4) Using activity coefficients, calculate the concentration of Co" present in a 0.1 M solution of KNO, saturated with COCO:(s). Calculate the expected concentration without activity coefficients (using only K) and state which is larger. COCO K-1.0x10
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- Using activities, calculate the molar solubility of Mg(OH)2 (Ksp= 7.1E-12) in a sol'n that is 0.0333M of Na2SO4In this activity we considered KNO3 solutions in the range 1.0x10-1 from 1 than they are for the lower concentration KNO3 to 1.0x10-5 M. The Extended Debye-Hückel equation is a reasonable way to compute activity coefficients for μ ≤ 0.1 M. Suppose we have AgBr(s) dissolved in a 1.0 M solution of KNO3. At this ionic strength will the activity coefficients be closer to or further solutions?Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
- Find the concentration of I- in 0.05 M AgNO3 saturated with AgI. Include activity coeffcients in the solubility-product expression. The Ksp of AgI is 8.3x10-17. Refer to the table of activity coefficients at various ionic strengths as needed.For µ=0.1, the activity coefficient (gamma) of M2+ is 0.41 while gamma of X- is 0.75. Calculate how many micrograms of MX2 dissolve in 324 mL of 0.10 M NaX solution. The molar mass of MX2 is 201 g/mol, and its Ksp is 3.8 x 10-9. Note that NaX is a salt of X-, an ion that participates in the equilibrium that applies to the solubility of MX2. a. 110 µg b. 27 µg c. 9.7 µg d. 44 µg e. 1000 µgUsing an experimentally determined value (2.4×10−10) of Ksp, determine the value for the reaction quotient 'Q' if Ag2CrO4 will precipitate when 7.00 mL of 0.0040 M AgNO3 are added to 4.00 mL of 0.0024 M K2CrO4.
- Using activities,(a) Find the concentration of of hydroxide ion in 0.10 M NaClO 4 saturated with Mn(OH)2(Ksp = 1.6 x 10 –13 ).(b) Determine the pH of the solution at 25 ̊C if Kw is 1.0 x 10 –1calculate the ksp for PbBr2 if it's molar solubility is 2.14x10^-2 M at 25 degrees celsius. show workA solution of PbCl2 has 0.018 moles of Cl- and 0.0089 moles of Pb2+. Its Ksp = 2.88x10-6 (based on molarities), and its ionic strength = 0.027. a) What are the activity coefficients of Pb2+ and Cl-? b) Use activities of ions instead of molarities to calculate a value for the thermodynamic solubility product of the solution.
- Calculate the solubility of La(IO3)3 in a 0.03 M solution of Mg(ClO4)2 using (a) activities and (b) molar concentrations when its Ksp is 1.0x10^-11Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3 (Ksp = 1.36 × 10–7).(b) If the NiCO3 were a contaminant in a sample of CoCO3 (Ksp = 1.0 × 10–12), what mass of CoCO3 would have been lost? Keep in mind that both NiCO3 and CoCO3 dissolve in the same solution.-Please determine the ksp for Cu(OH)2. pH for solution was 5.25 Show ice box for chemical equation. please show all steps to solution clearly