Final answer:
In your experiment, depending on the step, you should initially pour 5 ml of H₂SO₄ into the funnel, and then repeat the process with 10 ml of H₂SO₄. A balanced equation is crucial for stoichiometry, which in turn helps to calculate the necessary volume of reagents for a reaction.
Step-by-step explanation:
When handling an experiment involving sulphuric acid (H₂SO₄), it's crucial to measure out the correct volume of the acid to ensure the success of the experiment and maintain safety in the lab. In your provided instructions, it is initially stated that 5 ml of H₂SO₄ should be carefully poured into the funnel. After the first reaction, you are instructed to repeat the steps but this time using 10 ml of H₂SO₄. The usage of sulphuric acid within reactions usually involves stoichiometric calculations to determine the correct amount needed to react with a given substance or to achieve a desired concentration.
A balanced equation, such as one involving H₂SO₄ reacting with a base like ammonia (NH₃) to form ammonium sulphate ((NH₄)₂SO₄), helps to find the mole ratio necessary for the reaction. For example, the equation H₂SO₄ (aq) + 2NH₃ (g) → (NH₄)₂SO₄ (aq) shows a 1:1 mole ratio between H₂SO₄ and (NH₄)₂SO₄. With stoichiometry, you can then calculate the exact moles of substances required for a reaction, such as neutralizing H₂SO₄ with potassium hydroxide (KOH), where the equation provided indicates a 1 mol H₂SO₄ to 2 mol NaOH ratio.