Determine the mass of the crystals used in the experiment.
The crystals in the beaker are added to water. State two methods for making them dissolve as fast as possible.
Suggest how the student can ensure that every drop of solution in the beaker ends up in the volumetric flask.
Why is a pipette chosen rather than a measuring cylinder?
Which colour change is seen in the conical flask when the titration reaches the end-point?
Use the diagrams to fill in the results table and work out the average volume of $0.0100\text{ mol dm}^{-3}$ potassium manganate(VII).
Why must this student carry out three titrations rather than averaging the first two results?
Calculate the amount, in moles, of potassium manganate(VII) present in the average volume of $0.0100\text{ mol dm}^{-3}$ potassium manganate(VII).
Find the number of moles of $H_2C_2O_4\cdot xH_2O$ contained in $25.0\text{ cm}^3$ of $D$.
Find the number of moles of $H_2C_2O_4\cdot xH_2O$ in $250\text{ cm}^3$ of $D$.
Using your answers to (a) and (i), work out the relative molecular mass of $H_2C_2O_4\cdot xH_2O$.
Using your answer to (j), calculate the value of $x$ in $H_2C_2O_4\cdot xH_2O$.