Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH', the Al³+(aq) ion forms a hydroxide complex ion, Al(OH)4 Calculate the concentration of free Al³+ ion when 1.01x102 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH ] is held constant (buffered at pH 12.50). For AI(OH)4, K=1.1×1033 [A1³]= M

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A buffer solution is 0.500 M in KF and 0.500 M in HF (KA = 3.5 × 10–4). What is the solution’s pH after 0.200 moles of solid CsOH is added to 3.00 L of buffer solution?  Assume that no volume change results from the addition of the CsOH. 3.09 4.46 3.82 3.22 3.57

A buffer solution made from HCN and KCN has a pH of 9.18. If pK, for HCN is 9.40 , [CN ] [HCN] what is the in the buffer? [CN ] [HCN]

For the aqueous [Ag (NH3)₂ complex K₁=1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0042M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. M x10 Times 10 to an exponent

What is the approximate concentration of free Fe2+ ion at equilibrium when 1.90×10-2 mol iron(II) nitrate is added to 1.00 L of solution that is 1.480 M in CN. For [Fe(CN)6l+, Kf= 1.0×1035. [Fe²*] = [ M

To a 0.10-M solution of Pb(NO3)2 is added enough HF(g) to make [HF] = 0.10 M.(a) Does PbF2 precipitate from this solution? Show the calculations that support your conclusion.(b) What is the minimum pH at which PbF2 precipitates?