indictae the reactant that is a bronsted lowry acid.
HCN(aq) +H2O (l)---> H3O+(aq)=CN-(aq)
HCN
CN-
H20
H30
i think it is HCN the weak acid substance which acts as a proton (H+) donor and CN the weak base?
You are right. The HCN donates the proton (to H2O) so that makes HCN the Bronsted acid and CN^- is its conjugate base. H2O in the equation is the Bronsted base and H3O^+ is its conjugate acid.
Well, it looks like chemistry just loves to play with letters. In this reaction, the HCN is indeed the Bronsted Lowry acid, because it donates a proton (H+) to H2O. So, HCN is like the party animal who loves to share its protons with others. Meanwhile, CN- is the lucky recipient of the proton, making it the conjugate base. So, yes, HCN is the acid and CN- is the base in this reaction, while H2O and H3O+ are just chilling on the sidelines, minding their own business.
That's correct! HCN is the reactant that acts as a Bronsted-Lowry acid in the given equation. It donates a proton (H+) to water (H2O) to form H3O+ (hydronium ion) and CN- (cyanide ion). HCN can be considered a weak acid as it donates a proton. CN- can be considered a weak base as it accepts a proton.
To determine the reactant that is a Bronsted-Lowry acid, you can identify the substance that donates a proton (H+) in the reaction. In the given equation:
HCN(aq) + H2O(l) --> H3O+(aq) + CN-(aq)
The HCN donates a proton to H2O, forming H3O+. Therefore, HCN is the Bronsted-Lowry acid in this reaction.
Similarly, the substance that accepts the donated proton is called the Bronsted-Lowry base. In this case, H2O accepts the proton from HCN, making it the Bronsted-Lowry base. The H3O+ formed is the conjugate acid of H2O, and CN- is the conjugate base of HCN.
So, the reactant that is a Bronsted-Lowry acid in this reaction is HCN.