Determine the molar solubility (S) of Ag, CO, in a buffered solution with a pH of 4.983 using the systematic treatment of equilibrium. K„(Ag,CO,) = 8.46 x 10-12, K(H,CO,) = 4.45 x 107; K2(H,CO, ) = 4.69 x 10. %D M.
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- Calculate the molar solubility of Ag2S in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. Ag2S: pKsp = 48.70H2S: Ka1 = 1.0 x 10-7 ; Ka2 = 1.2 x 10-15[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103Determine the molar solubility of MF2 in a solution containing 0.0952 M KF. Ksp MF2 = 1.71 × 10–6 0.0952 M 7.52 × 10–3 M 1.80 × 10–5 M 1.89 × 10–4 M 9.25 × 10–4 MWrite a balanced net ionic equation to show why the solubility of BaF2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). + + + K =
- The molar solubility of CuCO3 at 298K is 1.5811×10-5 M. Determine the Ksp of this salt.Consider the reaction Agl <-> Ag+ + I- What will happen to the solubility of the salt if the solvent is at pH 4.5? (It will increase, decrease, or not change?) What will happem to the solubility of the salt if Ag+ forms a complex with NH3 in the solution? (It will increase, decrease, or not change?)Write a balanced net ionic equation to show why the solubility of Ag3PO4 (s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Consider only the FIRST STEP in the reaction with strong acid. Be sure to specify states such as (aq) or (s). + + + K =
- The solubility product constant of silver arsenate is 1.0x10-23 (ksp) the molar slubiility of Ag3AsO4 is :Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.Calculate the molar solubility of AgI in a 2.5 M NH3 solution if the Ksp for AgI is 8.5 x 10-17 and the Kf for [Ag(NH3)2]+ is 1.6 x 107.
- Determine the molar solubility of AgSCN in a solution maintained at pH 11.00 and where the concentration of free ammonia is 0.100 M. AgSCN: Ksp = 1.1 x 10-12HSCN: pKa = 4.0[Ag(NH3)2]+: Kf1 = 2.04 x 103 ; Kf2 = 8.13 x 103you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphidesfrom each other. What pH value must you set so that one of the twometals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l)is precipitated while the other is still in solution? Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20,Saturation concentration of H2S in water: 0.1 mol/lThe solubility product constant of mercury(I) iodide is 1.2 × 10-28 at 25°C. Estimate the concentration of Hg22+ and I2 in equilibrium with solid Hg2I2.