If 400 mL of some Pb(NO3)2 solution is mixed with 150 mL of 1.80 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.

The maximum concentration of Pb(NO3)2 is 2.68 M

Explanation:

Step 1: Data given

Volume of the Pb(NO3)2 solution = 400 mL = 0.400 L

Volume of the 0.01 M NaCl solution = 150 mL = 0.150 L

Ksp = 2.00 * 10^-5

Step 2: The equations

NaCl → Na+ + Cl -

PbCl2 → Pb^2+ + 2Cl-

Step 3: Calculate moles

Moles = volume * molarity

Moles NaCl = 0.150 L * 0.01 M

Moles NaCl = 0.0015 moles

Moles Cl- = 0.0015 moles

Step 4: Calculate total volume

Total volume = 400 + 150 = 550 mL

Step 5: Calculate [Cl-]

Molarity = moles / volume

Molarity Cl- = 0.0015 moles / 0.550 L

Molarity = 0.00273 M

Step 6: Calculate Ksp

Ksp = [Pb^2+]*[Cl-]²

2.00 * 10^-5 = [Pb^2+]* 0.00273²

[Pb^2+] = 2.68 M

[Pb^2+] = [Pb(NO3)2] = 2.68 M

The maximum concentration of Pb(NO3)2 is 2.68 M

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.