CHEM QUESTION

Consider the reaction of a 20.0 mL of 0.220 M CSHSNHCI (Ka = 5.9 x 10.5) with 12.0 mL of 0.201 M CsOH. a) Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction. b) What quantity in moles of CSHSNH+ would be present at the start of the titration? c) What quantity in moles of OH' would be present in 12.0 mL of CsOH solution? d) What species would be left in the beaker after the reaction goes to completion? e) What quantity in moles of CSHSNH+ would be left in the beaker after the reaction goes to completion? f) What quantity in moles of CSHSN are produced after the reaction goes to completion? 9) What would be the pH of this solution after the reaction goes to completion and the system reaches equilibrium?