Agl is a slightly soluble salt with Ksp = 1.5x1016, In presence of NH3 silver ion forms the complex Ag(NH3)2* with Kf = 1.7x10. %3D Use these information to answer the next 2 questions. Question 2 Calculate the equilibrium constant (K) for the reaction shown below: Agl (s) + 2 NH3 (aq) A Ag(NH3)2" (aq) + (aq) K = ??? Report answer to 3 sig figs) 2.55x10^-9 Question 3 Calculate the molar solubility of Agl in 3.0M NH3 as shown below: Agl (s) + 2 NH3 (aq) A Ag(NH3)2 (aq) + (aq) (Report answer to 2 sig figs)

The acidity of a solution is measured by its pH. If (T*] represents the concentration of hydrogen ions (in moles/liter) in the solution, the pH is defined by pH = – log Ht || Suppose a solution has pH = 1.98. (a) Rewrite the logarithmic form of the equation into exponential form. indicates two way equivalence) Click for List - ] – log H+ pH O Click for List Click for List (b) Find Ht, the approximate concentration of hydrogen ions. (Select one) O [H*]= 0.2967 moles/liter [H']~0.5051 moles/liter O [H*]= 0.01047 moles/liter O [H*]~ -0.2967 moles/liter O [H*]=0.03177 moles/liter [H*]= -95.4993 moles/liter O [H*]=3.3708 moles/liter

y= 0.0624x+0.0123 R^2=0.9867

If the initial volume reading for the first titration was 0.16 mL and the final volume reading was 11.68 mL, what volume of iodine solution was used in your first titration (in mL)? Include the unit in your answer and two decimal places in your answer.