Complete the following solubility constant expression for CaF2. K sp

What is the pH of the solution after the addition of 0.10 mol of NaOH to a 1.00 L buffer solution that is 0.78 MHCN and 0.14 M NACN [K,(HCN) = 4.9 x 10101? 8.75 O7.97 8.86 9.23 O 8.08

Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HA is 3.2 x 10⁹. Complete Parts 1-4 before submitting your answer. NEXT > 0.0015 mol of solid Ba(OH), is added to a 0.350 L buffer containing 0.110 M weak acid, HA, and 0.220 M of its conjugate base, A. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. H₂O(1) + A (aq) Before (mol) Change (mol) After (mol) HA(aq) + OH (aq) -

Ksp of Lead iodide (Pbl2) is 1.4 x 10 0. Calculate the molar solubility of this compound. 4.5 x 10-6M O 3.5 x 10-5M O2.5x 10-4M O 15 x 10-3M