Question

Aqueous hydrochloric acid will react with solid sodium hydroxide to produce aqueous sodium chloride and liquid water . Suppose 30.3 g of hydrochloric acid is mixed with 25. g of sodium hydroxide. Calculate the minimum mass of hydrochloric acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

Answer 1

`m_(HCl)^(leftover)=7.50g`

Step-by-step explanation:

Hello.

In this case, since the undergoing chemical reaction is:

`HCl+NaOH\rightarrow NaCl+H_2O`

In order to identify the limiting reactant, we compute the available moles of sodium hydroxide (molar mass = 40 g/mol) and the moles of hydrochloric acid consumed by those moles via their 1:1 mole ratio considering the chemical reaction:

`n_(HCl)=25.0gNaOH*(1molNaOH)/(40gNaOH) *(1molHCl)/(1molNaOH) =0.625molHCl`

Next, since the molar mass of hydrochloric acid is 36.46 g/mol, we compute the mass of that reactant that is actually consumed:

`m_(HCl)=0.625molHCl*(36.46gHCl)/(1molHCl)=22.8gHCl`

In such a way, the leftover of HCl is:

`m_(HCl)^(leftover)=30.3g-22.8g\\\\m_(HCl)^(leftover)=7.50g`

Best regards!