Edexcel A-Level Chemistry AS 1.5 The Concentration of a Solution in Mol Dm 3 And G Dm 3 Titration Calculations Are Not Required At This Stage Questions

Calculate solution concentration from mass, moles and volume, account for ion ratios, and use balanced equations to determine volumes and precipitating amounts.

Exam points

calculate mol dm^-3 from mass and volume, converting cm^3 to dm^3 accurately
find moles of ions in solution by combining concentration, volume and formula ratios
use concentration and balanced equations to determine required volumes or precipitating amounts

[Maximum number: 1]

This question is about magnesium, magnesium oxide and magnesium sulfate.

Hydrated crystals of magnesium sulfate, $\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}$ , can be made by reacting magnesium with sulfuric acid.

In an experiment, magnesium was added to $30.0 \mathrm{~cm}^{3}$ of $0.500 \mathrm{~mol} \mathrm{dm}^{-3}$ sulfuric acid.
$\left[M_{\mathrm{r}}\right.$ value: $\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}=246.4 \quad A_{\mathrm{r}}$ value: $\left.\mathrm{Mg}=24.3\right]$

Calculate the number of moles of sulfuric acid used in this experiment.

number of moles of sulfuric acid

Example of calculation
$30 \times 0.5 \div 1000=0.015 / 1.5 \times 10^{-2}(\mathrm{~mol})$

Do not award 1 SF .

(1)

All question bank results loaded

Edexcel A-Level Chemistry AS 1.5 The Concentration of a Solution in Mol Dm 3 And G Dm 3 Titration Calculations Are Not Required At This Stage Questions question 1