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The thermodynamic dissociation constant of formic acid (HCOOH) is Kd=1.77104 in water at 25C and 1atm. With this information (and neglecting the intrinsic dissociation of water): (a) Determine the molality (and pH ) at equilibrium if one prepares a solution by dissolving initially 1.5g of acid in 300g of water. (b) Repeat the calculation when preparing a solution with 0.075mol of HCl and 0.15mol of potassiun formiate ( HCOOK ) in 300g. (Both HCl and HCOOK are strong electrolytes, leading to the formation of the weak eletrolyte HCOOH in situ after their full dissociation.) Data: Consider the activity coefficient for the unionized formic acid as (formic acid) 1. Determine the molality of mH+(and pH) in a solution of HCN in water at 25C and 1atm prepared initially with mini=2104mol/kg of "undissociated HCN ", where the thermodynamic dissociation constant is Kd=6.21010. (Note that the values of Kd0 and mini are small and thus one must include the intrisic dissociation of water, in contrast with Probl. (14). Determine mH+by combining the two simultaneous equilibria.)