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What is the solubility (in grams per liter) of lead(II) chromate, PbCrO4, in 0.315 M potassium chromate, K2CrO4? The Ksp for PbCrO4 is 1.8 x 10-14.


The solubility of silver sulfate, Ag2SO4, in water has been determined to be 8.0 g/L. What is the solubility in 0.36 M sodium sulfate, Na2SO4?


Magnesium sulfate, MgSO4, is added to 508 mL of 0.016 M sodium hydroxide, NaOH, until a precipitate just forms. How many grams of magnesium sulfate were added? Assume that the volume of the solution is not changed significantly by the addition of magnesium sulfate.


The formation constant Kf for the complex ion Zn(OH)42- is 2.8 x 1015. What is the concentration of zinc ion, Zn2+, in a solution that is initially 0.41 M in Zn(OH)42-?


What is the solubility of silver oxide, in a solution buffered at pH 10.65? The equilibrium is:

Ag2O(s) + H2O(l) 2Ag+(aq) + 2OH-(aq); Kc = 2.0 x 10-8.


What must be the concentration of chromate ion in order to precipitate strontium chromate, SrCrO4, from a solution that is 0.0018 M Sr2+. Ksp for strontium chromate is 3.5 x 10-5.


How many grams of sodium sulfate can be added to 259 mL of 0.0042 M barium chloride before a precipitate forms?


Calculate the molar solubility of silver iodide, AgI, in 2.2 M NH3.


Hydrazine, N2H4, is a base that ionizes to give N2H5+ and OH- (Kb = 1.7 x 10-6). You add magnesium sulfate to a hydrazine solution. Calculate the concentration of Mg2+ ion when magnesium hydroxide, Mg(OH)2, just begins to precipitate from 0.24 M N2H4. Ksp for Mg(OH)2 is 1.8 x 10-11.


A saturated solution of lead(II) iodate in pure water has an iodate-ion concentration of 8.0 x 10-5 M. What is the molar solubility of lead(II) iodate in a 0.31 M lead(II) nitrate solution at the same temperature?


A solution contains 0.00712 M calcium ion. A concentrated sodium fluoride solution is added to precipitate calcium fluoride (assume no volume change). At what concentration of F- does precipitate start to form?


What is the molar solubility of beryllium(II) hydroxide in a solution that is 0.30 M in NH3 and 0.25 M in NH4Cl? Be(OH)2 Ksp = 2.5 x 10-18.

From the following Ho and So values predict which of reactions I, II and III would be spontaneous at 300ºC.

H (kJ) S(J/K)
I >-5.0 -15
II -10.0 +20
III -5.0 -30

From the following Ho and So values predict which of reactions I, II and III would be spontaneous at 25ºC.

H (kJ)











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