A student was given the task of titrating a 20. mL sample of (aq)0.10 M HCl with 0.10 M NaOH(aq). The HCl 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 water produced in the reaction?
(b) Write the net ionic equation for the equation written above
(c) In the equation you wrote in part (b), which species is a proton acceptor?
(d) How many moles of HCl are in the 20. mL sample of 0.10 M HCl?
(e)
The graph above shows the results of the titration of the 20. mL sample of 0.10 M HCl with 0.10 M NaOH. On the graph, draw an
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to identify the location of the equivalence point of the titration.
f) Using the graph in (e), at what pH does the equivalence point occur? What does that tell you about the strength of the acid and the base?
(g)
The student performs a second titration using the 0.10 M NaOH solution again as the titrant, but this time with a 20. mL sample of 0.20 M HCl instead of 0.10 M HCl.
The box below to the left represents ions in a certain volume of 0.10 M HCl. In the box below to the right, draw, or explain, a representation of ions in the same volume of 0.20 M HCl. (Do not include any water molecules in your drawing.)

(h) The student made observations related to the contents of the Erlenmeyer flask during the titration. Identify an observation that could have led the student to conclude that a chemical change took place during the titration.