Question

write dissociation in water of formic acid​

Answer 1

Answer:

Weak acids and weak bases

Explanation:

A weak acid is a proton donor that when put in water will only partially dissociate. A weak base is a proton acceptor that when put in water will only partially dissociate. Let's look at the example of a weak acid, formic acid, HCOOH. This is a carboxylic acid that has the following structure.

Answer 2

Answer:

Acid and base chemistry is a particular form of aqueous equilibria chemistry that is important in both chemistry and biology. The reason the chemistry is so specifically different is that unlike many other chemical processes in solution, in acid/base chemistry the solvent water is an active participant in the process.

Three key ideas to remember about acid/base chemistry.

1. You put stuff in water and something happens. Water is important in the chemistry. It not only solvates the chemical species (so they are "hydrated" by water molecules), but it allows them to break apart into ions.

2. There are many different definitions of acids and bases. For most of what we discuss we will use the Brønsted Lowry definition of acid and bases. In this definition

an acid is a proton donor

a base is a proton acceptor

The proton is H+, a hydrogen atom without an electron. The H+ is then a chemical species that is swapping from one molecule (the donor) to another molecule (the acceptor). This means there is never a reaction of an acid without a base. The proton always goes somewhere.

3. When you put things into water sometimes they break apart into ions to a small extent and sometimes to a large extent. The things that break apart a lot we call strong. The things that break apart a little we call weak. Much of acid/base chemistry deals with the very small concentrations that normally we would simply ignore. However, small amounts of protons can have large impacts on chemistry. So even when the concentrations are very small we need to keep track of them.

In all acid/base chemistry we are often tracking a small concentration of two ions in water. These are , water with an extra proton, H3O+ , called hydronium ion. Or water minus a proton, OH-, called the hydroxide ion. Note: often chemists are lazy and simply interchange H3O+ and H+ in aqueous solution. H3O+(aq) is more accurate, but if you see a reaction with H+(aq) know that this is simply a short hand that leaves out the water. Thus [H3O+] means the same things as [H+].

A video with an introduction to aqueous equilibria