Predicting precipitationComplete the table below by deciding whether a precipitate forms whenaqueous solutions A and B are mixed. If a precipitate will form, enter itsempirical formula in the last column.Does aempiricalprecipitate formsolution Asolution Bformula ofwhen A and Bprecipitateare mixed?sodium chlorideammonium nitrateyesnozinc chlorideammonium sulfideyesnonickel(II) sulfateiron(II) chlorideyesno

Given : We have to tell that precipitate will form or not.

Complete the table below by deciding whether a precipitate forms w aqueous solutions A and B are mixed. If a precipitate will form, ent empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? sodium chloride ammonium nitrate yes no zinc chloride ammonium sulfide yes no iele blenid

Complete the table below by deciding whether a precipitate forms w aqueous solutions A and B are mixed. If a precipitate will form, ent empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? sodium chloride ammonium nitrate yes no zinc chloride ammonium sulfide yes no iele blenid

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 98AE: In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion...

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In the chapter discussion of precipitate formation, we ran the precipitation reaction to completion and then let some of the precipitate redissolve to get back to equilibrium. To see why, redo Example 15-6, where Initial Cocentration (mol/L) Equilibrium Concentration (mol)/L [Mg2+]0 = 3.75 103 [F]0 = 6.25 102 reactstoformMgF2ymol/Mg2+ [Mg2+] = 3.75 103 y [F] = 6.25 102 2y
Recommend a specific cation for the quantitative precipitation of carbonate ion andjustify your recommendations.
The solubility of Ag(I) in aqueous solutions containing dif-ferent concentrations of Cl is based on the following equilibria:Ag⁺(aq)+Cl⁻(aq)⇌AgCl(s) Kₛₚ=1.8X10⁻¹⁰ Ag⁺(aq)+2Cl⁻(aq)⇌AgCl₂⁻(s) K(f)=1.8X10⁻⁵ When solid AgCl is shaken with a solution containing Cl⁻, Ag(I)is present as both Ag⁺ and AgCl₂⁻. The solubility of AgCl is thesum of the concentrations of Ag and AgCl₂.(a) Show that [Ag⁺] in solution is given by[Ag⁺]=1.8X10⁻¹⁰/[Cl⁻]and that [AgCl₂⁻] in solution is given by [AgCl₂⁻](3.2X10⁻⁵)([Cl⁻] (b) Find the [Cl⁻] at which [Ag⁺][AgCl₂⁻].(c) Explain the shape of a plot of AgCl solubility vs. [Cl⁻].(d) Find the solubility of AgCl at the [Cl⁻] of part (b), which is the minimum solubility of AgCl in the presence of Cl
The solubility product constant for CaCO3 (s) in water is Ksp = [Ca+2] [CO3 -2] = 4.8 x 10^-9 Consider a 1.00 M solution of calcium chloride, in which you drop a piece of Dry Ice. Show that the minimum concentration (threshold amount) of carbonate ions necessary for a precipitate to appear is 4.8 x 10-9 M. Another way to think about this situation is to calculate the Q for the calcium chloride/Dry Ice solution and ask “will precipitation occur?”..
Some sulfuric acid is spilled on a lab bench. You can neutralizethe acid by sprinkling sodium bicarbonate on it and thenmopping up the resulting solution. The sodium bicarbonatereacts with sulfuric acid according to:2 NaHCO3(s) + H2SO4(aq)----->Na2SO4(aq) + 2 H2O(l)+ 2 CO2(g)Sodium bicarbonate is added until the fizzing due to the formationof CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled,what is the minimum mass of NaHCO3 that must be addedto the spill to neutralize the acid?
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…
In the deposition method, one of the conditions that must be met is…a. The precipitate has a high solubility or solubility productb. The precipitate formed must be quite difficult to dissolvec. The precipitate formed does not have to be quite pured. Free precipitate form
An aqueous solution contains Ag+, Pb2+, Cu+, and Tl+ with each ion at a concentration of 0.15M. The chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate. AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18
In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H2O, at 20−25∘C) OH− CO2−3 SO2−4 CrO2−4 C2O2−4 Mg2+ 0.00069 0.18 35.7 54.8 0.038Ca2+ 0.16 0.00066 0.205 13.2 0.00061Sr2+ 2.25 0.00034 0.135 0.106 0.005Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate.
(c) 1.0cm^3 0.25 moldm^-3 potassium chromate(VI), K2CrO4, is added as an indicator. At the end-point, all the silver chloride has been precipitated in the 52.5cm^3 solution. A slight excess of silver ions causes a red-brown precipitate of silver chromate(VI) to form. 2Ag + (aq) + CrO4 2- (aq) - - > Ag2CrO4 (s) (i) The solubility product of silver chloride is: Ksp = 2.0 ×10^-10 mol^2 dm^-6 Use this value to explain why [Ag+] = 1.41 × 10^-5 moldm^-3 at the end point.
Determine how the solubility of the following weak electrolytes is affected upon addition of excess reagent in aqueous solution. If the solubility is affected, write the overall chemical reaction and the balanced net ionic equation that occurs between the weak electrolyte and the reagent. If the reagent is not expected to affect the solubility, state that there is no reaction: a.) Excess NaSCN is added to a mixture of CoCO3 in water. b.) Excess NH3 is added to a mixture of BaSO4 in water. c.) Excess HClO4 is added to a mixture of PbO2 in water.
2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4