Question

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?

Answer #1

In order to determine if a precipitate will form it is necessary
to determine if the reaction quotient Q exceeds the Ksp
value.

First write a net ionic equation for the reaction:

Pb(NO3)2(aq) + NaCl(aq) → PbCl2(s) + 2NaNO3(aq)

Net ionic equation:

Pb2+(aq) + 2Cl-(aq) →PbCl2(s)

Write this reaction in terms of Ksp:

Ksp = [Pb 2+] * [Cl-]^2

Use the dilution equation M1V1 = M2V2 to determine the initial
concentration of each species as mixed - that is before any
reaction has taken place: final volume = 700mL

For Pb(NO3)2:

0.0021 * 170 = M2*700

M of Pb(NO3)2 = 0.00051M

For NaCl :

0.0085*530 = M2*700

M of NaCl = 5/700 = 0.006436M

Pb2+ = 0.00051M

Cl-- = 0.006436M

Using these concentration values, calculate Q the reaction
quotient:

Q = [Pb2+] * [Cl-] ^2

Q = 0.00051 * (0.006436)^2

Q = 2.11*10^-8

Now compare this to Ksp for PbCl2= 1.6 x 10^-5

Q > Ksp - Therefore a precipitate would form.

Hence ,in our case precipitate will not form

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)

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)

Will a precipitate form if 0.0200 M Pb(NO3)2(aq) is mixed with
0.0250 M NaBr(aq)?
Reaction equation:
Pb(NO3)2(aq) + 2 NaBr(aq) → PbBr2(s) + 2 NaNO3(aq) Ksp of PbBr2
= 4.67 × 10^–6

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.

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

1A.If 14.0 mL of 0.10 M Ba(NO3)2
are added to 48.0 mL of 0.17 M
Na2CO3, will BaCO3
precipitate?
A.BaCO3 will precipitate.
B. BaCO3 will not
precipitate.
Calculate Q. ______________
1B The molar solubility of MnCO3 is 4.2 ?
10-6M. What is Ksp for this
compound?

Calculate the volume, in mL, of 0.230 M
Pb(NO3)2 that must be added to completely
react with 34.8 mL of 0.417 M NaCl.
Pb(NO3)2 (aq) + 2NaCl (aq) ->
PbCl2 (s) + 2NaNO3 (aq)

Will a precipitate form if 100.0 mL of 2.5 x 10-3 M
Cd(NO3)2 and 75.0 mL of 0.0500 M NaOH are
mixed at 25o C? (Yes or No) Calculate the concentration
of cadmiun ion in solution at equilibrium after the two solutions
are mixed. (Ksp is 7.2 x 10-15 for
Cd(OH)2 at 25o C) Please show all work.

Which of the following solutions
will form a precipitate when added to Ba(NO3)2?
KOH, NaC2H3O2, KNO3, NaI, or MgSO4

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