Question
In: Chemistry
When a solution of potassium iodide is mixed with a solution of lead nitrate, a bright yellow solid precipitate forms.
When a solution of potassium iodide is mixed with a solution of lead nitrate, a bright yellow solid precipitate forms. Calculate the mass of the solid produced (molar mass = 461 g/mol) when starting with a solution containing 141.00 g of potassium iodide (molar mass = 166 g/mol), assuming that the reaction goes to completion.
Give your answer to three significant figures.
2KI (aq) + Pb(NO3)2 (aq) → PbI2 (s) + 2KNO3 (l)
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
When a solution of potassium iodide is mixed with a solution of lead nitrate, a bright...
When a solution of potassium iodide is mixed with a solution of
lead nitrate, a bright yellow solid precipitate forms.
Calculate the mass of the solid produced (molar mass = 461 g/mol)
when starting with a solution containing 163.20 g
of potassium iodide (molar mass = 166 g/mol), assuming that the
reaction goes to completion.
Give your answer to three significant figures.
2KI (aq) + Pb(NO3)2 (aq) → PbI2
(s) + 2KNO3 (l)
when a solution of lead(ii) nitrate is mixed with a solution of potassium chromate, a yellow...
when a solution of lead(ii) nitrate is mixed with a solution of
potassium chromate, a yellow precipitate forms according to the
equation: Pb(NO3)2 (aq) + K2CrO4 (aq) -> 2 KNO3 (aq) + PbCrO4.
Volume of 0.105 M lead(ii) nitrate react with 100.0 ml of 0.120 M
potassium chromate. What mass of PbCrO4 will be formed?
Part 1. A 13 ml sample of a 1.38 M potassium chloride solution is mixed with 52.9 ml of a 1.43 M lead(II) nitrate solution and a precipitate forms.
Part 1. A 13 ml sample of a 1.38 M potassium chloride solution is mixed with 52.9 ml of a 1.43 M lead(II) nitrate solution and a precipitate forms. The solid is collected, dried, and found to have a mass of 0.9 g. What is the percent yield? Enter to 2 decimal places.Part 2. What is the net ionic equation of barium hydroxide + hydrofluoric acid?
What precipitate forms when aqueous soulutions of Potassium Chloride, Sodium Sulfide, Iron(II) Nitrate are simultaneously mixed?...
What precipitate forms when aqueous soulutions of Potassium
Chloride, Sodium Sulfide, Iron(II) Nitrate are simultaneously
mixed? Show the molecular and net ionic equation for the
reaction.
10.00g lead (II) nitrate reacts with 10.00g sodium iodide in aqueous solution to produce solid lead...
10.00g lead (II) nitrate reacts with 10.00g sodium iodide in
aqueous solution to produce solid lead (II) iodide and aqueous
sodium nitrate. What mass of NaI remains?
I have the answer, and the process of using stoichiometry to
find it. I just do not understand the logic of the stoichiometry
and why you use it to find the NaI consumed. How is do you know it
is "consumed" based off of the stoichiometry you do?
Aqueous solutions of sodium sulfate and lead(II) nitrate are mixed and a white solid forms. What...
Aqueous solutions of sodium sulfate and lead(II) nitrate are
mixed and a white solid forms. What is the formula of the solid?
Click in the answer box to open the symbol palette.
Aqueous solutions of sodium sulfate and lead(II) nitrate are mixed and a white solid forms. What...
Aqueous solutions of sodium sulfate and lead(II) nitrate
are mixed and a white solid forms. What is the formula of the
solid?
A solution contains 0.13 M sodium iodide and 0.13 M potassium hydroxide. Solid silver nitrate is...
A solution contains 0.13 M sodium iodide and 0.13 M potassium
hydroxide. Solid silver nitrate is added slowly to this mixture.
What ionic compound precipitates first from the solution?
Ksp AgI = (1.5e-16)
Ksp AgOH = (2e-8)
Formula of first precipitate = _______
Hint: It is not necessary to do a calculation here.
If you react 3.1g of lead nitrate with 1.7g of potassium iodide, what is the theoretical...
If you react 3.1g of lead nitrate with 1.7g of potassium iodide,
what is the theoretical yield of the lead iodide precipitate?
When chlorine is bubbled through an ethanol solution of [NEt4]I a bright yellow precipitate results. Elemental...
When chlorine is bubbled through an ethanol solution of [NEt4]I
a bright yellow precipitate results. Elemental analysis of the
product reveals that it contains 3.51% nitrogen. Use this
information to elucidate the product of this reaction. Write a
balanced equation for the reaction and use VSEPR theory to predict
the structure of the solid. What is the oxidation state of iodine
at the end of the reaction?
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