Construct the expression for Ksp for solid A9CN in aqueous solution. AgCN(s) = Ag*(aq) + CN-(aq) 1 Based on your knowledge of how the solid will dissociate in aqueous solution, use the tiles to form the expression. Ksp

Determine the molar solubility for Cr(OH)₃ (Ksp = 6.3 × 10⁻³¹) in an aqueous solution that has a pH of 11.90 at 25 °C. Give an ice table

The solubility of silver chloride is 1.3 x 10-5 mol L-1. What is the Ksp for silver chloride at 25 °C?

Enter the solubility expression for Mg, (PO4)₂(s). Ksp =

At 15°C a saturated solution of Calcium fluoride (CaF2) is observed to contain 45.6 mg of CaF2 in 1.88 L of aqueous solution. Calculate Ksp for CaF2 at this temperature.

Given the equation Ag*(aq) + 2 NH, (aq) → [Ag(NH,),]*(aq) Kf = 2.00 x 107 determine the concentration of NH3(aq) that is required to dissolve 653 mg of AgCl(s) in 100.0 mL of solution. The Ksp of AgCl is 1.77 x 10-10. [NH,] =

Complete the following solubility constant expression for Ag2CrO4. Ksp = ☐ == ✗

Use this information to calculate K for BaSO. 4 The solubility of BaSO, in water at 25 °C is measured to be 0.0023 sp Round your answer to 2 significant digits.

A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq):             Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.

Zn(s)|Zn2+(aq) || Fe2+(aq, ) | Fe(s)  What would you change to increase the Ecell decrease Zn2+concentration increase Zn2+concentration decrease concentration of both ions decrease Fe2+concentration increase concentration of both ions