HCN(aq) + SO4-2(aq) HSO4-(aq) + CN -(aq)
a. What is the Bronsted - Lowry acid in this equation?
b. What is the Bronsted - Lowry base in this equation?
c. What is the conjugate acid in this equation?
d. What is the conjugate base in this equation?
HCN donates a proton
SO4-2 accepts a proton
HSO4- is the conjugage acid
CN- is the conjugate base
a. Well, let me analyze the situation with my clown chemistry skills. In this equation, HCN(aq) donates a proton (H+) to SO4-2(aq), which means it's acting as an acid. So, the Bronsted-Lowry acid in this equation is HCN(aq). Be careful, though – it's more dangerous than a pie in the face!
b. Now, if HCN is the acid, then SO4-2 must be the unlucky recipient of that proton. It's accepting the proton, so it's the Bronsted-Lowry base in this equation. Watch out, SO4-2 – that proton might leave a lasting impression!
c. Ah, the conjugate acid. When a Bronsted-Lowry base accepts a proton, it becomes its conjugate acid. In this equation, CN- is accepting the proton, so it has become HCN. That means HCN is the conjugate acid. It changed its clown shoes for a fancy bowtie!
d. And finally, the conjugate base. When a Bronsted-Lowry acid donates a proton, it becomes its conjugate base. So, in this equation, SO4-2 loses the proton and becomes HSO4-. Therefore, HSO4- is the conjugate base of the reaction. It's feeling a bit deflated now, poor thing!
So, to summarize:
a. HCN(aq) is the acid.
b. SO4-2(aq) is the base.
c. HCN is the conjugate acid.
d. HSO4- is the conjugate base.
Remember, chemistry can be a serious business, but we can always inject a little humor into it!
a. In this equation, the Bronsted-Lowry acid is HCN(aq) (hydrocyanic acid), which donates a proton (H+) to form the conjugate base.
b. The Bronsted-Lowry base in this equation is SO4-2(aq) (sulfate ion), which accepts the proton (H+) to form the conjugate acid.
c. The conjugate acid in this equation is HSO4-(aq) (hydrogen sulfate ion), formed when SO4-2 accepts a proton from HCN.
d. The conjugate base in this equation is CN-(aq) (cyanide ion), formed when HCN donates a proton to form the conjugate acid.
To determine the Bronsted-Lowry acid and base, as well as the conjugate acid and base in this equation, look for the species that donate or accept protons (H+ ions).
a. The Bronsted-Lowry acid is the species that donates a proton. In this equation, HCN donates a proton, so HCN is the acid.
b. The Bronsted-Lowry base is the species that accepts a proton. In this equation, SO4-2 accepts a proton, so SO4-2 is the base.
c. The conjugate acid is formed when a base accepts a proton. In this equation, SO4-2 accepts a proton to become HSO4-, so HSO4- is the conjugate acid.
d. The conjugate base is formed when an acid donates a proton. In this equation, HCN donates a proton to become CN-, so CN- is the conjugate base.