2. ? Assume volumes are A sample of pure KHC_(2)O_(4)cdot H_(2)C_(2)O_(4)cdot 2H_(2)O (three replaceable hydrogens)requires 46.2 mL of 0.100 M NaOH for titration.How many milliliters of 0.100 M KMnO_(4) will the same-size sample react?

Question

Answer 1

To solve this problem, we need to determine the stoichiometry of the reaction between

and

.First, let's write the balanced chemical equation for the reaction between

and

:

From the balanced equation, we can see that 5 moles of

react with 2 moles of

.Now, let's calculate the number of moles of

in the sample:Moles of

= (Volume of NaOH solution * Concentration of NaOH solution) / (Molar mass of

)Moles of

= (46.2 mL * 0.100 M) / (204.22 g/mol) = 0.0225 molesSince 5 moles of

react with 2 moles of

, we can set up a proportion to find the number of moles of

needed:5 moles of

: 2 moles of

= 0.0225 moles of

: x moles of

Solving for x, we get:x = (0.0225 moles * 2 moles) / 5 moles = 0.009 moles of

Now, let's calculate the volume of 0.100 M

solution needed to react with the sample:Volume of

solution = Moles of

/ Concentration of

solutionVolume of

solution = 0.009 moles / 0.100 M = 0.09 L or 90 mLTherefore, the same-size sample will react with 90 mL of 0.100 M

solution.

Вопрос