Chemistry Bronsted-Lowery Help: Understanding HCOOH + CN- and H2O + HCO3- Reactions

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    Acids and bases
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The discussion focuses on the reactions involving formic acid (HCOOH) and cyanide (CN-) as well as water (H2O) and bicarbonate (HCO3-). The first reaction, HCOOH + CN- producing HCOO- and HCN, is identified as unbalanced due to a discrepancy in hydrogen atom counts. The second reaction, H2O + HCO3- yielding H3O+ and CO3^2-, is presented as a reversible reaction. Participants seek clarification on the definitions of conjugate acids and bases, emphasizing their differences. Understanding these reactions and their balance is crucial for grasping Bronsted-Lowry acid-base theory.
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Homework Statement
Hi I'm super stuck in understanding bronsted lowry theory. I understand how it supposed to function but I can't wrap my brain around it. Generally any tips and advice in helping identifying bases and acids would greatly help me.

In the attempt at a solution is my possible take on this challenge, my friend offered to check it for me and said he is certain that the second one is completely incorrect.

Translation: First equation find acid and the conjugate acid.
Second equation find the base and the conjugate base.
Relevant Equations
bronsted lowry conjugate acids and conjugate bases.
1) HCOOH + CN- ---> HCOOH- + HCN


2) H2O + HCO3- <===> H3O+ + CO3-2
image_2022-01-26_191049.png
 
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Can you quote the definition of conjugate acid and base? How do they differ?
 
Reaction 1 is not a balanced chemical equation (compare the number of hydrogen atoms on the left side of the reaction vs the right side of the reaction).
 

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