Question
In: Chemistry
A 77.0-mL sample of a 0.203 M lithium sulfate solution is mixed with 55.0 mL of...
A 77.0-mL sample of a 0.203 M lithium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this precipitation reaction occurs:
Li2SO4(aq) + Pb(NO3)2(aq) ⟶ 2 LiNO3(aq) + PbSO4(s)
The solid PbSO4 is collected, dried, and found to have a
mass of 4.71 g. Determine the percent yield. 1 mole
PbSO4 = 303.26 g
Group of answer choices
A.) 64.7 %
B.) 71.9 %
C. 98.5 %
D.) 80.0 %
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
35.40 mL of a 1.20 M solution of KCl is mixed with 55.0 ML of a...
35.40 mL of a 1.20 M solution of KCl is mixed with 55.0 ML of a
solution of Pb(NO3)2 with unknown Molarity. 2KCl(aq) + Pb(NO3)2(aq)
-->2KNO3(aq) + PbCl2(s). The solid PbCl2 weights 5.29g. If the
concerntration of lead (II) ions in solution after the complete
precipitation is 0.3564 M, what was the original concentration of
the lead(II) nitrate solution
A 17.0 mL sample of a 1.62 M potassium sulfate solution is mixed with 14.8 mL...
A 17.0 mL sample of a 1.62 M potassium sulfate solution is mixed
with 14.8 mL of a 0.890 M barium nitrate solution and this
precipitation reaction occurs:
K2SO4(aq)+Ba(NO3)2(aq)→BaSO4(s)+2KNO3(aq)
The solid BaSO4 is collected, dried, and found to have a mass of
2.48 g . Determine the limiting reactant, the theoretical yield,
and the percent yield.
Part A
Determine the limiting reactant.
Express your answer as a chemical formula.
K2SO4+Ba(NO3)2→BaSO4+2KNO3
SubmitMy AnswersGive
Up
Incorrect; Try Again; 5 attempts remaining
Part...
A 65.0 mL sample of a 0.122 M potassium sulfate solution is mixed with 34.0 mL...
A 65.0 mL sample of a 0.122 M potassium sulfate solution is
mixed with 34.0 mL of a 0.100 M lead (II) acetate solution and the
following precipitation reaction occurs:
K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s)
The solid PbSO4 is collected, dried, and found to have a mass of
0.994 g .
Determine the limiting reactant, the theoretical yield, and the
percent yield.
A 62.0 mL sample of a 0.122 M potassium sulfate solution is mixed with 36.5 mL...
A 62.0 mL sample of a 0.122 M potassium sulfate solution is
mixed with 36.5 mL of a 0.108 M lead(II) acetate solution and the
following precipitation reaction occurs:
K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s) The solid PbSO4 is
collected, dried, and found to have a mass of 0.992 g . Determine
the limiting reactant, the theoretical yield, and the percent
yield.
A 77.0 mL sample of 0.0400 M HNO3 is titrated with 0.0800 M CsOH solution. Calculate...
A 77.0 mL sample of 0.0400 M
HNO3 is titrated with 0.0800 M
CsOH solution. Calculate the pH after the following
volumes of base have been added.
(a) 10.0
mL
pH =
(b) 37.3
mL
pH =
(c) 38.5
mL
pH =
(d) 39.3
mL
pH =
(e) 65.1
mL
pH =
A solution prepared by mixing 55.0 mL of 0.260 M AgNO3 and 55.0 mL of 0.260...
A solution prepared by mixing 55.0 mL of 0.260 M AgNO3 and 55.0
mL of 0.260 M TlNO3 was titrated with 0.520 M NaBr in a cell
containing a silver indicator electrode and a reference electrode
of constant potential 0.175 V. The reference electrode is attached
to the positive terminal of the potentiometer, and the silver
electrode is attached to the negative terminal. The solubility
constant of TlBr is Ksp = 3.6 × 10–6 and the solubility constant of
AgBr...
A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is mixed with...
A 130.0 mL sample of a solution that is 0.0126 M in NiCl2 is
mixed with a 190.0 mL sample of a solution that is 0.400 M in
NH3.
-After the solution reaches
equilibrium, what concentration of Ni2+(aq) remains?
The value of Kf for
Ni(NH3)62+ is 2.0×108.
A 29.3-mL sample of a 1.84 M potassium chloride solution is mixed with 15.0 mL of...
A 29.3-mL sample of a 1.84 M potassium chloride solution is
mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this
precipitation reaction occurs:
2KCl(aq)+Pb(NO3)2(aq)→PbCl2(s)+2KNO3(aq)
What is the
1. Limiting reactant
2. Theoretical yield
3. percent yield
This seems like an easy question but for some reason I keep
getting hung up on these!
A 130.0 mL sample of a solution that is 2.7×10−3 M in AgNO3 is mixed with...
A 130.0 mL sample of a solution that is 2.7×10−3 M in
AgNO3 is mixed with a 230.0 mL sample of a solution that
is 0.14 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
A 130.0 mL sample of a solution that is 2.7×10−3 M in AgNO3 is mixed with...
A 130.0 mL sample of a solution that is 2.7×10−3 M in
AgNO3 is mixed with a 230.0 mL sample of a solution that
is 0.14 M in NaCN.
After the solution reaches equilibrium, what concentration of
Ag+(aq) remains?
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- what were some of Ida B Wells significant contributions to the civil rights movement?
- In 2007, there were many people in Sri Lanka who have an opinion that the government...
- Example #2: Write the following set of four linear equations with 4 unknowns x1, x2, x3,...
- "In the digital age, our personal and collective privacy is threatened like it never has been...
- when i type those python code below, i got True, but when i type not a...
- Assume sales for Peach Street Industries are expected to increase by 8.00% from 2015 to 2016....
- Merrimac Manufacturing has always purchased a certain component part from a supplier on the East Coast...
ADVERTISEMENT