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Consider a saturated solution of calcium fluoride in 0.039 M potassium nitrate. Complete the following tasks, and then answer the question.
a) Write the chemical equation corresponding to Ksp.
b) Write the defining expression for the thermodynamic solubility product constant, Kspo.
c) Write the defining expression for the conditional solubility product constant, Ksp'.
d) For the Ca2+ and F- ions, write the mathematical relations defining activity of each ion in terms of its concentration and activity coefficient.
e) Based on your answers above, derive a relationship for Ksp' in terms of Kspo and activity coefficients, and calculate the value of Ksp', given that Kspo = 3.9 x 10-11. (Note: Compute the activity coefficient for each ion using the Debye-Huckel equation. You can disregard the contribution of the dissolved CaF2 to the overall ionic strength. Also disregard the formation of any HF in the equilibrium solution.)
72.0 mL of a 1.60 M solution is diluted to a volume of 268 mL. A 134-mL portion of that solution is diluted using 139 mL of water.
Calculate the equilibrium constant at 0c and at 50c(assuming enthalpies of formation are independent of temp)
What is the pH of the solution when 50 grams of Ca(OH)2 was added to 1 liter of water? Ksp of Ca(OH)2 = 6.5 x 10^-6
Determine the pH of a solution prepared by adding 0.0500 mole of solid ammonium chloride to 100 mL of a 0.150-molar solution of ammonia.
A 1.784 gram sample containing an unknown amount of arsenic trichloride and the rest inerts was dissolved into a NaHCO3 and HCl aqueous solution.
The rule works particularly well for weakly interacting molecules, such as those of a noble gas, but not so well for water among other substances. Assuming the rule is exact, estimate the molar enthalpy of evaporation for Argon (in kJ/mol), whose ..
Classify each of the following solutions as acidic, basic, or neutral. Explain how you reached this conclusion.
The temperature of a sample of water increases from 21.9°C to 45.3°C as it absorbs 5669 J of heat. What is the mass of the sample.
Calculate the pH of the titration mixture after 10.0, 20.0 and 30.0 mL of base have been added. (the ka for acetic acid is 1.76 x 10^-5).
Choose all of the processes from below which describe changes which are independent of the path by which the change occurs. the elevation increase experienced by a traveller travelling from Grand Isle, LA to Denver, Colorado
Arrange these compounds in order of increasing boiling point and explain your reasoning. (assume similar mass) CH3OCH3 CH3CH2CH3 CH3CH2OH 2. Which of the following compounds would have the greater viscosity?
What is the pH when 100 mL of 0.1 M NH3 is titrated with 50 mL of 0.2 M HCl? pKa of NH4Br is 9.25.
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