)$?

You know that $color(white)(aaaa)"HF"_ ((aq)) rightleftharpoons "H"_ ((aq))^(+) + "F"_ ((aq))^(-)" "K_(c1) = 6.8 * 10^(-4)$ $"H"_ 2"C"_ 2"O"_ (4(aq)) rightleftharpoons 2"H"_ ((aq))^(+) + "C" _ 2"O"_ (4(aq))^(2-)"...

Arrhenius measured the conductivity of highly pure samples of water. Because even the most pure samples retained a conductance, Arrhenius proposed an equilibrium between charged particles, and base ........... $H_2O...

Bronsted Acid is an H+ donor, Bronsted Base is an H+ acceptor. Usually Bronsted Acids have an H bonded to a halogen or an oxygen. A base, usually OH- or...

Bronstead-Lowry bases are species that can accept a proton due to a high energy pair of electrons being present. For Example, Ammonia acts as a base when reacting with...

Identify the Bronsted-Lowry base in this reaction. $"NH"_4^(+) + "H"_2"O" rightleftharpoons "NH"_3 + "H"_3"O"^(+)$ Lewis acid: $"NH"_4^(+)$ Bronsted-Lowry acid: $"NH"_4^(+)$ Lewis base: $"H"_2"O"$ Bronsted-Lowry base: ??? Conjugate base:...

Bronsted and Lowry characterized acid base behaviour on the basis of proton transfer, $H^+$. The acid was the proton donor, and the base the proton acceptor. I think your question...

A Bronsted Lowry ion is a species that acquires hydrogen ions

Alternatively, $HCO_3^(-) + H^(+)(aq) rightleftharpoonsH_2CO_3(aq)$ $H_2CO_3$ is so-called $"carbonic acid"$; which is probably better represented as $H_2O*CO_2(aq)$. You could not buy a bottle of the same, though you could make...

$c.$, you got $"bisulfate ion"$; in aqueous solution this is a moderately strong acid. Certainly we treat $H_2SO_4$ as a diacid in aqueous solution. $e.$, you got $"ammonium ion"$; in...

Boric acid is a weak, monoprotic acid in water, whose $pK_(a1)$ $=$ $9.24$. To titrate this successfully in aqueous solution, often quantities of mannitol are added (the mannitol is added...