a. At a certain temperature, the solubility of potassium iodate, KIO3, is 36.8 g/L. Calculate its solubility product constant for this temperature.
b. At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.185 mol/L. Calculate its solubility product constant for this temperature.
c. At a certain temperature, the solubility product constant* of
copper (II) iodate, Cu(IO3)2, is
4.08x10-8 M3. Calculate the solubility of
this compound for this temperature.
a)
Molar mass of KIO3,
MM = 1*MM(K) + 1*MM(I) + 3*MM(O)
= 1*39.1 + 1*126.9 + 3*16.0
= 214 g/mol
Molar mass of KIO3= 214 g/mol
s = 36.8 g/L
To covert it to mol/L, divide it by molar mass
s = 36.8 g/L / 214 g/mol
s = 0.172 mol/L
At equilibrium:
KIO3 <----> K+ + IO3-
s s
Ksp = [K+][IO3-]
Ksp = (s)*(s)
Ksp = 1(s)^2
Ksp = 1(0.172)^2
Ksp = 2.957*10^-2
Answer: 2.96*10^-2
b)
At equilibrium:
CdF2 <----> Cd2+ + 2 F-
s 2s
Ksp = [Cd2+][F-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(0.185)^3
Ksp = 2.533*10^-2
Answer: 2.53*10^-2
C)
At equilibrium:
Cu(IO3)2 <----> Cu2+ + 2 IO3-
s 2s
Ksp = [Cu2+][IO3-]^2
4.08*10^-8=(s)*(2s)^2
4.08*10^-8= 4(s)^3
s = 2.169*10^-3 M
Answer: 2.17*10^-3 M
a. At a certain temperature, the solubility of potassium iodate, KIO3, is 36.8 g/L. Calculate its...
At a certain temperature, the solubility of potassium iodate, KIO3, is 58.1 g/L. Calculate its solubility product constant for this temperature. Answer:
At a certain temperature* (probably not 25 °C), the solubility of silver sulfate, Ag2SO4, is 0.012 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small) Solubility product constants are very temperature sensitive. They are generally reported at 25°C. Not necessarily using this temperature allows me some flexibility. Answer: At a certain temperature, the solubility of potassium iodate, KIO3, is 36.1 g/L. Calculate its solubility product constant for this temperature. Answer: At a certain...
At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.093 mol/L. Calculate its solubility product constant for this temperature. Answer:
At a certain temperature, the solubility product constant* of copper (11) iodate, Cu(IO3)2, is 7.81x10-8 M. Calculate the solubility of this compound for this temperature. *Unless stated otherwise all solubility product constants are for water. Answer:
At a certain temperature, the solubility product constant of copper (II) iodate, Cu(O3)2, is 7.17X10 solubility of this compound for this temperature, M. Calculate the "Unless stated otherwise all solubility product constants are for water. Answer:
Question 4 At a certain temperature, the solubility product constant of copper in iodate, Cu(los), is 7.17x10M compound for this temperature. Calculate the solubility of this Not yet answered Marked out of 100 "Unless stated otherwise all solubility product constants are for water. F Flag question Answer: 5 Calculate the solubility of copper (1) iodate in 0.40 M copper (11) nitrate, Kupis 74x10M Not you *You should know that the Kp must refer to the copper iodate because all nitrate...
calculate molar solubility of Ca(IO3)2 in 0.0100M KIO3 Average lo concentration Subtract the concentration of IO on that came from the KIO3 from the average value of the total 10i concentration to get the iodate ion concentration that came from dissolved Cadonnz. Total ro, concentration 10, concentration from Kloo lo, concentration from dissolved Callobl M Calculate the molar solubility of Ca n 0.0100 M Klo, solution. Molar solubility mol/L
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
Calculate the solubility of copper (II) iodate in 0.48 M copper (II) nitrate. Ksp* is 7.4x10-8 M3. *You should know that the Ksp must refer to the copper iodate because all nitrate compounds are soluble and strong electrolytes! Answer: 1.92e-4 X
The solubility of Ce(IO3)3 in a 0.14-M KIO3 solution is 1.3 x 10-7 mol/L. Calculate Ksp for Ce(IO3)3 - Ksp = Submit Answer Try Another Version 10 item attempts remaining Which of the following two compounds is expected to be more soluble in acidic solution than in pure water? a. Agi AgNO2 b. Mn(NO3) Mn(CN)2 Submit Answer Try Another Version 10 item attempts remaining Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3x10-32) in a 0.16 M Na3PO4 solution. S...