It might not be obvious until chem 183 why the \"limiting reagent\" concept is u

Question

It might not be obvious until chem 183 why the "limiting reagent" concept is useful. For example, in chapter 18 (p. 716), the book presents a "stoichiometry" table. This refers to limiting reagent calculations. Suppose you have 17 mL of an HCl solution (concentration 400 mg/mL), and react it with 32 mL of an NaOH solution (concentration 250 mg/mL). This reaction proceeds in a 1:1 mol ratio. What is the limiting reagent? HCl is the limiting reagent. NaOH is the limiting reagent. Neither HCl nor NaOH is a limiting reagent in this reaction.

Explanation / Answer

mass of HCl = 17 x 400 = 6800 mg

                    = 6.8 g

moles of HCl = 6.8 / 36.5 = 0.186

mass of NaOH = 32 x 250 = 8000 mg = 8.0 g

moles of NaOH = 8 / 40 = 0.2

HCl   +   NaOH   ----------------> NaCl + H2O

1           1

0.186     0.2

here limiting reagent is HCl.

because mol ration of HCl is less than the NaOH.

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