Question

For parts of the free-response question that require calculations, clearly show the method used and the steps involved in arriving at your answers. You must show your work to receive credit for your answer. Examples and equations may be included in your answers where appropriate. HCl(aq)+NaOH(aq)?NaCl(aq)+H2O(l) A student was given the task of titrating a 20.mL sample of 0.10MHCl(aq) with 0.10MNaOH(aq) . The HCl(aq) was placed in an Erlenmeyer flask. An equation for the reaction that occurs during the titration is given above. (a) According to the equation for the reaction, if the amount of the reactants is halved, how does this affect the amount of H2O(l) produced in the reaction?

Answer 1

Answer: Answer: If the amount of reactants is halved, the amount of H2O(l) produced in the reaction will also be halved.

Explanation: The balanced equation for the reaction between HCl(aq) and NaOH(aq) is:

HCl(aq) + NaOH(aq) --> NaCl(aq) + H2O(l)

From this equation, it is clear that for every 1 mole of HCl(aq) and 1 mole of NaOH(aq) that react, 1 mole of H2O(l) is produced.

If the amount of reactants is halved, the amount of H2O(l) produced will also be halved, because the ratio of reactants to products is 1:1.

So, in the case of 20.mL of 0.10MHCl(aq) + 0.10MNaOH(aq) , the amount of H2O(l) produced is 20.mL x 0.10M = 2.00x10^-3mol.

If the amount of reactants is halved, the amount of H2O(l) produced in the reaction will be 1.00x10^-3mol.