The above reaction proceeds as :
HBr + NaOH ---> NaBr + H2O
We use the mole concept to analyse the problem.
As we can see, 1 mole of HBr reacts with 1 mole of NaOH to produce 1 mole of water.
That is, every 81g of HBr reacts with 40 g of NaOH to produce 18 g of water.
We are provided with 1.6g and 1.3 g of HBr and NaOH respectively.
We first find the limiting reagent.
As 81 g HBr reacts with 40 g NaOH, 1.3 g NaOH should react with : (81 / 40 ) * 1.3 = 2.6325 g of HBr. However, we have 1.6 g of HBr, which is therefore in short supply.
Therefore, HBr is the limiting reagent in this reaction.
1.6 g of HBr reacts with NaOH to produce = ( 18 / 81) * 1.6 = 0.356 g water
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