Question
In: Chemistry
A basic solution contains the iodide and phosphate ions that are to be separated via selective...
A basic solution contains the iodide and phosphate ions that are to be separated via selective precipitation. The I– concentration, which is 7.80×10-5 M, is 10,000 times less than that of the PO43– ion at 0.780 M . A solution containing the silver(I) ion is slowly added. Answer the questions below.Ksp of AgI is 8.30×10-17 and of Ag3PO4, 8.90×10-17. Calculate the minimum Ag+ concentration required to cause precipitation of AgI. Calculate the minimum Ag+ concentration required to cause precipitation of Ag3PO4. I got the first part correct being 1.064x10^-12. the second part i got wrong, being 4.774x10^-14
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
A basic solution contains the iodide and phosphate ions that are to be separated via selective...
A basic solution contains the iodide and phosphate ions that are
to be separated via selective precipitation. The I– concentration,
which is 8.30×10^-5 M, is 10,000 times less than that of the PO43–
ion at 0.830 M . A solution containing the silver(I) ion is slowly
added. Answer the questions below. Ksp of AgI is 8.30×10^-17 and of
Ag3PO4, 8.90×10^-17. Calculate the minimum Ag+ concentration
required to cause precipitation of AgI.____mol/L Calculate the
minimum Ag+ concentration required to cause precipitation...
An unknown solution MAY contain the following ions:carbonate, sulfate, phosphate, sulfide, chloride iodide and bromide. a)...
An unknown solution MAY contain the following ions:carbonate,
sulfate, phosphate, sulfide, chloride iodide and bromide.
a) Upon adding Ba(NO3)2, a precipitate
formed. Which of the above ions could be present in this solution?
Write (full equation or net ionic) equations showing formation of
the precipitate(s).
b) After adding nitric acid (HNO3) to the above
precipitate, it completely dissolved, and bubbles were noted in the
process. When saturated ammonium molybdate was added, no yellow
precipitate was observed. Which of the ions...
A 20 cm3 aliquot of a 0.0577 mol dm-3 vanadium(V) solution wasreduced by iodide ions to...
A 20 cm3 aliquot of a 0.0577 mol dm-3
vanadium(V) solution wasreduced by iodide ions to
an unknown oxidation state (x). The liberated
iodine (I2) was titrated with 10.2 cm3 of a
0.0986 mol dm-3 Na2S2O3
solution.
Calculate the experimental value for the unknown oxidation state x
(to two decimal places).
Iodide ion is oxidized to hypoiodite ion, IO- , by hypochlorite ion, ClO-, in basic solution....
Iodide ion is oxidized to hypoiodite ion,
IO- , by hypochlorite ion, ClO-, in basic
solution. The equation is
The following initial rate experiments were run and, for each,
the initial rate of formation of IO- was determined.
Find the rate law and the value of the rate constant.
Initial concentrations initial rate
please explain with steps.
In basic solution hydrogen peroxide oxidizes chromite ions, Cr(OH)4- to chromate ions, CrO4^2-. The hydrogen peroxide...
In basic solution hydrogen peroxide oxidizes chromite ions,
Cr(OH)4- to chromate ions, CrO4^2-. The hydrogen peroxide is
reduced to hydroxide ions. Write and balance the net ionic equation
for this reaction. What is the sum of the reactant
coefficients?
Sodium phosphate is added to a solution that contains 0.0051 M aluminum nitrate and 0.014 M...
Sodium phosphate is added to a solution that contains 0.0051 M
aluminum nitrate and 0.014 M calcium chloride. The concentration of
the first ion to precipitate (either Al3+ or Ca2+) decreases as its
precipitate forms. What is the concentration of this ion when the
second ion begins to precipitate?
Sodium phosphate is added to a solution that contains 0.0099 M aluminum nitrate and 0.021 M...
Sodium phosphate is added to a solution that contains 0.0099 M
aluminum nitrate and 0.021 M calcium chloride. The concentration of
the first ion to precipitate (either Al3+ or Ca2+) decreases as its
precipitate forms. What is the concentration of this ion when the
second ion begins to precipitate? Hint: Note that well over 99% of
the first ion has precipitated before the second ion starts to
precipitate. Correct Answer: 2.613e-7 (I need an "EXPERT" to show
me how to...
Sodium phosphate is added to a solution that contains 0.0071 M aluminum nitrate and 0.016 M...
Sodium phosphate is added to a solution that contains 0.0071 M
aluminum nitrate and 0.016 M calcium chloride. The concentration of
the first ion to precipitate (either Al3+ or Ca2+) decreases as its
precipitate forms. What is the concentration of this ion when the
second ion begins to precipitate?
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.
2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M ammonium iodide. If 0.16...
2. A 1.00 liter solution contains 0.42 M ammonia and 0.32 M
ammonium iodide. If 0.16 moles of hydroiodic acid are added to this
system, indicate whether the following statements are true or
false. (Assume that the volume does not change upon the addition of
hydroiodic acid.)
A. The number of moles of NH3 will decrease.
B. The number of moles of NH4+ will increase.
C. The equilibrium concentration of H3O+ will increase.
D. The pH will increase.
E. The...
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