2. A solution may contain Ag+, Pb2+, and Hg22+. A white precipitate forms on the addition of 6 M HCI. The precipitate is partially soluble in hot water. The residue dissolves on addition of 6 M NH3. Which of the ions are present, which are absent, and which remain undetermined? State your reasoning. (The partial solubility of the precipitate in hot water implies that an ion is present, so you can report it as present.) Present Absent In doubt Reasoning:
Q: 16. A solution may contain Ag*, Pb2+, and Hg22+, A white precipitate is formed after the addition on…
A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: 2. 6 M HCI is added to a solution of Ag*, Cu²+, Fe3•. A white precipitate forms. Predict which ions…
A: The ions present in the solution are : Ag+, Cu2+, Fe3+. When a 6M HCl is added to the solution and…
Q: Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of…
A: Solubility product : For a sparingly soluble salt, It is defined as the product of solubility…
Q: Above what Fe2+ concentration will Fe(OH)2 precipitate from a buffer solution that has a pH of 9.31?…
A: Ionic product of a salt solution is the product of the ion in the solution at a given concentration…
Q: A solution containing a mixture of metal cations was treated as outlined. 1. Dilute HCl was added…
A: Group analysis are specific test performed to detect the presence of the certain group elements.
Q: Cadmium cations Cd^2+ form a soluble metal complex ion [Cd(NH3)4]^2+ upon the addition of ammonia.…
A:
Q: A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final…
A:
Q: Write all the reactions involved in the Mohr's method, if an unknown solution containing chloride…
A: Introduction Mohr's method is used to determine the chloride ion concentration with the help of…
Q: The following experimental process steps have been made to determine the hardness of water.…
A: Given: Volume of water = 100 mL Concentration of EDTA = 0.0086 M Volume of EDTA = 11.44 mL molar…
Q: D. Preparation of a Buffer from a Solution of a Weak Acid So far in this experiment the buffers that…
A: Pka=pH So B-=HB
Q: The Ksp of silver bromide at 25°C (298 K) is 5.0 x 1013. Write the solubility expression for this…
A: Given : Ksp = 5.0 X 10-13
Q: The cation M 2+ reacts with NH 3 to form a series of complex ions as follows: M2+ + NH3M(NH3)2+ K1…
A:
Q: 8. Suppose sufficient ammonia (NH3) was added to a solution containing 0.010 M nickel nitrate…
A: We have the value for formation constant, Kf in the question. So we can use the equation for Kf to…
Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…
A: Given: Volume of buffer solution = 100 mL pH of buffer solution = 9.02 Concentration of acid and…
Q: Consider a flask containing 50.00 ml. of 0.0426 M trimethylamine ((CH,),NH,). This is titrated with…
A:
Q: What is NOT recommended for precipitation of crystal deposits: precipitation in presence of…
A: The correct option is option c.
Q: gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds…
A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
Q: Write a balanced net ionic equation to show why the solubility of PbCO3(s) increases in the presence…
A: We have to write a balanced net ionic equation to show why the Solubility of Pb(CO3) increases in…
Q: Quantitative analysis of Cl⁻ ion is often performed by atitration with silver nitrate, using…
A: Quantitative analysis is the determination of the absolute or relative abundance of one particular…
Q: A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final…
A:
Q: 5.31e-08 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 9.14e-08 g of…
A:
Q: The substance to be analyzed - is white, highly soluble in water salt. When interacting with…
A: There are several chemical tests are reported in literature for the determination of different metal…
Q: Why homogenously formed precipitates are better suited for analysis than a precipitate formed by…
A: The gravimetric method is inherently more accurate than the volumetric method because the…
Q: What is the purpose of adding concentrated ammonia in the elimination test for cations? a. to…
A: Here we have to choose correct option about above qualitative analysis-
Q: Solid KSCN was added to a(2.20x10^0) M Co2+ solution so that it was also initially (2.20x10^0) M…
A:
Q: A student performing this lab experiment receives his unknown solution that may contain ( Ba, Ca,…
A: In the given steps, initially barium chloride reacts with potassium chromate which results in the…
Q: Given that the average concentration of calcium ion in natural waters is 3.8x10⁻⁴ M, and that the…
A:
Q: 2) The following experimental process steps have been made to determine the hardness of water.…
A: Hard water does not form lather with soap instead from a curd-like substance. It is due to the…
Q: A colorless aqueous solution contains nitrates of two metals, X and Y. When it was added to a…
A: The question is based on the concept of qualitative analysis. We have to identify the cations…
Q: In many titrations, you need to add an indicator that changes color when the titration is complete.…
A: Interpretation: To find out what causes the color change at the end point signaling the completed…
Q: Solid KSCN was added to a 2.25 M Co²* solution so that it was also initially 2.25 M SCN¯. These ions…
A: Co2+ + SCN- ⇔ Co(SCN)+ initially : 2.25 M 2.25 M 0…
Q: 1. One of the methods of eliminating interferences, is by adding solvents to the solution in which…
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: A solution may contain Ag*, Pb²+, Hg₂². A white precipitate forms on addition of 6 M HCI. The…
A: Ag+, Hg2+2 and Pb+2 are group-I cation. They can be separated by group separation technique.
Q: The solubility of cadmium oxalate, CdC204, in 0.150 M ammonia is 6.1 x 10-³ mol/L. What is the…
A:
Q: Calculate the equilibrium concentrations of all species when 10 mL of 0.90M Fe2+ is mixed with 10 mL…
A: First we have to find initial concentration all the species just after mixing. Total volume, Vt =…
Q: To verify the existence of silver in your solution, one should first form a white precipitate by…
A: Reaction of Silver ion in the solution with NaCl is as follows. Ag+(aq) + NaCl (aq) → AgCl (s) +…
Q: The NaOH titrant in this experiment was prepared to be approximately 0.1 M and then was…
A: Given that, in an experiment, approximately 0.1 M of NaOH solution was prepared and then was…
Q: The substance to be analyzed – is white, highly soluble in water salt. When interacting with…
A: Salt analysis:
Q: What are the new concentrations for the standard solutions?
A: Clearly, this is a case of half dilution. 25 mL of aliquote is reacted with Fe(NO3)3 to form the…
Q: Precipitation of Ag+, Pb2+, and Hg+ with KOH a) Write out the correspoding solubility equilibrium…
A: Solubility is a phenomenon where the solute get dissolved in a solvent to form a solution. The…
Q: 2. In an iodometry titration, the appearance of blue colour upon addition of starch indicator is…
A: Iodometry titration can be defined as a method of volumetric analysis where the appearance or…
Q: 2. Consider a solution that is 0.100M in silver and 0.050 M in copper(I). Is it possible to…
A: Selective precipitation is a method of separating a specific ion from the mixture of ions present in…
Q: Write a balanced net ionic equation to show why the solubility of PbCO3(s) increases in the presence…
A: We have to write a balanced net ionic equation to show why the Solubility of Pb(CO3) increases in…
Q: The chemical formula for the oxalate ion is C2O42-. A liter of a saturated solution of calcium…
A: Since the solution was already saturated hence it means the concentration of ions present in the…
Q: How to qualitatively search for NO3- and NO2- in the presence of Br- anion? Explain with reaction…
A: Since you have asked multiple questions, we will solve the first question for you. If you want any…
Q: Part 2 Show your work, explain your reasoning fully, and indicate correct units (where appropriate).…
A: Solubility product: It is defined as the product of its dissolved ion concentrations raised to the…
Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…
A: Answer-a Henderson-hasslebalch equation is: pH=pKa+log[Base][Acid] if [Base]=[Acid}, then…
find present, absent and in doubt. And the reasoning of the following problem (photo)
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
- Will Mn(OH)2 precipitate from a 0.01 M solution of MnCl2 at pH = 9? Ksp(Mn(OH)2) = 1,0 x 10-13. Discuss from solubility diagrams and prove by calculation.calculation. Co is a metal that is present in every lithium battery to stabilize its charge and toincrease stability. Every cell phone, tablet and electric car relies on the availability ofcobalt, 97% of which is extracted from mines in places like the Congo, where essentially slave labor is used.Cobalt ions form complexes with e.g. CN- . You see solubility diagrams and fraction diagrams for CoCO3 with and without the addition of 10 mM CN- .. Explain whythe solubility of cobalt carbonate increases at high pH when cyanide ions are present.Write reaction formulas for the formation of the dominant cobalt cyanide complexes.ou are tasked with determining a way to identify the following ions in solution: Na+, Ni2+, Ag+, and Pb2+. What techniques would you use to selectively precipitate out the ions and how would you separate the precipitates from the supernatant layers? Your arsenal of compounds to use for the separation is KCl, KCH3COO, and KOH. Clearly define each step.A 1 L solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3. Ksp of CuCO3 = 1.4 x10-10Ksp of NiCO3 = 1.42X 10-7B. What would be the Molarity of Na2CO3 you will use in A , so that assumption of no volume change on addition of Na2CO3 will be valid ? please answer only B.
- How would you use an experimentally determined Ksp value to calculate that Ag2CrO4 should precipitate when 5ml of 0.0040 M AgNO3 are added to 5ml of 0.0024 M K2CrO4. You can come up with your own experimentally Ksp value. I just want to see steps in solvingThe solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?If 0.3074 g of a mixture of pure KCl and KBr requires 30.98 mL of 0.1007 M AgNO3 solution for its titration, calculate the% KCl and KBr in the sample. (Pat Data: Cl, 35.453; Br, 79.904; K, 39.098)
- A solution contains 1.0 × 10−4 M Cu+ and 2.0 × 10−3 M Pb2+. If a source of I− is added gradually to this solution, will CuI (Ksp = 1.27 × 10−12) or PbI2 (Ksp = 7.1× 10−9) precipitate first? Specify the concentration of I− necessary to begin precipitation of each salt and determine if the complete separation of Cu+ and Pb2+ feasible by fractional precipitation.The solubility of Ag2CrO4 (Ksp = 1.2 x 10^-12) is several times greater than that of AgCl (Ksp = 1.82 x 10^-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 as an indicator for 100 mL of sample solution, what is the concentration (M) of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
- In the determination of chloride by the Mob method, what will be the equiliblium concentration of silver ions in mgil, on the basis of the solubility product principle, when the chloride concentation has been reduced to 0.2 ma? (b) If the concentration of chromate indicator used is 5X M, how much excess silver ion in mgil must be present before the formation of a red precipitate will begi(a) In the defermination of chloride by the Mohr method, what will be the equilibrium concentration of silver ions in meL., an the basis of the solubility. pcoduct principle, when the chloride concencration has beea reduced to 0.2m 1.2m? (b) If -3 the concentration of chromate indicator ased is 5 x 10M, bow much excess silver ion in mel, must be present before the formatice of a red precipitate will begin?A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before developing. What mass of Na2S2O3∙5H2O (sodium thiosulfate pentahydrate or hypo) in 1.0 L of developer is required to dissolve the AgBr as Ag(S2 O3)2 3− (Kf = 4.7 × 1013)?Calculate the Molar Solubility of Calcium Hyroxide in the Presence of a Common Ion (CaCl2) I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.0646 2. volume of saturated Ca(OH)2 with added CaCl2 solution (mL) = 25 mL 3. Buret reading, initial (mL) = 0.03 mL 4. Buret reading, final (mL) = 19.85 mL 5. Volume of HCl added (mL) = 19.82mL Calculations: 6. Amount of HCl added (mol) = 1.28x10^-3 7. Amount of OH- in saturated solution (mol) =1.28x10^-3 8. [OH-] equillirium (mol/L) =5.12x10^-2 Molar solubility of Ca(OH)2=?