The Ksp of PbCl2 is 1.7 x 10-5 at 25 C. What is concentration of Cl-...

Question

Question

The Ksp of PbCl2 is 1.7 x 10-5 at 25 C. What is concentration of Cl- in saturated solution of PbCl2?

Answer is 3.2 x 10-2

science chemistry

Answer 1

Answer #1

Consider dissolution of PbCl ₂ in water as PbCl _2(s) Pb ²⁺_(aq) + 2 Cl ^-_(aq)

The solubility product constant for above reaction is

K sp = [Pb ²⁺ ] [ Cl ^- ] ² = 1.7 x 10 ^-05

If S is the solubility of PbCl ₂ in mol / L , then [Pb ²⁺ ] = [ PbCl ₂ ] = S and [ Cl ^- ] = 2 x [ PbCl ₂ ] = 2 S.

Therefore, K sp = S x ( 2 S) ² = 1.7 x 10 ^-05

4 S ³ = 1.7 x 10 ^-05

S ³ = 1.7 x 10 ^-05/ 4

= 4.25 x 10 ^-06

S = 0.0162 mol / L

We have [ Cl ^- ] = 2 S = 2 x 0.0162 mol / L =3.2 x 10 ^-02 mol / L

Answer 2

Similar Homework Help Questions

For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5. calculate deltaG standard at...

For the Dissolving of PbCl2 in water Ksp is 1.7 x 10^-5. calculate deltaG standard at 25 degrees C. 12. For the dissolving of PbCl2 in water Ksp is 1.7 x 10-5. Calculate AG at 25°C. If [Pb2+] = .010M and [Cl-) = .01M what is AG?
For PbCl2, the Ksp = 1.7 x 10-5. What is the solubility of PbCl 2 in...

For PbCl2, the Ksp = 1.7 x 10-5. What is the solubility of PbCl 2 in 1.0 M NaCl? O a. 4.1 x 10-3 M O b. 2.6 x 10-2 M O c. 1.6 x 10-2 M O d. 1.7 x 10-4 M O e. 1.7 x 10-5 M
#5 Write the solubility product expression for PbCl2. Using the concentration for the Pb+2 and Cl-...

#5 Write the solubility product expression for PbCl2. Using the concentration for the Pb+2 and Cl- ions, solve for your experimental Ksp. #6 Using your book, find the theoretical Ksp for PbCl2 to determine your percent error A Solubility Product Constant Introduction: Many substances are very soluble in water. However, in this experiment you will be concerned with substances that are insoluble or only slightly soluble. Dynamic equilibrium is established when an excess of a slightly soluble substance is placed...

Calculate the molar solubility of PbCl2 in a 0.20 M NaCl solution. The Ksp of PbCl2 = 1.7 x...

Calculate the molar solubility of PbCl2 in a 0.20 M NaCl solution. The Ksp of PbCl2 = 1.7 x 10^–5. (hint: can any assumptions be made to simplify thiscalculation?)A. 4.1 x 10^–3 MB. 4.3 x 10^–4 MC. 8.5 x 10^–5 MD. 3.6 x 10^–6 ME. 1.6 x 10^–2 M
using activities, calculate the concentration of chloride ion concentration in a solution that contains 25 mM NaNO3, 75...

using activities, calculate the concentration of chloride ion concentration in a solution that contains 25 mM NaNO3, 75 mM NaBr and is saturated with lead (ll) chloride (PbCl2). The Ksp for PbCl2 is 1.7 x 10 -5. don't neglect activity. please show work :)
What is the concentration of Hg2* in a saturated solution of Hg Cl, if ksp =...

What is the concentration of Hg2* in a saturated solution of Hg Cl, if ksp = 8 x 10-187

The solubility of PbCl2 in a .10M NaCl solution is 1.7*10^-3 mol/L at 25 degrees C....

The solubility of PbCl2 in a .10M NaCl solution is 1.7*10^-3 mol/L at 25 degrees C. Calculate Ksp for PbCl2. (Note this is a "common ion effect" problem.) Please show all work!
Calculate the solubility of lead chloride, PbCl2 in units of grams per liter. Ksp(PbCl2) = 1.7×10-5....

Calculate the solubility of lead chloride, PbCl2 in units of grams per liter. Ksp(PbCl2) = 1.7×10-5. solubility = g/L
Ksp of AgCl = 1.77x10^-10 Ksp of PbCl2 = 1.70x10^-5 thanks! A solution contains 0.036 M...

Ksp of AgCl = 1.77x10^-10 Ksp of PbCl2 = 1.70x10^-5 thanks! A solution contains 0.036 M Ag+ and 0.032 M Pb2+. If you add CI", AgCl and PbCI, will begin to precipitate. What is the concentration of Cl" required, in molarity, when AgCl precipitation begins? concentration of Cl" = What is the concentration of Cl required, in molarity when AgCl precipitation is 99.99% complete? concentration of Cl" = What is the concentration of CI required, in molarity when PbCl, precipitation...

What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10−2 M in...

What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbCl2 from a solution that is 1.00×10−2 M in the chloride ion, Cl−? Ksp for lead(II) chloride is 1.17×10−5