without converting HBr to moles, I get the concentration of Pb.
I need how many grams of Pb(NO3)2 so what Volume would I multiply the concentration of Pb to, so I end up with moles of Pb? Would it be multiplied by 0.750 L the same volume as the HBr?
I need the moles of Pb to multiply with...
Homework Statement
How many grams of Pb(NO3)2 must be added to 750.0 mL of 0.10 M HBr in order for PbBr2 to precipitate?
Ksp = 2.1*10^-6
Homework Equations
Ksp = [Pb][Br]^2
The Attempt at a Solution
For PbBr2 to precipitate, [Pb][Br]^2 must be greater than Ksp
0.750 L * 0.10 M...
Without using the Henderson–Hasselbalch equation, Can I do this?
also different Kb value.
The NN4CL will completely dissociate adding 0.35 NH4
NH4OH -> NH4+ + OH-
0.65-x. 0.35+x. . x
H2O + NH3 -> NH4+ + OH-
Kb =1.8 x 10^-5 = [NH4+][OH-]/[NH3]= (0.35+x)(x)/ 0.65-x
x =...
Homework Statement
What is the pH of a saturated Zn(OH)2 solution?
Ksp = 1.2 x 10^-17
Homework Equations
Ksp = [Zn2+] [OH-]^2
Zn(OH)2 <----> Zn2+ + 2OH-
pOH = -log [OH-]
pH = 14- pOH
The Attempt at a Solution
Ksp = 1.2 x 10^-17 = [Zn2+] [OH-]^2
Zn(OH)2 <---->...
Here is a problem I was working on but I do not have a solutions manual because Its an old textbook. I would just like someone to look over my work.
Homework Statement
Calculate the pH of a 0.67 M NaClO solution.
NaClO -> Na+ + ClO-
ClO- + H2O -> HCLO + OH-
Kw = 1.0*10^-14
Ka...
This isn't really homework, Its just a problem I'm trying to learn to solve. I'm not taking a chemistry course so I'm learning on my own.
Calculate the pH of a solution that is 0.65 M NH4OH and 0.35 M NH4Cl.
Well we can calulate the pOH = -log(OH-) and 14-pOH = pH
I guess I need the...
Two long straight wires are suspended vertically the wires are connected in series and a current from a battery is maintained in them. What happens to the wires? What happens if the battery is replaced by an a-c source.
This is a crude schematic of the circuit.
----|i|i----
|...