Calculate the molar solubility of Hg2Br2 in 0.075 M NaBr, ignoring the effects of ionic strength.
Solubility of Hg2Br2 = [xxx] M
Calculate the molar solubility of Hg2Br2 in 0.075 M NaBr, ignoring the effects of ionic strength....
What is the solubility of Ag3PO4 (s) in pure water given Ksp = 1.8x 10^-18? Ignoring activity and effects of ionic strength, calculate the solubility of Ag3PO4 (s) in 0.1 M H3PO4. '
The Ksp for Hg2Br2 is
1.2 ? 10-18. Calculate [ Hg22+ ]
in saturated solutions of Hg2Br2 in
0.001 M KBr.
Hints:
(1) calculate ionic strength and the mean ionic activity
coefficient.
(2) calculate m+ from ksp and mean ionic activity
coefficient.
mz logy, = -0.509|242. 11
Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.
3. (a) Calculate the activity of SO42- whose concentration is 0.01M. Assume an ionic strength, for the solution, of 0.03 M. (b) Calculate the ionic strength of a solution that is 0.02M in NaBr and 0.01M in Na2SO4.
IN Calculate the ionic strength of 0.0092 M NaOH. М Calculate the ionic strength of 0.00034 M La(I0). Assume complete dissociation at this low concentration and no hydrolysis reaction to form LaOH2+
Calculate the ionic strength of 0.0078 M NaOH Calculate the ionic strength of 0.00049 M La(IO,),. Assume complete dissociation at this low concentration and no hydrolysis reaction to form LaOH2+. М
Calculate the molar solubility of La(IO)s in 0.050 M NalOs by taking into account the activity coefficients of the ions involved. Utilize for the activity coefficients: Where Iz is the ionic strength: CiZi With appropriate summation over all ions, ci being the molar concentration of the i'th ion and zi being its charge. Explain why you either ignore or take into account the additional ions from dissolution of La(I03)3. If you make any approximations, check whether they are justified.
Calculate the solubility (in M) of lead(II) bromide, PbBr2(s), in a 0.250 M NaBr solution if Ksp = 4.60 × 10–6.
Calculate the solubility (in M) of lead(II) bromide, PbBr2(s), in a 0.150 M NaBr solution if Ksp = 4.60 × 10–6.
Calculate the ionic strength of a solution that is a. 0.040 Min FeSO4. Ionic strength = b. 0.40 M in (NH4), Cr 04. Ionic strength = c. 0.40 Min FeCl2 and 0.40 M in FeCl2. Ionic strength = d. 0.040 M in La (NO3)2 and 0.050 M in Fe(NO3)2- Ionic strength =