Using the Debye-Huckel Limiting law, calculate the activity coefficient of sulfate ion with u = 0.223 in a MBSO4 solution. O 0.109 0.0.245 O 0.213 O 0.134
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- Calculating the activity coeffcient of a 0.004M aqueous solution of phenobarbital has beed brought up to an ionic strength of 0.09 by the addition of sodium chloride. Compare answers using the 2 Debye-Huckel equations. A (activity coefficient) = 0.51 Please show each stepusing the debye-huckel limiting law, calculate the activity coefficient of sulfate ion with u = 0.223 in an MGSO4 solutionUsing simple Debye-Huckel equation, estimate the following activity coefficients: SO42- at µ = 0.025
- 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?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.Given: 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.
- When methanol is dissolved n water a conducting solution results. Justify your answer.The mean activity coefficient for an aqueous 0.0020-molal solution of KCl at 25C is 0.951. How well does the Debye-Huckel limiting law, equation 8.50, predicts this coefficient? As an additional exercise, calculate using equations 8.52 and 8.53 where both a(K+) and a(Cl)=31010m and using equation 8.44.Use the thermodynamic data given below to compute the formation constant, Kf for [Zn(NH3)4]2+ in aqueous solution at 337.0 K. Species ΔfH0kJ/mol S0J/mol/K NH3(aq) -80.29 111.3 Zn2+(aq) -153.89 -112.1 [Zn(NH3)4]2+(aq) -533.5 301 Include 3 significant figures
- Consider a solution of that is 0.0020 M K2SO4. Calculate the ionic strength of the solution.Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.Would you expect calcite to be appreciably soluble in a solution whose pH is maintained at 4? A solution at pH? A solution containing 0.1 m H2S? where might you find such solutions in nature?