1. Balanced Reaction a. You add 1.00 mL tert-butyl chloride to 100.0 mL of your
ID: 1061919 • Letter: 1
Question
1. Balanced Reaction
a. You add 1.00 mL tert-butyl chloride to 100.0 mL of your organic solvent (soln A).
Calculate the concentration (moles/liter) of tert-butyl chloride in your solution A.
___________
b. How many moles of t-BuCl (tert-butyl chloride) are in a 10.00-mL aliquot of soln A?
___________
c. If the organic solvent is an alcohol/water mixture with more than sufficient amount of
water to react with the t-BuCl according to the Balanced Reaction above, how many
moles of HCl will be produced in this 10.00-mL aliquot of soln A in the above problem,
upon complete reaction?
___________ moles t-BuCl * (1 mol HCl produced/ 1 mol t-BuCl reacted) = __________
d. How many mL of 0.0400 M NaOH (aq) solution would be required to titrate (neutralize)
this 10.00 mL aliquot of soln A after the reaction has been allowed to proceed to
completion (one week's time is sufficient for this 99.99+% completion).
___________
Explanation / Answer
(a) Density of t-butyl chloride = 0.84 g/mL
Mass of 1 mL of t-butyl chloride = 0.84 g.
Molar mass of t-butylchloride = 92.57 g/mol
Moles of t-butylchloride taken in 100 mL solvent = 0.89 g / (92.57 g/mol) = 0.0096 moles.
Concentration of solution in moles per litre = 0.0096 mole / 100 mL * 1000 mL / 1 L = 0.096 M
(b) 1 L of solution contains = 0.096 moles
10 mL will have = 0.096 mol * 10 mL/1000mL = 0.00096 moles.
(c) When reaction is complete , according to balanced chemical equation 1 mole of t-butyl chloride yields 1 mole of HCl.
Thus 0.00096 moles (present in 10 mL solution) of t-butylchloride will yield 0.00096 moles of HCl upon completing the reaction.
(d) Since 10 mL solution will yield 0.00096 moles of HCl upon completion, we need 0.00096 moles of NaOH to titrate it.
Volume of NaOH which will have 0.00096 moles of NaOH can be calculated as:
Volume = 0.00096 mol / (0.0400 mol/L) = 0.024 L = 24 mL.
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