Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.405 M HCl. a) Write the net ionic equation for the reaction that takes place. b) How many moles of C₅H₅N would be present before the reaction takes place. c) How many moles of H+ would be present is 100.00mL of H+ were added
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Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.405 M HCl.
a) Write the net ionic equation for the reaction that takes place.
b) How many moles of C₅H₅N would be present before the reaction takes place.
c) How many moles of H+ would be present is 100.00mL of H+ were added
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