By titration, it is found that 13.5 mL of 0.112 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the concentration of the HCl solution. HCl concentration: м
By titration, it is found that 13.5 mL of 0.112 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the concentration of the HCl solution. HCl concentration: м
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Transcribed Image Text:By titration, it is found that 13.5 mL of 0.112 M NaOH(aq) is needed to neutralize 25.0 mL of HCI(aq). Calculate the
concentration of the HCl solution.
HCl concentration:
м
Expert Solution
Step 1
Since the reaction taking place is given by
NaOH + HCl ----> NaCl + H2O
Hence we can say that 1 mole of HCl will need 1 mole of NaOH for the neutralization
Hence the moles of NaOH needed = moles of HCl present
Since moles of NaOH needed = concentration X volume in L = 0.112 X 13.5 / 1000
And moles of HCl present = concentration of HCl X volume of HCl in L = concentration of HCl X 25 / 1000
Hence equating both we get
concentration of HCl X 25 / 1000 = 0.112 X 13.5 / 1000
=> concentration of HCl = 0.0605 M
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