Question
In: Chemistry
1.) Why must the solution used to wash the precipitate be slightly acidified? 2.) If a...
1.) Why must the solution used to wash the precipitate be slightly acidified?
2.) If a student did not test the precipitate for presence of copper and some was included with the AgCl, will the final result (Ag %) be higher or lower than the true value? Why?
3.) If the precipitate was not dried completely before final weighing, will the final result (Ag %) be higher or lower than the true value? Why?
4.)Assuming the final concentration of chloride anion after the addition of HCl (precipitation step) was 0.1M, what is the remaining concentration of Ag+ in the solution? (pKsp for AgCl = 9.74)
5.)What is aqua regia? How is it different in composition from aqua fortis? Why might it be used instead of aqua fortis?
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
1- a. If ΔHsolution is slightly endothermic, a solution might form. Explain why b. If ΔHsolution...
1- a. If ΔHsolution is slightly endothermic, a solution might
form. Explain why
b. If ΔHsolution is highly endothermic, a solution can never form.
Explain why.
c. If ΔHsolution is exothermic, a solution will always form.
Explain why.
When ammonia is added to a solution that has Cu(OH)2(s) precipitate in it, the precipitate dissolves....
When ammonia is added to a solution that has Cu(OH)2(s)
precipitate in it, the precipitate dissolves. Use Le Châtelier’s
principle to explain this.
1) Explain why a primary standard, like KHP, must be used to standardize a sodiumhydroxide solution....
1) Explain why a primary standard, like KHP, must be used to
standardize a sodiumhydroxide solution. Define hygroscopic.
2) Determine the molarity of NaOH if 22.05 mL of NaOH is used to
titrate 0.3440 g of KHP.
3) What is the molarity of a monoprotic acid if 19.00 mL of
0.102 M NaOH is used to titrate 25.00 mL of the acid?
4) What is the Ka of an acid if the pH of the solution at the
half-point is...
How many moles of potassium chloride must be added to the solution to completely precipitate 1.18g...
How many moles of potassium chloride must be added to the
solution to completely precipitate 1.18g dissolved Ag?
Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the...
Potassium hydroxide is used to precipitate each of the cations
from their respective solution. Determine the minimum concentration
of KOH required for precipitation to begin in each case.
A) 1.8×10^−2 M CaCl2
B) 2.1×10^−3 M Fe(NO3)2
C)1.8×10^−3 M MgBr2
2(a). Describe how adding a solution of KOH to the original sulfide precipitate results in the...
2(a). Describe how adding a solution of KOH to the original
sulfide precipitate results in the separation of Sn4+ ion from the
other Group II cations.
2(b). Why wouldn’t a weak base, such as aqueous NH3 work just as
well as aqueous KOH in (a)?
2(a). Describe how adding a solution of KOH to the original sulfide precipitate results in the...
2(a). Describe how adding a solution of KOH to the original
sulfide precipitate results in the separation of Sn4+ ion from the
other Group II cations.
2(b). Why wouldn’t a weak base, such as aqueous NH3 work just as
well as aqueous KOH in (a)?
When a solution of Pb(NO3)2 and NaF are mixed, a precipitate is formed. The net ionic...
When a solution of Pb(NO3)2 and NaF are
mixed, a precipitate is formed. The net ionic equation is:
Pb+2(aq) + 2F-(aq) --> PbF2(s)
and the Ksp for this compound is 3.3 x 10-8.
What is the concentration of the ions remaining in solution?
To solve, first do the stoichiometry of the reaction to
determine the limiting reactant. Then, any excess reactant is
treated as a common ion when the net ionic reaction is reversed and
treated as a Ksp problem....
Extraction flowchart: Starting material: isopentyl acetate 1. Wash with deionized water 2. Wash with 5% aqueous...
Extraction flowchart:
Starting material: isopentyl acetate
1. Wash with deionized water
2. Wash with 5% aqueous sodium bicarbonate solution
3. Dry liquid water with sodium sulfate
A 20.00 mL unknown solution containing SO42- was treated with Ba(NO3)2 to precipitate 0.2613 g of...
A 20.00 mL unknown solution containing
SO42- was treated with
Ba(NO3)2 to precipitate 0.2613 g of
BaSO4. What was the molarity of
SO42- in the unknown?
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