50 ml of a mixture consisting of 0.019 m cerium (iv) and 2.7 m h2so4, or sulfuric acid. begin by preparing 100 ml of 2.7 m h2so4 using the available solution of 42.3% w/w h2so4. this concentration unit, which may be less familiar to you, is a weight-to-weight percent (100.0 g of the solution contains 42.3 g of h2so4). the density of 42.3% w/w h2so4 is 1.25 g solution/ml solution. using a graduated cylinder, measure out the correct volume of 42.3% w/w h2so4 and slowly add it to a 100-ml volumetric flask that already contains approximately 25 ml of deionized water.

The correct volume of 42.3% w/w H₂SO₄ is 50,1 mL

Explanation:

In order to know the correct volume of 42.3% w/w H₂SO₄ needed, we need to know the mass of H₂SO₄ that is needed. We'll use the wanted concentration, the final volume and the molecular weight of sulphuric acid, thus:

2,7 M * 0,1 L * 98,079 g/mol = 26,48 g of sulphuric acid are needed.

Now we can calculate the correct volume, using the concentration of the available solution, and the density of said solution, thus:

We would then need to measure 50,1 mL (rounded up) of 42.3% w/w H₂SO₄ with the graduated cylinder, and then add it to the volumetric flask.

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it is stable as it is in group 0 which have full outer shells of electrons