Question

Calculate the molar solubility of Ca(IO_{3})_{2}
in each solution below. The *K*_{sp} of calcium
iodate is

7.1

×

10^{−7}.

(a) 0.070 *M* Ca(NO_{3})_{2}

(b) 0.070 *M* NaIO_{3}

Answer #1

The species lanthanum iodate, La(IO3)3, has a Ksp = 6.12e-12.
Calculate the molar solubility of a saturated solution of the
sparingly soluble salt in the following solutions. Note that the
iodate anion bears a one minus charge and note any assumptions made
in simplifying algebraic expressions. a. in neutral pure water b.
in 0.0380 M La(NO3)3 c. in 0.0380 M NaIO3 (The answers are 6.9e-4
in neutral pure water, 1.81e-4 in 0.0380M La(NO3)3, and 1.12e-7 in
0.0380M NaIO3 but i...

The Ksp of chromium (III) iodate, Cr(IO3)3, is 5.00 × 10-6.
Calculate the molar solubility of this compound.

Calculate the molar solubility of Ba(IO3)2 in a solution that is
also 0.0600 M in Ba(NO3)2. (Ksp (Ba(IO3)2) = 1.57 x 10-9 )

If calcium iodate, Ca(IO3)2, is dissolved in a calcium nitrate
solution, instead of DI water, does the equilibrium concentration
of iodate ions:
a. increase, b. decrease, or remain the same?

What is the molar solubility of La(IO3)3 in a 0.830 M solution
of Mg(IO3)2? The Ksp for La(IO3)3 = 7.50 10-12

A student followed the procedure of this experiment to determine
the Ksp of zinc(II) iodate, Zn(IO3)2. Solutions of Zn(NO3)2 of
known concentrations were titrated with 0.200 M KIO3 solutions to
the first appearance of a white precipitate. For each of the
zinc(II) nitrate solution concentrations below, calculate the
expected concentration of iodate that would be required to initiate
precipitation of zinc(II) iodate. Show all calculations. (Assume
that Ksp = 3.9 x 10-6 at 25oC for zinc(II) iodate). a) 0.100 M...

Part I: Calculate the concentration of IO3– in a 9.05 mM
Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is
2.5 × 10-13. Assume that Pb(IO3)2 is a negligible source of Pb2
compared to Pb(NO3)2.
Part II: A different solution contains dissolved NaIO3. What is
the concentration of NaIO3 if adding excess Pb(IO3)2(s) produces
[Pb2 ] = 3.80 × 10-6 M?
Please explain thoroughly. I am SO confused!! Thank you SO much
in advance!

Question
Molar Solubility and solubility Product of Calcium
Hydroxide:
1. Volume of Saturated Ca(OH)2 solution (mL) = 25.0 mL
2. Concentration of Standardized HCL solution (mol/L) = 0.05
mol/L
3. Buret reading, initial (mL) = 50.0 mL
4. Buret reading, final (mL) = 32.5 mL
5. Volume of HCL added (mL) = 17.5 mL
6. Moles of HCL added (mol) = (concentration of HCl)(Volume of
HCl) = (0.05)(19.1) = 0.875 mol.
7.Moles of OH- in saturated solution (mol)=8.75x10^-4
8.the [OH-]...

Titrating 30.00 mL of a saturated calcium iodate solution
requires 28.91 mL of a 0.092 M solution of Na2S2O3 according to the
equation
IO3 – + 6S2O3 2– + 6H+ → I– + 2S3O6 2– + 3H2O
Calculate Ksp for Ca(IO3)2
a. 7.14 × 10–8
b. 6.97 × 10–4
c. 2.79 × 10–3
d. 1.61 × 10–6
e. none of these
I have the answer it is (D), But i would like a detailed
solution on how to solve the...

calculate the molar solubility of Ag2SO4 in each solution below.
(the ksp of silver sulfate is 1.5x10^-5)
a.0.34M AgNO3
b.0.34M Na2SO4

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