Complete the following solubility constant expression for CaF2. Ksp = ☐ == ✗

Many common weak bases are derivatives of NH3, where one or more of the hydrogen atoms have been replaced by another substituent. Such reactions can be generically symbolized as NX3(aq) + H₂O(1) HNX3+ (aq) + OH- (aq) where NX3 is the base and HNX3 is the conjugate acid. The equilibrium-constant expression for this reaction is Kb = [HNX,'][OH ] [NX3] where K is the base ionization constant. The extent of ionization, and thus the strength of the base, increases as the value of K₁, increases. K and K are related through the equation K₂ x Kb = Kw As the strength of an acid increases, its K₂ value increase and the strength of the conjugate base decreases (smaller K₁, value). If Kb for NX3 is 2.0x10-6, what is the percent ionization of a 0.325 M aqueous solution of NX3? Express your answer numerically to three significant figures. ► View Available Hint(s) percent ionization = 27 Submit Previous Answers Request Answer * Incorrect; Try Again; 4 attempts remaining Part C ΠΙΑΣΦ If K₁, for NX3 is…

Enter the solubility expression for Mg3(PO4)₂(s). Ksp =

A 3.20 L solution of 1.25 x 10³ M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 x 10¹¹ M NaCl. (a) Calculate Qc for the dissolution of PbCl₂. (b) No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated