What is the concentration of Ca2+ that can be found in a saturated solution of CaF2 (s) at 25 °C ? Note: At 25 °C, Ksp of CaF2 (s) = 6.5 x 10-6 O 9.8 x 10-2 M 1.8 x 10-3 M 1.2 x 10-2 M 2.6 x 10-3 M

1. What is the equilibrium constant expression for the following reaction? (Pay careful attention to the phase indicators!) 2 HCl (g) + Mg(OH)2 (s) ? MgCl2 (aq) + 2 H2O (l)

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The value of Kh for methylamine, CH2NH,, is 4.20×10-4. Write the equation for the reaction that goes with this equilibrium constant. +

The solubility product for silver chloride is 1.6 x 10−10. What is the molar solubility of silver chloride in a 6.5 x 10−3 M AgNO3 aqueous solution at 298 K? Group of answer choices 6.5 x 10−3 M 2.5 x 10−8 M 1.3 x 10−5 M 4.8 x 10−4 M 2.8 x 10−20 M

The equilibrium constant, Keq, for the reaction: 2 NOCl(g) -> 2NO(g) + Cl2(g) is 2.4 x 10-7 (no units). What is the Keq for the reaction 1/3 Cl2(g) + 2/3 NO (g) -> 2/3 NOCl(g)

Don

II. GENERAL INSTRUCTIONS Read and analyze carefully each problem. Show your complete solution. 1. At 500 K, the following concentrations were measured: [N2] =3.0 x 102 M [Hz] = 3.7 x 102 M, (NH3) = 16 x 10-2² M 2NH3(g) N2(g) + 3H2(g) a What is the equilibrium constant expression? b. What is the equilibrium constant? 2 N2(g) + 3H2(g) 2NH3(g) At 375°C, the equilibrium constant of the reaction is 2 79 x 10-5 a. What is Kp? b. What is the partial pressure of NHS if the partial pressures of H₂ and Nz are 1.24 atm and 2.17 atm, respectively? 3. Consider the following reaction where Kc = 3900 at 2000 K 2SO2 (g) + O2(g) = 250³(g) 4 a Write the equilibrium constant expression

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5. Calculate the solubility (g/L) for silver sulfate, Ag2SO4 in 0.250 M AgBr. Ksp = 1.5 x 10s %3D