mosm/L 0.9 gms NaCl + pure water 100 mLs total

Consider the reaction of a 20.0 mL of 0.220 M C5H5NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.217 M CSOH. Write the net ionic equation for the reaction that takes place. Be sure to include the proper phases for all species within the reaction.

STATES OF MATTER Applying like dissolves like HO- solute : 0: || HOC-CH- OH I I OH OH I -CH₂-CH-CH-CH-CH-C-H : 0: || CH₂-C-OH | OH : 0: || NH,−C–NH, I OH : 0: || H H Which is the better solvent? :0: || CH₂ C- H 1 H-C CH₂OH Q2 CH, OH H-C .C II H H H 1 - CH₂ CH₂(CH₂), CH₂ CIH H H | C-H H : 0: || C-C-OH H 3/5

1. If Mg(OH)2 has a Ksp of 7.0 × 10–6, then what is the solubility of Mg(OH)2 in pure water?  Give your answer in units of g/L.  Express the answer to 4 significant digits and do not use scientific notation. *Use the Ksp given here.  Do not look up your own value. 2. 200.0 mL of 0.005 M Na2CO3 are added to 200.0 mL of 0.002 M MgCl2. Does a precipitate form? [Ksp(MgCO3) = 6.82 × 10–6]   Question 2 options:   No, because Q = Ksp.   Yes, because Q > Ksp.   No, because Q < Ksp.   No, because Q > Ksp.   Yes, because Q < Ksp. 3.In order for a precipitate of PbBr2 to form, what is the minimum concentration of Br- that must be present in a solution of 0.00050 M Pb(NO3)2.   The Ksp of PbBr2 is 2.20 × 10–6.