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A solution consists of 0.020 mol.kg-1 KCl(aq) and 0.035 mol.kg-1 Ca(NO3)2(aq). For Cd(NO3)2(aq), calculate (i) the average activity coefficient, and (ii) the activities of Cd2+ and NO3
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- Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) ⇌ Ba2+ + 2IO3- Ksp = 1.57 \times× 10-9 at 25 deg C What is the activity coefficient of Ba2+? Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) ⇌ Ba2+ + 2IO3- Ksp = 1.57 × 10-9 at 25 deg C What is the activity coefficient of Ba2+?. 0.439 0.364 0.276 0.405Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(2IO3)^2(s) = Ba2+ + 2IO3^- Ksp= 1.57 × 10-9 at 25 deg C What is the activity coefficient of Ba2+? 0.276 0.439 0.405 0.364A. What is the solubility (in grams/L) of PbI2 in distilled water? B. What is the solubility of PbI2 (in grams/L) in 0.001 M NaNO3? For this part ignore any contribution to ionic strength from the PbI2. C. Take your results from B and calculate a new ionic strength including Na+, NO3-, Pb2+, and I-. Use this new ionic strength to determine new activity coefficients for Pb2+ and I- and calculate the new solubility. You may need to use the extended Debye-Huckel equation to do this.
- A 10mL solution contains dissolved PbCl2. There are 0.02575 moles Pb2+ and 0.0515 moles Cl-. What is the math expression for the activity coefficient of an ion according to Extended Debye-Hückel approach?if the mean ionic activity coefficient ,? ± of KIO4 in the saturated solution 0.85, what Ksp of KIO4? the information is above in the paper.Calculate the solubility at 25°C of BaCrO4 in pure water and in a 0.0050M BaCl2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. Ksp of BaCrO4 = 1.17 x 10^-10
- Calculate the gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate) 2 Fe is sought(Analyte), 1Fe2O3 is weighed (Precipitate)A student performed titrations of samples of borax at different temperatures to determine the KSP at each temperature. After graphing the 1/T (K-1 ) versus ln(KSP), the student obtained the trend line and R2 value. Use this information to answer the following questions: a. What is deltaH? b. Is this dissolution endothermic or exothermic? c. What is deltaS? d. Determine deltaG at 298K.A 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 gravimetric factor of the following. 2 Fe3O4 is sought(Analyte), 3 Fe2O3 is weighed (Precipitate)Part A: mean Activity coefficients (1) Examine the effect of changing the value of molality on the mean activity coefficients1 γ± [0.2mol, 0.02mol, 0.1mol ,0.03 0.01mol]for a given ionic compound [KBr]. Select 5 molalities in the mmol/kg range. Make a table of values of molality, ionic strength (I), and γ± . Make a plot of log γ± vs square root of ionic strength, I½ . (2) Study the effect of changing the charge number of ions on the mean activity coefficients γ± at a constant molality of 1 mmol/kg for several ionic compounds [KBr] you select. (3) What is the conclusion on effect of molality (ionic strength) and ionic charge numbers on γ± ?. Where is the deviation from ideal behavior is most likely? Explain.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).