In each space below, enter one or more of the letters A-D, as needed. Which of these compounds can exist as optical isomers?
On hydrolysis, which of these compounds yield(s) a secondary alcohol?
Ethanoic acid, $\text{CH}_3\text{CO}_2\text{H}$, is one of the products formed when all of these compounds undergo hydrolysis. State the reagents and conditions required for this hydrolysis.
The acid dissociation constant, $K_a$, of ethanoic acid is $1.75 \times 10^{-5}\ \text{mol dm}^{-3}$. Explain why this value of $K_a$ is much larger than that of ethanol, $\text{CH}_3\text{CH}_2\text{OH}$, and smaller than that of chloroethanoic acid, $\text{ClCH}_2\text{CO}_2\text{H}$.
Calculate the pH of a $0.100\ \text{mol dm}^{-3}$ solution of ethanoic acid.
$20.0\ \text{cm}^3$ of $0.100\ \text{mol dm}^{-3}$ NaOH were gradually added to a $10.0\ \text{cm}^3$ sample of $0.100\ \text{mol dm}^{-3}$ ethanoic acid, while the pH was recorded throughout the addition. Calculate the number of moles of NaOH remaining at the end of the addition.
Calculate the $[\text{OH}^-]$ at the end of the addition.
Using $K_w = [\text{H}^+][\text{OH}^-]$ and your value from (ii), calculate $[\text{H}^+]$ and the pH of the solution at the end of the addition.
On the axes below, sketch the way in which pH changes as a total of $20.0\ \text{cm}^3$ of $0.100\ \text{mol dm}^{-3}$ NaOH is added. Make sure the end point is clearly indicated.
From the list of indicators below, place a tick in the box beside the one you judge to be most suitable for this titration.