1. Determine the following values for a 0.020 m (NH4)2CrO4 solution. Ionic strength, I (in molality) a. b. Activity coefficient, y+ (using Davies equation) c. Activity expression, a. d. Activity, a
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Q: 1. Determine the following values for a 0.020 m (NH4)½CrO4 solution. a. Ionic strength, I (in…
A: The ionization equation for (NH4)2CrO4 is, NH42CrO4⇔2NH4+ + CrO42- So, 0.020 m (NH4)2CrO4 solution…
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- How can I calculate the activity coefficient and the resulting activities of a mixture of 0.001M NaCl with 0.05 NaNO2 using Debye-Hückel approximation? Is the resulting activity coefficient only for one ion species or the whole salt?Using simple Debye-Huckel equation, estimate the following activity coefficients: SO42- at µ = 0.025Calculate the average activity (a±), the average activity coefficient (γ±) and the activity of the electrolyte (a2) for a solution Al2(SO4)3 0.01 m. Assume that the Debye-Hückel las is valid. Result: γ±= 0.0656; a±=0.00167; a2=1.31 10-14
- 3. To 20,00 ml of 0,1250 mol/l solution of silver nitrate – 25,00 ml of 0,1000 mol/l solution of potassium thiocyanate were added. Calculate pAg of this mixture. pKs(AgSCN) = 11,97 Express numerical result with an accuracy of: Х,ХXGiven: molality = 0.54, pH = 2.43, Using the given equation, estimate the mean activity coefficient of HCl using the given molality and pH. ?± = mean activity coefficient of H+ and Cl- ionsb = molality relative to the standard 1 molal bo.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.
- 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 0.405A 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 NO3A pH probe/meter uses the following equations: Ecell = L + 0.0592 log a1 = L - 0.0592 pH Where L = L1 + EAg/AgCI + Easy= constants L1 = - 0.0592 log a2 a1 = activity of analyte solution a2 = activity of internal solution Questions: How will measured pH value be affected vs “real” pH if the temperature of the sample is 30C when pH was measured? How will measured pH value be affected vs “real” pH if HCl in pH electrode, became 0.15M instead of 0.1M? How pH value will be affected vs “real” pH if the glass of the pH electrode is not fully hydrated? Please answer all questions and provide a brief explanation
- For an experiment, you made a solution that was 0.0100 M acetic acid and 0.1400 M NaCl. a. What is the ionic strength of the solution? b. Without accounting for activities, what is the pH of the solution? c. What are the activity coefficients of all of the relevant species in this system? d. Accounting for activities, what is the pH of the solution? e. What is the percent error incurred by not accounting for the activity coefficients? Please help with dAn equimolar solution of ammonium sulfate, sodium chloride, and magnesium nitrate has an ionic strength of 0.15M. What is molar concentration of the solution wiht respect to each solute? a. 0.010 b. 0.015 c. 0.020 d. 0.025A. 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.