Calculate the concentration, in $\text{mol dm}^{-3}$, of $\text{ClO}^-$ ions in the bleach solution.
Name a suitable indicator for this titration.
State the colour change you would expect to see at the end-point in this titration.
State at what stage in the procedure you would add the indicator.
When an excess of aqueous hydrogen peroxide was added to $5.0\,\text{cm}^3$ of a different bleach solution, $82\,\text{cm}^3$ of oxygen was produced at room temperature and pressure. Calculate the concentration of $\text{ClO}^-$ ions in this bleach solution.
Write the expression for $K_c$ for the equilibrium: $\text{C}_3\text{Cl}_3\text{N}_3\text{O}_3 + 3\text{H}_2\text{O} \rightleftharpoons \text{C}_3\text{H}_3\text{N}_3\text{O}_3 + 3\text{HClO}$
In outdoor swimming pools, $\text{HClO}$ is decomposed by sunlight. The decomposition of $\text{HClO}$ is a redox reaction which forms a gas that relights a glowing splint. Describe and explain the effect of the decomposition of $\text{HClO}$ on the equilibrium in (d). State the effect on $K_c$.
Trichlorocyanuric acid, $\text{C}_3\text{Cl}_3\text{N}_3\text{O}_3$, works as a chlorine buffer and disinfectant in swimming pools. It reacts with water to produce chloric(I) acid, $\text{HClO}$. $\text{C}_3\text{Cl}_3\text{N}_3\text{O}_3 + 3\text{H}_2\text{O} \rightleftharpoons \text{C}_3\text{H}_3\text{N}_3\text{O}_3 + 3\text{HClO}$
The decomposition of $\text{HClO}$ is a redox reaction. Suggest an equation for this reaction.
The buffer system in blood is a mixture of carbonic acid, $\text{H}_2\text{CO}_3$, and hydrogencarbonate ions, $\text{HCO}_3^-$. Healthy blood has a pH of $7.40$. $\text{H}_2\text{CO}_3 + \text{H}_2\text{O} \rightleftharpoons \text{HCO}_3^- + \text{H}_3\text{O}^+ \qquad K_a = 7.94 \times 10^{-7}\,\text{mol dm}^{-3}$
Explain how this buffer system works to control the blood pH. Include equations in your answer.
A patient’s blood has a $[\text{HCO}_3^-] : [\text{H}_2\text{CO}_3]$ ratio of $9.5 : 1$. Calculate the pH of the patient’s blood.