[Ag (NH3)₂]* complex K₁ = 1.12 × 10² at 25 °C. Suppose equal volumes of 0.0042 M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Agion. For the aqueous Round your answer to 2 significant digits. M 0 x10 Times 10 to an exponent

Calculate the molar solubility of Ga(OH)3 (Kp 7.28 x 10 36) in a solution that is buffered at pH = 3.22.

5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.

2b

Chemistry

Complete the following solubility constant expression for ZnCO3. K = 0 sp X 0 9 3

Calculate the equilibrium concentration (in M) of PO43− that would be present in a mixture that is originally 0.015 M H3PO4 as well as 0.005 M NaH2PO4, given the following information:     H3PO4(aq)   ↔   H+(aq)   +   H2PO4−(aq)                   Ka1  =  1.5 x 10−5   H2PO4−(aq)   ↔   H+(aq)   +   HPO42−(aq)                 Ka2  =  2.5 x 10−7   HPO42−(aq)   ↔   H+(aq)   +   PO43−(aq)                    Ka3  =  3.5 x 10−9

HA, a weak acid, also forms the ion HA, in solution. The reaction is HA(aq) + A (aq) = HA, (aq) The weak acid has K, = 8.64 × 10-7 and the reaction has K = 3.80. Calculate the concentrations of A, H*, and HA, in a 1.00 M solution of HA. [A¯] = M [H*] = M [HA,] = M

32

Write the equilibrium expression for Kc for the reaction: Ag+(aq) + 2 NH3(aq) => Ag(NH3)2+(aq)