Question

will a precipitation form when 0.10L of 8.0x10^-3M Pb(N03)2 is added to 0.40L of 5.0x10^-3M Na2So4?

will a precipitation form when 0.10L of 8.0x10^-3M Pb(N03)2 is added to 0.40L of 5.0x10^-3M Na2So4?

Homework Answers

Answer #1

we have

0.10 L of 8.0 x 10^-3 M Pb(N03)2 and 0.40 L of 5.0 x 10^-3 M Na2So4

and after addition concentration of these solutions are

[Pb[NO3)2] = ( 0.10 L x 8.0 x 10^-3 M) / 0.50 L = 1.6 x 10^-3 M

[Na2SO4] =  ( 0.40 L x 5.0 x 10^-3 M) / 0.50 L = 4.0 x 10^-3 M

and the precipitation constan for these two solution is

Q = [Pb2+] [SO4^2-]

= 1.6 x 10^-3 M x  4.0 x 10^-3 M

Q = 6.4 x 10^-6

and

Ksp for the PbSO4 is 1.6 x 10^-8

therefore

Q > Ksp

and

precipitation will occur.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The following reactions worked: Pb(NO3)2 + KI, BaCl2 + Na2SO4 , NaOH + HCl , and...
The following reactions worked: Pb(NO3)2 + KI, BaCl2 + Na2SO4 , NaOH + HCl , and NaHCO3 + HCl. The following did not work: HCl + Na2SO4 and KCl + Na2SO4. Please classify into precipitation, neutralization, or gas-producing. Why do some work and the others don't?
A 1.555 g mixture of the solid salts Na2SO4 (MM=142.04) + Pb(NO3)2 (MM=331.21) forms an aqueous...
A 1.555 g mixture of the solid salts Na2SO4 (MM=142.04) + Pb(NO3)2 (MM=331.21) forms an aqueous solution with the precipitation of PbSO4 (MM=303.26). The precipitate was filtered and dried, and its mass was determined to be 0.68 g. The limiting reactant was determined to be Na2SO4. Determine the mass in g of Pb(NO3)2 in the original salt mixture. Na2SO4 (aq) + Pb(NO3)2 (aq) -> PbSO4 (s) + 2 NaNO3 (aq)
Will a precipitate form when 0.17 L of 2.1 x 10^-3 M Pb(NO3)2 is added to...
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?
You mix 6.0mL of 0.50M Na2SO4 with 8.0mL of 0.50M Pb(NO3)2 and collect and dry the...
You mix 6.0mL of 0.50M Na2SO4 with 8.0mL of 0.50M Pb(NO3)2 and collect and dry the PbSO4 precipitate. Calculate the following: a. Moles of Na2SO4 used b. Moles of Pb(NO3)2 used c. Moles of PbSO4 precipitate expected from Na2SO4 d. Moles of PbSO4 precipitate expected from Pb(NO3)2 e. What mass of PbSO4 do you expect to obtain from this reaction? f. If the actual mass of the precipitate you recover is 0.78g, what is the percent recovery of the precipitate?
Write balanced molecular and ionic equations for each. explain AgNO3+NaBr AgNO3+NaOH AgNO3+Na2CO3 Pb(NO3)2+NaBr Pb(NO3)2+Na2SO4 Pb(NO3)2+NaOH Pb(NO3)2+Na2CO3...
Write balanced molecular and ionic equations for each. explain AgNO3+NaBr AgNO3+NaOH AgNO3+Na2CO3 Pb(NO3)2+NaBr Pb(NO3)2+Na2SO4 Pb(NO3)2+NaOH Pb(NO3)2+Na2CO3 Ni(NO3)2+NaOH Ni(NO3)2+Na2CO3
(13) will a precipitate of Mg F2 form when 300 mL of 1.10*10^-3M MgCl2 solution is...
(13) will a precipitate of Mg F2 form when 300 mL of 1.10*10^-3M MgCl2 solution is added to 500, mL of 1.20 *10^-3M NaF? The Ksp of the precipitate ( if one forms) is 6.9*10^-9.
Consider the following precipitation reaction: 2 NaBr(aq) + Pb(NO3)2 (aq) → PbBr2 (s) + 2 KNO3...
Consider the following precipitation reaction: 2 NaBr(aq) + Pb(NO3)2 (aq) → PbBr2 (s) + 2 KNO3 (aq) Calculate the mass of NaBr(aq) in grams required to react with 58.1 g of Pb(NO3)2 (aq)
How many ml of 0.125 M Na2SO4 are needed to react with excess Pb(NO3)2 to obtain...
How many ml of 0.125 M Na2SO4 are needed to react with excess Pb(NO3)2 to obtain 0.750 grams of solid PbSO4?
Suppose we have a solution of lead nitrate, Pb(NO3)2(aq). A solution of NaCl(aq) is added slowly...
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
Why do solutions of NaNO3 abd Mg(NO3)2 behave differently when aqueous ammonium is added? A compound...
Why do solutions of NaNO3 abd Mg(NO3)2 behave differently when aqueous ammonium is added? A compound is known to be Na2CO3, Na2SO4, NaOH, NaCL, NaC2H3O2 or NaNO3-. When barium nitrate solution is added to a solution containing the unknown a white precipitation forms. No precipitate is onserved when a magnesium nitrate solution is added to a solution containing the unknown. What is the identity of the unknown compound? Explain reasoning
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT