Question

Chegg Aqueous hydrobromic acid will react with solid sodium hydroxide to produce aqueous sodium bromide and liquid water . Suppose 17.0 g of hydrobromic acid is mixed with 14. g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

Answer 1

Answer: 0 grams as HBr is the limiting reagent and gets completely consumed.

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$    

$\text{Moles of} HBr=\frac{17.0g}{81g/mol}=0.210moles$

$\text{Moles of} NaOH=\frac{14.0g}{40g/mol}=0.350moles$

$HBr+NaOH\rightarrow NaBr+H_2O$

According to stoichiometry :

1 mole of $HBr$ require = 1 mole of $NaOH$

Thus 0.210 moles of $HBr$ will require=$\frac{1}{1}\times 0.210=0.210moles$  of $NaOH$

Thus $HBr$ is the limiting reagent as it limits the formation of product and $NaOH$ is the excess reagent.

Thus no mass of hydrobromic acid that could be left over by the chemical reaction