The $\text{MnO}_4^-$ ions in the potassium manganate(VII) oxidise the ethanedioate ions. Explain, using electron transfer, what the word oxidise means in the statement above.
Complete the ionic equation for the reaction of the manganate(VII) ions with the ethanedioate ions, balancing it fully. $2\text{MnO}_4^-\text{(aq)} + 5\text{C}_2\text{O}_4^{2-}\text{(aq)} + \ldots\ldots\text{H}^+\text{(aq)} \rightarrow \ldots\text{(aq)} + 10\text{CO}_2\text{(aq)} + \ldots\ldots\text{H}_2\text{O(l)}$
Calculate how many moles of manganate(VII) are used in the titration.
Use the equation in a(ii) together with your answer to b(i) to calculate how many moles of $\text{C}_2\text{O}_4^{2-}$ are present in the $25.0\,\text{cm}^3$ sample of solution used.
Calculate how many moles of $\text{H}_2\text{C}_2\text{O}_4\cdot x\text{H}_2\text{O}$ are in $6.30\,\text{g}$ of the compound.
Calculate the relative formula mass of $\text{H}_2\text{C}_2\text{O}_4\cdot x\text{H}_2\text{O}$.
The relative formula mass of anhydrous ethanedioic acid, $\text{H}_2\text{C}_2\text{O}_4$, is $90$. Calculate the value of $x$ in $\text{H}_2\text{C}_2\text{O}_4\cdot x\text{H}_2\text{O}$.