Question

A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10) A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)

Answer #1

A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is
added to the solution, what is [Ag+] when PbCl2 begins to
precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)

A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is
added slowly until the second solid compound just begins to
precipitate. What is the concentration of Au+ ions at this point?
Ksp for AgCl = 1.8 x 10-10 and for AuCl is
2.0 x 10-13

If 550 mL of some Pb(NO3)2 solution is mixed with 400 mL of 6.70
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.

If 450 ml of some Pb(NO3)2 solution is mixed with 400 ml of 1.10
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.

Suppose we have a solution of lead nitrate, Pb(NO3)2(aq). A
solution of NaCl(aq) is added slowly until no further precipitation
occurs. The precipitate is collected by filtration, dried, and
weighed. A total of 13.93 g of PbCl2(s) is obtained from 200.0 mL
of the original solution. Calculate the molarity of the
Pb(NO3)2(aq) solution.
? M

If 100. mL of 0.025 M NaCl is mixed with 150. mL of 0.0015 M
Pb(NO3)2, will a precipitate form? (Ksp PbCl2 = 1.6 × 10−5) -
Answer: No- (Justify this answer) please show work

a) A 0.1500 M of AgNO3 solution was employed to
titrate a 25.00 mL of 0.1250 M of NaI and 0.2500 M NaCl. Given that
Ksp, AgI(s) = 8.3*10-17, and Ksp, AgCl(s) =
1.8*10-10, please calculate the concentration of
Ag+ ion after 6.00 mL of AgNO3 was added.
b) please calculate the pAg after 100.00 mL of AgNO3
was added

a) A 0.1500 M of AgNO3 solution was employed to titrate a 25.00
mL of 0.1250 M of NaI and 0.2500 M NaCl. Given that Ksp, AgI(s) =
8.3*10-17, and Ksp, AgCl(s) = 1.8*10-10, please calculate the
concentration of Ag+ ion after 6.00 mL of AgNO3 was added.
Answer: 1.2 x 10-15 M
b) please calculate the pAg after 100.00 mL of AgNO3 was
added
Answer: 1.35
I just want to see how they got that.

What is the I– concentration just as AgCl begins to precipitate
when 1.0 M AgNO3 is slowly added to a solution containing 0.0500 M
Cl– and 0.0500 M I– ? (Ksp values: AgCl = 1.8×10−10 ; AgI = 1×10−16
) (the halide ions could come from sodium salts...)

Will a precipitate form when 0.17 L of 2.1 x 10^-3 M Pb(NO3)2 is
added to 0.53 L of 8.5 x 10^-3 M NaCl?

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