Question

For each of the following acid-base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 5.75 g of the base. HCl(aq)+NaOH(aq)→H2O(l)+NaCl(aq)

Answer 1

Chemical reactions are always proceeds through stoichiometric ratio interms of number of moles from a well balanced chemical reaction equation, this is fundamental for any reaction.

Given reaction equation is already balanced i.e., 1 mole HCl reacts with 1 mole NaOH only.

Find the number of moles present in base NaOH, then exactly that much moles of acid HCl will consume since mole ratio of HCl:NaOH is 1:1. Now convert acid HCl moles into mass by multiplying HCl moles with HCl molar mass.

moles present in 5.75 g of base NaOH

= weight of base NaOH / molar mass of NaOH

= 5.75g / 39.997 g/mol

= 0.14376078205 mol

exactly this much moles of HCl are required,

now mass of acid HCl necessary to completely react with and neutralize 5.75 g of the base can be obtained by multiplying these moles with molar mass of HCl (36.46 g/mol).

= 0.14376078205 mol x 36.46 g/mol = 5.24151811386 grams

Mass of acid HCl necessary to completely react with and neutralize 5.75 g of the base = 5.24 g

in this way you can do the reactions of your interest perfectly.

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