Question $1$

The simplest carboxylic acid is methanoic acid $($or formic acid$),H\frac{C}{O}OH,$ which occurs naturally in ants.

When an ant bites, it injects an aqueous solution of $50\%($by volume$)$ methanoic acid, typically injecting around $6\mathrm{.}0{10}^{-3}mL$ of this solution.

a$)$ For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects $80\%$ of its methanoic acid, what is the total volume of pure methanoic acid contained in a 'typical ant'?

b$)$ How many 'typical' ants would have to be distilled to produce $1L$ of pure methanoic acid?

Sodium hydrogencarbonate, $NaHC{O}_3,$ is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is:

$()-$

c$)$ Given that the density of methanoic acid is $1\mathrm{.}2gm{L}^{-1},$ how many moles of methanoic acid does a typical ant inject?

d$)$ What mass $(g)$ of sodium hydrogencarbonate would be required to completely neutralise a typical ant sting?