calculate the ksp for Ca(IO3)2 if at equilibrium the concentration of IO3 ion is 2.35x10^-2 M.
calculate the ksp for Ca(IO3)2 if at equilibrium the concentration of IO3 ion is 2.35x10^-2 M.
Calculate the Ksp Ca(IO3)2 if at equilibrium the concentration of IO3- ion is 2.35 x 10-2 M. A) 8.3x10-4 B) 3.2x10-9 C) 5.7x10-2 D)1.2x10-10 E) 6.5x10-6
Calculate the concentration of IO3 in a 1.25 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 x 10-13. Assume that Pb(IO3), is a negligible source of Pb2+ compared to Pb(NO3)2. [103] = 2 x10-10 M A different solution contains dissolved NalO3. What is the concentration of NaIO, if adding excess Pb(IO3)2(s) produces a Pb2+ concentration of 7.00 x 10-6 M? concentration: -1.396 x10-5 M
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
Calculate the molar solubility of Ca(IO3)2 in each solution below. The Ksp of calcium iodate is 7.1*10^-7. a) 0.070 M Ca(NO3)2 b).070 M NaIO3
1) Use equilibrium ion concentration to calculate Ksp. The Pb2+ concentration in a saturated solution of lead bromide is measured and found to be 1.19×10-2 M. Use this information to calculate a Ksp value for lead bromide. Ksp =___________ 2) Use solubility to calculate Ksp. The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide. Ksp =______________
Calculate the concentration of IO3 in a 1.81 mM Pb(NO3)2 solution saturated with Pb(IO3)2 The Ksp of Pb(IO3)2 is 2.5 x 1013. Assume that Pb(IO3)2 is a negligible source of Pb2 compared to Pb(NO3)2 Number 10;]- М A different solution contains dissolved NalO3. What is the concentration of NalO3 if adding excess Pb(IO3)2(s) produces [Pb21] 5.10 x10 M? Number [Nalo,j= М
Calculate the concentration of 103 in a 9.27 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 x 10-13. Assume that Pb(IO3), is a negligible source of Pb2+ compared to Pb(NO3)2. [103] = M A different solution contains dissolved NalO3. What is the concentration of Naloz if adding excess Pb(IO3)2(s) produces a Pb2+ concentration of 5.20 x 10-6 M? concentration: M
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 =...
What is the molar solubility of Ca(IO3)2 in the presence of 0.06 M NaIO3? Ksp= 7.1 × 10-7 1. 1.8 × 10-9 2. 4.9 × 10-5 3. 2.0 × 10-4 4. 0.060
Solid Ca(IO3)2 is added to 0.0100 M KIO3. Titration shows that the concentration of iodate in the solution is now 0.0150 M IO3-. a) What portion of the iodate concentration was derived from the dissolving of calcium iodate? b) What is the concentration of calcium created by the dissolving solid?