The activity coefficient (y) of a neutral molecule is typically approximated as 1.00; however, a more acc be made by using the equation, log (y) = ku where k≈ 0.2 for organic molecules and is the ionic strength. Using the activity coefficients for H¹, the value of the given concentration quotient for acetic acid (HA = CH₂ CO₂H). You will need to look L coefficients for H and A in a table. concentration quotient [H][A] [HA] [H+][A] at μ = 0 M at μ = 0.1 M

The activity coefficient (y) of a neutral molecule is typically approximated as 1.00; however, a more acc be made by using the equation, log (y) = ku where k≈ 0.2 for organic molecules and is the ionic strength. Using the activity coefficients for H¹, the value of the given concentration quotient for acetic acid (HA = CH₂ CO₂H). You will need to look L coefficients for H and A in a table. concentration quotient [H][A] [HA] [H+][A] at μ = 0 M at μ = 0.1 M

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter10: Effect Of Electrolytes On Chemical Equilibria

Section: Chapter Questions

Problem 10.8QAP

See similar textbooks

Similar questions

12. The following quantities of salts were added to a volume of water to make 1 liter of solution: 1 x 10-2 moles NaCl 2 x 10-2 moles CaCl, 2 x 10-2 moles BaCl, (a) What is the ionic strength of the solution? (b) A small amount of phosphate salt is added to the same solution with negligible change in ionic strength. Given K = 10-7.2 for the reaction H,PO, = H+ + HPO,?- Calculate (H*][HPO,2-1/[H,PO,"), called °K, using the Güntelberg ap- proximation of the DeBye-Hückel law. (c) Calculate the "salting-out" coefficient, k,, for a nonelectrolyte in the same solution if its activity is 10-3 M and its concentration is 9.5 x 10 4 M.
Calculate the solubility of calcium carbonate water temperature of 5 °C; at that temperature, Ksp = 8.1 x 10^-9 for CaCO3, Ka = 2.8 x 10^-11 for HCO3-, and Kw = 2.0 x 10^-14.
Neglecting any effects caused by volume changes, what is the effect on the ionic strength by the addition of FeCl3 to (a) HCl? (b) NaOH? (c) AgNO₂?
Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2 (s). (a) If solid CaCl2 is added to this solution, will the amount of solid CaF2 at the bottom of the beaker increase, decrease or remain the same? (b) Will the concentration of Ca2+ ions in solution increase or decrease?
Complete the following solubility constant expression for Co (OH),. K - U sp =
Calculate the molar enthalpy of dissolution ΔsHm of the reaction.
The two salts BaCl2 and Ag2SO4 are both far more soluble in water than either BaSO4 (Ksp= 1.1 × 10-10) or AgCl (Ksp= 1.6 × 10-10) at 25°C. Suppose 50.0 mL of 0.040 M BaCl2(aq) is added to 50.0 mL of 0.020 M Ag2SO4(aq). Calculate the concentrations of SO42- (aq), Cl2(aq), Ba2+(aq), and Ag+(aq) that remain in solution at equilibrium.
Determine the distribution ratio (D) when K is 4.00 with a Ka of 2.10 x 10^-4 . The pH of the acid is 3.022
Consider the equilibrium shown. SrF, (s) = Sr + (aq) + 2F (aq) K = 2.60 x 10-9 Determine the concentrations of Sr+ and F in a saturated solution of SrF, in pure water (assume u = 0M). !3! [S?*1 = M [F] = Determine the concentrations of Sr+ and F in a saturated solution of SrF, in a solution with an ionic strength of 0.010 M. [Sr*] = [F] = M
If ΔHsoln < 0, will the conditions for solubility always be met?
Write the equilibrium constant expression for acetic acid, and calculate a K value and an apparent percent dissociation for each concentration + ICE tables for 0.10 M HC2H302 +0.010 M +0.0010 M. (ph for 0.10M is 3.3, pH for 0.010 M is 3.7, ph for0.0010 M is 4.4) HA(aq) = H+(aq) + A-(aq)
The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?