The concentration of sodium hydroxide is 1.0 m and the concentration of crystal violet is 1.00 x 10-5 m. identify the limiting reagent and calculate how much of the excess reagent remains after the reaction runs to completion

Some additional information is required to answer this question: the volumes of the solutions. So this answer assume 10.0 ml of each solution.

Explanation:

This question deals with the first part of a common experiment carried out in a lab, where a solution is preperared by mixing certain volume of crystal violet of known concentration with a volume of sodium hydroxide of known concentration, to obtain information about the kinetics of the reaction.

Both volumes must be known too.

To solve the answer you must know the volumes of each solution.

For explanation purposes, I will assume that the solution is prepared by mixing 10.0 mL of the 1.0× 10⁻⁵ M crystal violet with 10.0 mL of the 0.10 M sodium hydroxide.

Crystal violet is the organic compound with unit formula formula: C₂₅N₃H₃₀Cl.

1) Chemical equation:

Crystal violet is an ionic compound and the reaction with sodium hydroxied may be represented as folllows:

2) Mole ratio:

So by each mol of crystal violet 1 mol of sodium hydroxide react.

3) Calculate the number of moles of each reactant:

3) Limiting reactant:

4) Excess reagent:

The excess reagent is sodium chloride. The amount of excess reagent that remains after the reaction runs to completion is calculated by:

       1.00×10⁻³ mol - 1.00×10⁻⁵ mol = 0.00100 mol - 0.0000100 mol = 0.00099 mol (sodium hydroxide)

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