Final answer:
The volume of 0.1 N K₂Cr₂O₇ solution needed to convert 1.19 g of Sn to SnCl₄ cannot be determined without the balanced chemical equation for the reaction in an acidic medium, which would provide the necessary stoichiometry.
Step-by-step explanation:
To find the volume of decinormal (0.1 N) K₂Cr₂O₇ solution required to convert 1.19 g of tin (Sn) to stannic chloride (SnCl₄) in an acidic medium, we first calculate the number of moles of Sn. Using the molar mass of Sn (119 g/mol), we get 0.01 moles of Sn. The balanced chemical equation for the reaction between Sn and K₂Cr₂O₇ in an acidic medium will provide the stoichiometry necessary to determine the volume of K₂Cr₂O₇ needed. However, without the balanced equation, we can't proceed further with the calculation.
The general idea in a titration, such as with K₂Cr₂O₇ and Fe²⁺, is that the moles of the titrant and analyte are related by the stoichiometry of the balanced chemical equation. In a similar case, where it required a certain volume of K₂Cr₂O₇ to titrate Fe²⁺, it was found that each mole of K₂Cr₂O₇ reacts with six moles of Fe²⁺. Such information helps to understand the relation between the substances during the reaction.