A student is asked to perform a neutralization reaction between hydrochloric acid, HCl and sodium hydroxide, NaOH. The student transfers 5.00 mL of HCl solution to the titration flask and then adds 25.0 mL of distilled water and 3 drops of phenolphthalein indicator to the solution. The resulting solution uses 35.5 mL of 0.125M NaOH solution to reach the end point. a. Write a balanced chemical equation for the neutralization process. b. What will be the color of solution at the end point? c. Calculate the number of moles of NaOH used for complete neutralization.

Question

A student is asked to perform a neutralization reaction between hydrochloric acid, HCl and sodium hydroxide, NaOH. The student transfers 5.00 mL of HCl solution to the titration flask and then adds 25.0 mL of distilled water and 3 drops of phenolphthalein indicator to the solution. The resulting solution uses 35.5 mL of 0.125M NaOH solution to reach the end point.
a. Write a balanced chemical equation for the neutralization process.
b. What will be the color of solution at the end point?
c. Calculate the number of moles of NaOH used for complete neutralization.
d. Calculate the strength in terms of molarity for HCl solution
e. Calculate the m/v percent strength of the HCl solution

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