8. Determine the mass (in g) of PbCl2 (Ksp, PbCl2 = 1.7x10^-5) that will dissolve in 0.450L of 0.375M Pb(NO3)2 solution.
8. Determine the mass (in g) of PbCl2 (Ksp, PbCl2 = 1.7x10^-5) that will dissolve in...
Ksp of PbCl2(s) = 1.7x10-5 Delta Gf of PbCl2 = -314KJ/mol Delta Gf of Pb2+ = -24.3KJ/mol Calculate the standard free energy change for the formation of Cl-
What is the minimum amount of water (in L) needed to dissolve 8.37 g of PbCl2? The Ksp is 0.000015. Also for reference, Pb = 207.19 g/mol and Cl = 35.453 g/mol.
At 25oC the Ksp for PbCl2 is 1.6 × 10–5 1) Calculate Q for the following: 125.0 mL of 0.0700 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oC 2) Calculate Q for the following: 125.0 mL of 0.0700 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25oC
What mass of PbCl2 can form from 0.235L of 0.110 M KCl solution if there is plenty of Pb(NO3)2 present? Molar mass of PbCl2 is 278.1g/mol Balanced reaction: 2KCl(aq) + Pb(NO3)2(aq) -> PbCl2(s) + 2KNO3(aq)
#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...
The Ksp for lead chloride (PbCl2) is 1.6 x 10-5. Calculate the solubility of lead chloride in each of the following. a. water Solubility = mol/L b. 0.16 M Pb(NO3)2 Solubility = mol/L c. 0.016 M NaCl Solubility = mol/L
Please help asap =) 2. Lead(II)chloride is insoluble in water Kap PbCn 1.7x10-) and silver chloride is very insoluble in water (Ksp Agci 1.8x10-10). The reactions when they go into solution are: AgCl(s) ←→ Ag+(aq) + Cl-(aq) PbCl2(s)艹Pb+2(aq) + 2 Cl-(aq) a. What are the expressions for the equilibrium constants, Kop for the above reactions? b. Explain why it is possible to dissolve more lead(I)chloride in solutions in which the concentration of the silver ion is present. c. Explain what...
Silver sulfate has Ksp = 9.0 × 10−5. What mass (g) of Ag2SO4 will dissolve per liter of water? Enter your answer to 1 decimal place.
Lead (II) chloride (PbCl2) has Ksp = 4.5x10-6 at 25oC. Calculate Qsp when [Pb(NO3)2] = 0.0020 M and [NaCl] = 0.0030 M.
A galvanic cell Pb│PbCl2│NaCl (0.0100M)││AgNO3 (0.500 M)│Ag is setup in the lab. Ksp PbCl2 = 87× 10-5. What is the concentration of Pb2+ in the Pb│PbCl2 half-cell? (10 pts.) Calculate Ecell. (20 pts.) E0 red=-0.13 Pb2+ + 2e- --> Pb E0 red= 0.80 Ag+ + e= -->Ag