The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K s p for each of the slightly soluble solids indicated: (a) TlCl : [ Tl + ] = 1.21 × 10 − 2 M , [ Cl − ] = 1.2 × 10 − 2 M (b) Ce ( IO 3 ) 4 : [ Ce 4 + ] = 1.8 × 10 − 4 M , [ IO 3 − ] = 2.6 × 10 − 13 M (c) Gd 2 ( SO 4 ) 3 : [ Gd 3 + ] = 0.132 M , [ SO 4 2 − ] = 0.198 M (d) Ag 2 SO 4 : [ Ag + ] = 2.40 × 10 − 2 M , [ SO 4 2 − ] = 2.05 × 10 − 2 M (e) BaSO 4 : [ Ba 2 + ] = 0.500 M , [ SO 4 2 − ] = 2.16 × 10 − 10 M
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate K s p for each of the slightly soluble solids indicated: (a) TlCl : [ Tl + ] = 1.21 × 10 − 2 M , [ Cl − ] = 1.2 × 10 − 2 M (b) Ce ( IO 3 ) 4 : [ Ce 4 + ] = 1.8 × 10 − 4 M , [ IO 3 − ] = 2.6 × 10 − 13 M (c) Gd 2 ( SO 4 ) 3 : [ Gd 3 + ] = 0.132 M , [ SO 4 2 − ] = 0.198 M (d) Ag 2 SO 4 : [ Ag + ] = 2.40 × 10 − 2 M , [ SO 4 2 − ] = 2.05 × 10 − 2 M (e) BaSO 4 : [ Ba 2 + ] = 0.500 M , [ SO 4 2 − ] = 2.16 × 10 − 10 M
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:
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A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN (in 0.10 M HNO3) solution with 4.0
mL of 0.0030 M Fe(NO3)3 solution, and 3.0 mL of 0.10 M HNO3 solution.
Based on your average Kf value, determine the equilibrium concentrations
of Fe 3+, SCN, and FeSCN2+ in the solution. You cannot apply a small x approximation.
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:(a) AgBr: [Ag+] = 5.7 × 10–7 M, [Br–] = 5.7 × 10–7 M(b) CaCO3: [Ca2+] = 5.3 × 10–3 M, [CO32−] = 9.0 × 10–7 M(c) PbF2: [Pb2+] = 2.1 × 10–3 M, [F–] = 4.2 × 10–3 M(d) Ag2CrO4: [Ag+] = 5.3 × 10–5 M, 3.2 × 10–3 M(e) InF3: [In3+] = 2.3 × 10–3 M, [F–] = 7.0 × 10–3 M
Potassium hydrogen phthalate (KHP) concentrations can be determined through titrating samples of KHP (a monoprotic acid) with
bases such as NaOH in the presence of an indicator such as phenolphthalein. The indicator is colorless in an acidic solution and
turns pink in an alkaline solution. Thus, we can establish an equilibrium for the phenolphthalein with the following reaction.
HIn + H,0 = In + H;0*
If the Hin species is "acid color" or colorless for the phenolphthalein, and the In species is "base color" or pink for this particular
indicator, what color will appear in a flask in which a 0.2993 gram sample of KHP is completely neutralized with an excess of NaOH?
A The flask will be colorless.
B The flask will be pink.
The flask will be white from KCI precipitation.
There is insufficient information to solve this problem.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell