A solution contains 6.67x103 M sodium sulfite and 6.14x103 M potassium chromate. Solid silver nitrate is added slowly to this mixture. What is the concentration of sulfite ion when chromate ion begins to precipitate? [sulfite]= M
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Q: 1. You add excess Sodium Acetate (NaCH3COOH), Sodium Chloride (NaCl), and Sodium lodide (Nal) to an…
A: Precipitation is the process of conversion of a chemical substance into a solid from a solution by…
Q: A solution contains 8.26x103 M potassium sulfite and 9.76×10 M sodium hydroxide. Solid calcium…
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Q: Calcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate,Na2C2O4, is required…
A: Given: Volume of CaCl2 = 37.5 ml Molarity of CaCl2 = 0.104M
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Q: A 50.0 mL sample of 0.0152 M Na2SO4 (aq) is added to 50.0 mL 0.0125 M Ca(NO3)2 (aq). What percentage…
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Q: A solution contains 0.0490 M Ca²+ and 0.0980 M Ag*. If solid Na3PO4 is added to this mixture, which…
A: GivenCa2+ = 0.0490 MAg+ = 0.0980 MKspCa3(PO4)2 = 2.07 * 10-33Ca3(PO4)2 → 3 Ca2+ + 2…
Q: 1- In principle, it is possible to separate the Ba + 2 and Ca + 2 ions by the difference in…
A: Solubility product of BaF2 is given as Ksp=[Ba2+][F-]2 As per the given data we have Ksp of…
Q: A solution contains 1.23×102 M potassium sulfide and 1.34x102 M sodium carbonate. Solid cobalt(II)…
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Q: A solution contains 8.49x10 M calcium nitrate and 9.73x10 M magnesium ace Solid sodium carbonate is…
A: Given, Concentration of Calcium nitrate, Ca(NO3)2 = 8.49 X 10-3 M Concentration of Mg(CH3COO)2 =…
Q: A solution contains 1.32x102 M sodium carbonate and 8.59x10 M potassium hydroxide. Solid copper(II)…
A: Copper(II) nitrate reacts with sodium carbonate to form copper(II) carbonate and with potassium…
Q: A solution contains 1.33x102 M chromium(III) nitrate and 7.29×10-3 M iron(II) acetate. Solid…
A: I
Q: Use the solubility rules listed in Section 8.3B to predict whether each of the following ionic…
A: Since you have posted multiple sub-parts, the answer for first three sub-parts are given below.…
Q: If a solution contains 0.0020 mol of CrO42−CrO42− per liter, what concentration of Ag+ ion must be…
A: As the value of Ksp for AgCrO4 is not given, so the reference taken from internet, therefore; the…
Q: A solution contains 6.79x103 M magnesium nitrate and 1.30×102 M barium acetate. Solid potassium…
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Q: 1. A 10.0 mL graduated cylinder to measure 10.0 mL of a 1.00 M CaCl2 solution into an initially…
A: The balanced chemical equation has to be written,
Q: III) When 25.0 mL of 0.100 M cadmium (II) nitrate and 20.0 mL of 0.150 NazS are mixed a yellow…
A: Volume of Cd(NO3)2 solution (V1) = 25 ml Molarity of Cd(NO3)2 solution (M1) = 0.1 M Volume of Na2S…
Q: A solution contains 0.0430 M Ca²+ and 0.0990 M Ag*. If solid Na3PO4 is added to this mixture, which…
A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…
Q: solution contains 6.88×10-3 M ammonium carbonate and 1.16×10-2 M potassium fluoride. Solid magnesium…
A: The question is based on the concept of solubility product Principle. it states that a weak…
Q: A solution is 1.5×10-2 M in Ba?+ and 1.8×10-2 M in Ca²+. Consider that Ksp (BaSO4) ==1.07 × 10¬10…
A: Given : [Ba+2] = 1.5 x 10-2 M [Ca+2] = 1.8 x 10-2 M Ksp(CaSO4) = 7.1 x 10-5 Ksp (BaSO4) = 1.07 x…
Q: If a solution contains 0.0020 mol of CrO4 2− per liter, what concentration of Ag+ ion must be…
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Q: that contains 0.015 M Ni2+ ions and 0.015 M Ca2+ ions. You slowly add Na2CO3 to the solution. What…
A: Solubility equilibrium is a type of dynamic equilibrium that exists when a chemical compound in the…
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A: 1. In double displacement reaction, cation of one species easily replaces cation of another species…
Q: A solution contains 9.02×10-3 M calcium acetate and 9.34×10-3 M aluminum nitrate. Solid potassium…
A: Given concentration is: Ca2+=9.02×10-3MAl3+=9.34×10-3M When KOH(s) is added to the mixture solution.…
Q: A solution contains 5.38×10-3 M lead nitrate and 8.44x103 M cobalt(II) acetate. Solid ammonium…
A: The concentration of lead nitrate, Pb(NO3)2 = 5.38×10−3 M The concentration of cobalt(II) acetate,…
Q: A solution contains 5.51x10-3 M silver acetate and 5.89x10-3 M barium nitrate. Solid potassium…
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Q: A solution contains 1.43x10 M lead nitrate and 5.74x10 M silver acetate. Solid potassium sulfate is…
A: Given that: Concentration of lead nitrate =1.43x10-2 M Concentration of silver acetate =5.74x10-3 M…
Q: A solution contains 1.47x10? M zine nitrate and 1.37x102 M cobalt(II) acetate. Solid potassium…
A: The solubility products are - ZnCO3 =1.46 ×10-10CoCO3 =1 ×10-10
Q: A solution contains 1.05x102 M zinc acetate and 1.04×10 M nickel(II) nitrate. Solid sodium cyanide…
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Q: A solution contains 8.26x10-3 M potassium sulfite and 9.76x10-3 M sodium hydroxide. Solid calcium…
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Q: A solution contains 8.49x10 M sodium carbonate and 9.73x10 M potassium hydroxide. Solid calcium…
A: Precipitation reaction: Reaction in which some substance in form of precipitate is formed by…
Q: A solution contains 0.0480 M Ca²+ and 0.0990 M Ag*. If solid Na;PO4 is added to this mixture, which…
A: Given information: Concentration of calcium ions = 0.0480 M Concentration of silver ions = 0.0990 M
Q: In the laboratory, strontium chromate (Ksp = 3.6 x 105) can be prepared by mixing solutions…
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Q: A solution contains 1.34x102 M silver nitrate and 1.45x10 M barium acetate. Solid potassium…
A: Hi, since there are multiple questions posted we will provide you with answers for the first…
Q: A solution contains 1.14x10 M nickel(II) nitrate and 9.53x10 M lead acetate. Solid potassium…
A: A) The reactions taking place when the given compounds react with KOH is as follows:…
Q: 5, A litre of solution contains 100 mg of barium ions and 10.0 g of strontium ions. Within what…
A: Ksp of BaCrO4= 2.3×10^-10 Ksp of SrCrO4= 3.5× 10^-5 Q= [Ba2]× [CrO4-] Q=[Sr+][CrO4-] If…
Q: A solution contains 1.02x102 M iron(III) acetate and 7.84×103 M zinc nitrate. Solid potassium…
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Q: A solution contains 1.39x102 M sodium phosphate and 1.11×10-2 M sodium fluoride. Solid calcium…
A: Given: Concentration of sodium phosphate i.e. Na3PO4 = 1.39 × 10-2 M. And the concentration of…
Q: A solution contains 7.52x103 M potassium hydroxide and 1.40×102 M sodium carbonate. Solid zinc…
A: Given: Concentration of sodium carbonate i.e. Na2CO3 = 1.40 × 10-2 M. And concentration of potassium…
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A: The salt having lower value of solubility product precipitates out first in a solution . In the…
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Q: What is the maximum mass (in grams) of each of the following soluble salts that can be added to 310…
A: First we have to find the moles of BaCl2 then write the equation to find the mooea of respective…
Q: A solution contains 1.33×102 M chromium(III) nitrate and 7.29x10³ M iron(II) acetate. Solid…
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Q: A solution contains 1.21x102 M magnesium nitrate and 1.42x102 M lead acetate. Solid sodium carbonate…
A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…
Q: The removal of an ion is sometimes considered to be complete when its concentration drops to…
A: Given: Concentration of ion should be 1.00 × 10-6 M or lesser for the complete removal. And the Ksp…
Q: A solution contains 1.05x102 M zinc acetate and 1.04x10 M nickel(II) nitrate. Solid sodium cyanide…
A: Explained as follows
Q: Chemistry Will a precipitate form if 100.0 mL of 1.1X10 --mol/L lead(II)Chloride is mixed with 100.0…
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Q: When 1.0 mole of solid lead nitrate is added to 2.0 moles of aqueous potassium iodide, a yellow…
A: Electrolytes :- Substances whose aqueous solutions can conduct electricity are called electrolytes…
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A: Given, final solution contains 0.2mol Pb(CH3COO)2, 0.1mol Na2S and 0.1mol CaCl2.
Q: A solution contains 1.14×10² M magnesium nitrate and 1.13×10-² M copper(II) acetate. Solid potassium…
A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…
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- To determine the percent purity of a sample containing iron(II) ammonium sulfate; Suggest , 2 different methods for iron(II) ion. Explain in detail what errors may occur in the methods. (volhard method, gravimetric analysis, kjeldahl, etc.) Percentage content: 1-100% ; the solution concentrations to be used are 0.01-0.1M; Take the volumes of solution to be used between 1-50 mLCalculate the saturation indices of the solutions described below and classify each as undersaturated, supersaturated, or in equilibrium. Saturation state with respect to: Anhydrite (CaSO4) [Ca2+] = 0.00002 mM [SO42-] = 25 mM “Amakinite” (Fe(OH)2) [Fe2+] = 0.1 mM; [OH-] = 0.0001 mM Siderite (FeCO3) [Fe2+] = 3 mM; [CO32-] = 10 mMWhat weight of the soda ash (impure Na2CO3) should be taken for analysis in order that the number of milliliters of 0.500 N acid used will be equal to one-half of the percentage of Na2CO3 in the sample? Note: Present complete solutions for the following problems.
- Calculate the saturation indices of this solution. Then classify as: undersaturated, supersaturated, or in equilibrium. Why? Saturation state with respect to: Siderite (FeCO3) [Fe2+] = 3 mM; [CO32-] = 10 mMThe melting point of TiCl4 (-24°C) lies below those ofTiF4 (284°C) and TiBr4 (38°C). Explain why by considering the covalent-ionic nature of these compounds and theintermolecular forces in each case.USE THE DATA BELOW ON MOLAR ABSORPTIVITIES FOR THE TWO PRINCIPAL SPECIES IN A SOLUTION OF POTASSIUM DICHROMATE. Four solutions were prepared by dissolving 3.50 x 10^-4 , 3.00 x 10^-4, 2.50 x 10^-4, and 2.00 x 10^-4 moles of K2Cr2O7 in water and diluting to 1.0 L with a pH of 5.55 buffer. Derive theoretical absorbance values using a 1.00-cm cells for each solution and plot the data for (a) 345 nm (b) 370 nm, and (c) 400 nm.
- Caustic potash that has been exposed to air is found on analysis to contain 90.00% KOH, 2.38% K2CO3 and 7.62% H2O. What weight of residue will be obtained if 1.00 g of this sample is added to 46.00 mL of 1.00 N HCl and the resulting solution, after neutralization with 1.070N KOH is evaporated to dryness?You are assigned an unknown solution that contains Group III cations. To -1 mL of this solution was added 6 M NH3 the solution was agitated to mix well, and a reddish-brown precipitate with a gelatinous solid clinging to the inner walls of the test tube was observed. The solution was centrifuged and the supernatant was tested for completeness of precipitation by adding an additional drop of 6 M NH3. No cloudiness was observed as the drop of reagent diffused through the solution. The supernatant was then carefully decanted into a clean test tube, labeled (1st solution), and saved for further testing later. The precipitate remaining in the test tube was washed with a small amount of water, centrifuged, and the wash decanted and discarded. To the precipitate was added about 10 drops of 6 M NAOH plus ~1 mL H20 and the test tube was vigorously agitated. The resulting suspension was centrifuged and the supernatant liquid was transferred to another clean test tube and clearly labeled (2nd…Provide detailed solutions.
- Percentage purity of a sample of 0.1350 g of As2O3 assayed iodometrically using 23.5 mL of 0.1055N iodine solutionYou and a partner are asked to complete a lab entitled“Oxides of Ruthenium” that is scheduled to extend over twolab periods. The first lab, which is to be completed by yourpartner, is devoted to carrying out compositional analysis.In the second lab, you are to determine melting points. Upongoing to lab you find two unlabeled vials, one containinga soft yellow substance and the other a black powder. Youalso find the following notes in your partner’s notebook—Compound 1: 76.0% Ru and 24.0% O (by mass), Compound2: 61.2% Ru and 38.8% O (by mass). (a) What is the empiricalformula for Compound 1? (b) What is the empiricalformula for Compound 2? Upon determining the meltingpoints of these two compounds, you find that the yellowcompound melts at 25 °C, while the black powder does notmelt up to the maximum temperature of your apparatus,1200 °C. (c) What is the identity of the yellow compound?(d) What is the identity of the black compound? (e) Whichcompound is molecular? (f) Which compound is…Ammonium iron(II) sulfate crystals have the following formula: (NH4)2SO4.FeSO4.nH2O . In an experiment to determine n 8.492g of the salt were dissolved and made up to 250cm^-3 of solution with distilled water and sulphuric acid. A 25.0cm^-3 portion of the solution was titrated against 0.0150 mol dm^-3 KMnO4. A volume of 22.5cm^-3 was required. Find the value of n