Final answer:
In a reaction between 1ml of 0.1 m copper (II) sulfate and 5ml of 0.1 m sodium sulfide, copper (II) sulfate is likely the limiting reactant. The solution's appearance after the reaction depends on the stoichiometry and reaction conditions, often resulting in a precipitate or color change.
Step-by-step explanation:
Limiting Reactant in Chemical Reactions
When mixing 1ml of 0.1 m copper (II) sulfate with 5ml of 0.1 m sodium sulfide, a chemical reaction occurs where copper (II) sulfate is likely the limiting reactant due to its smaller volume and molarity. In a reaction, the limiting reactant is the substance that is completely consumed first and therefore determines the maximum amount of product that can be formed. After the reaction, if copper (II) sulfate is the limiting reactant, you would typically observe a change in the solution, such as the formation of a precipitate or a color change, indicating the formation of a new compound.
Understanding the concept of limiting reactants is essential for predicting the amounts of products formed in chemical reactions. The theoretical yield is calculated based on the limiting reactant, whereas the excess reactant remains partially or wholly unreacted. To determine the percent yield, the actual amount of product obtained is compared to the theoretical yield.
In a lab setting, when a reaction is carried out between copper (II) sulfate and sodium sulfide, the appearance of the solution post-reaction would depend on the precise stoichiometry and the reaction conditions. An accurate prediction would require knowledge of the balanced chemical equation and the molar quantities of the reactants.