Formula of a compound 261.0 mg of FeCl,-xH,O crystals were dissolved in a diluted hydrochloric acid and titrated with 0.02 M KMNO, solution of which 13.13 mL was required. Determine the formula of crystallohydrate.
Q: The phosphate in a 3.00 g sample of industrial detergent was precipitated by the addition of 1.000 g…
A: Precipitation titration is that type of volumetric titration in which precipitates are formed. It is…
Q: A 4.912-g sample of a petroleum product was burned in a tube furnace, and the SO 2 produced was…
A: The number of moles of excess base is equal to the number of moles of HCl used for back titration.…
Q: A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach…
A: Given Volume of Ca( OH)2 solution ( V1 ) = 50 mL Molarity of HNO3 ( M2 ) = 0.340 M…
Q: Calculate the solubility of TlBrO3(s) in water in grams per liter at 25C given that Ksp=1.1x10^-12…
A: Given-> Ksp of TlBrO3 = 1.1 × 10-12
Q: 9. What volume of a silver nitrate solution that contains 10.98 g of primary standard AgNO; in 1.00…
A: Mass of AgNO3 = 10.98 g Volume of primary standard AgNO3 = 1.0 L Mass of Na2CrO4 = 0.259 g
Q: 1. Titration of 0.485g sample by the Mohr method required 38.8mL of standard 0.1060 M AgNO3…
A: Given, Weight of sample= 0.485 g Concentration of AgNO3 = 0.1060 M Volume = 38.8mL = 38.8/1000 =…
Q: Determine the molar solubility of phosphate in Zn(OH)2 (Ksp = 1.8 x 10-14) in a solution of 0.025 M…
A:
Q: An acidic solution of copper (.35 M Cu+2) was treated with KOH until Cu(OH)2 precipitated. At what…
A: Given : Concentration of Cu2+ = 0.35 M Using appendix, the solubility product of Cu(OH)2 is 1.6 X…
Q: A 300.00 ml solution of HBr was treated with 5 ml of freshly boiled and cooled 8 M HNO3, and then…
A: Ag+ + Br- → AgBrs The balanced equation is, Ag+ + SCN- → Ag(SCN)(s) Number of moles of Ag+…
Q: A 0.7120 g of iron ore was brought into solution and passed through a Jones reductor. Titration of…
A: The balanced redox reaction given is 5 Fe+2 + MnO4- + 8H+ → 5 Fe+3 + Mn+2 + 4 H2O Volume of KMnO4 =…
Q: 0.250 g sample of impure CaCl2 is titrated with 40.00 mL 0.105 M AgNO3 solution. Calculate the…
A: Given: 1) Mass of impure CaCl2 = 0.25 g 2) Volume of AgNO3 = 40 mL 3) Concentration of AgNO3 = 0.105…
Q: Identify the type of coprecipitation that occurred in the following situation. (a) The…
A: answer - (a) The precipitation of bulky precipitates (e.g. MgNH4PO4) traps significant amount of the…
Q: A solution containing chloride ion was analyzed by the Volhard method. A 50.00 mL sample containing…
A: Given, MAgNO3 = 0.2500 M VKSCN = 25.00 mL = 0.025 L MKCN = 0.2380 M VKSCN = 10.67 mL = 0.01067 L
Q: A solution was prepared by dissolving 511 mg of Na,Fe(CN), (M = 303.91 g/mol) in sufficient water to…
A: c Weight/volume percentage is- W/V%=mass of solutegvolume of solution mL×100…
Q: 0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M' pure water, 2 M H2SO4 added,…
A:
Q: Limestone consists mainly of the mineral calcite, CaCO3. The carbonate content of 0.5413 g of…
A: The ratio of mass of solute to the mass of solution multiply by 100 is known as % mass.
Q: Limestone consists mainly of the mineral calcite, CaCO 3. The carbonate content of 0.5413 g of…
A: Given data: Mass of limestone = 0.5413 g Volume of HCl = 10 mL Molarity of HCl = 1.396 M Volume of…
Q: Chrome then curiously asked Senku if it was possible to titrate the pure KHA. H2A2H;O sample through…
A:
Q: 2. A sample of pure sodium chloride (MW = EW = 58.44 ) weighing 0.2286 g is dissolved in water and…
A: Given data : Mass of NaCl = 0.2286 g Volume of AgNO3 = 50.00 mL =…
Q: Calculate the molar solubility of CaF, at 25°C in a 0.010 M NaF solution. (Ksp CaF2 = 3.9 x 10 11)…
A:
Q: 4. Silver arsenate, Ag,AsO4, is very insoluble. What weight of Ag,AsO4 precipitate forms when 27.00…
A:
Q: The sulfur from 4.00g steel is evolved as dihydrogen sulfide gas and titrated with 1.60 mL of…
A:
Q: A mixture containing only KCl (74.55 g/mol) & NaBr (102.89 g/mol) was analyzed by the Mohr method. A…
A: Chloride ion concentration of an unknown sample can be calculated using Mohr method. In Mohr…
Q: A solution was prepared by dissolving 1210 mg of K3Fe(CN)6 (329.2 g/mol) in sufficient water to give…
A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…
Q: T1 0.3217 g 16.86 mL T2 0.3508 g 17.55 mL T3 0.2895 g 14.62 mL MW of KHP = 204.3 g/mole %3D
A: Given data: Molar mass of KHP = 204.3 g/mol Formula used: Molarity=molesVolume (L)
Q: An analysis for borohydride ion is based on its reaction with Ag+: BH4- + 8Ag+ + 8OH--> H2BO3- +…
A:
Q: accordingly
A: Mass of Na2C2O4 = 0.0585 g Molar mass of Na2C2O4 = 134 g/mol At equivalent point, Geq. of KMnO4 =…
Q: 0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL…
A: The titration of MBr by AgNO3 is a double-displacement reaction, which is given by,…
Q: A 25.00-mL sample of a household cleaning solution was diluted to 250.0 mL in a volumetric flask. A…
A: Answer: This is a question based on acid-base titration where base is the analyte and acid is the…
Q: Calculate the molar solubility of Mg(OH)2 in a solution of 0.050 M MgCl2 [Ksp for Mg(OH)2 = 5.6 ×…
A:
Q: The arsenic in a 1.208-g sample of a pesticide was converted to H3 AsO4 by suitable treatment. The…
A:
Q: The Zn in a 0.6803-g sample of foot powder was titrated with 27.3 mL of 0.04246 M EDTA. Calculate…
A: To calculate the percentage of zinc in the foot powder sample, use the EDTA titration. First…
Q: 0.683 grams of iron mineral dissolves with acid. Fe2+ is titrated with Ce(SO4)2 solution. Calculate…
A:
Q: A mixture containing iodide is analyzed by the Volhard method. 0.6712 g of the sample is reacted…
A: mass of the sample = 0.6712 g Concentration of AgNO3=0.05619 M Volume of AgNO3=50.00mL Concentration…
Q: Calculate the solubility of copper(I) sulfide (Cu2S, Ksp = 2.26 × 10−48) in a 0.010 M CuC2H3O2(aq)…
A: The solubility of copper (I) sulfide in 0.01 M copper (I) acetate solution can be expressed as…
Q: 1.0 g of a solid sample known to contain a mixture of NaOH and Na2CO3 is dissolved with distilled…
A: Volume of 0.107 M HCl added with Phenolphthalein indicator = 10.6 mL * (1L/1000 mL) = 0.0106 L…
Q: An aqueous ethylene glycol (HOCH, CH, OH, FW = 62.07 g/mol) solution with a mass of 220.9 mg is…
A: Answer: mass percent= 8.15 %
Q: Suppose that the solubility of calcium iodate are 2.5 g/L at 20oC and 5.5 g/L at 60oC. What are the…
A: I = Atomic mass of Ca + 2(Atomic mass of I) + 6(Atomic mass of O) = [40+2(127)+6(16)] g/mol = 390…
Q: A pure organic compound has the formula C4H8SOx. A sample of a compound was decomposed; the sulfur…
A: Molecular formula = C4H8SOx weight of sample = 12.64 mg Ba(ClO4)2 needed for titration = 10.60 mL…
Q: Explain why addition of NH3 or HNO, to a saturated solution of Cu(OH)2 in contact with solid Cu(OH)2…
A: This is a question from co-ordination chemistry. Coordination chemistry deals with the complex…
Q: From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 5.600 g Mass of FeCl3 : 1.60 g From Part B: %…
A: Given,
Q: Iro
A: (a) This step is performed to dissolve any impurity present in the precipitate and to make sure to…
Q: The gravimetric factor (GF ) for Ag in precipitated Ag2CrO4 equal:(Atomic (weights, Cr=24;Ag=108…
A: The reaction for the process is : 2Ag+ + CrO42- ⇌ Ag2CrO4(ppt.) The Gravimetric factor, (GF) can…
Q: Silver chromate is sparingly soluble in aqueous solutions. The ?spKsp of Ag2CrO4Ag2CrO4 is…
A: Given, Ksp of Ag2CrO4 = 1.12×10−12 concentration of potassium chromate = 1.10 M concentration of…
Q: Which of the following salts does NOT cause permanent hardness? B CaCl, © M8SO, Ca(HCO ,), 2
A:
Q: The excess K2Cr207 was back-titrated with 8.53 ml of 0.00949 M Fe2* şolution. Calculate the molar…
A: Answer is 1.12×10-²M
Q: A solution is made by mixing 500.0 mL of 0.02018 M Na, HASO, with 500.0 mL of 0.04078 M NaOH.…
A: Solution: From the given data one thing we have clear that this is the type of acid base reaction.…
Q: Calculate the mass solubility of AgCO (K = 8.1 x 10, MM = 275.74 g/mol) in a 0.010 M AgNO solution…
A: The compound is actually Ag2CO3(s) with Ksp = 8.1*10-12 The other compound is AgNO3. Since AgNO3…
Step by step
Solved in 5 steps
- It is desired to determine the concentration of chlorides in a powdered milk following the method of Volhard, for such case 1.5g of milk is weighed, it is heated in a muffle until obtaining ashes, which are treated with acid water with some drops of HNO3, the solution is filtered and the obtained filtrate is collected in an Erlenmeyer and 20 mL of AgNO3 0 is added. 1M excess silver is titrated with 0.05M potassium thiocyanate, if 8 mL of KSCN has been used up at the time of the indicator turn. Calculate the % of chloride in the milk powder.If 175ml of a 0.00550 M KCI solution is mixed with 145ml of a 0.00150M AgNO3 solution,will AgCl (Ksp=1.77 x 10-10) precipitate?A sample consisting of Na2CO3, NaOH and inert matter weighs 1.179g. It is titrated with 0.2239M HCl with phenolphthalein as the indicator. The solution became colorless after the addition of 45.62 mL. Methyl orange is then added and 12.85 mL more of the acid are needed for the color change. what is the percent Na2CO3 in the sample?
- Calculate the solubility (in mol L-1) of CaF2(s) at 25°C in a 0.040 M aqueous solution of NaF.A soda ash sample was contaminated with NaOH. It was made up of 0.00069 moles of NaOH and 0.00115 moles of Na2CO3. What would be the expected volumes of Vphth and Vmo if the said sample was titrated with 0.1M HCl?Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00 mL vinegar sample requires 12.15 mL of 0.250 M NaOH to reach the phenolphthalein endpoint. How many grams of acetic acid are present in the sample?
- A solution is prepared by mixing 100.0 mL of 1.0x10-2 M Pb(NO3)2 and 100.0 mL of 1.0x10-3 M NaF. Will PbF2 (Ksp= 4x10-8 ) precipitate?2.1 Calculate the pH of the pre-equivalence solution for the titration of 25mL of a 0.025 M H2SO4 solution with 0.050 M NaOH, after the addition of 25.9 mL NaOH. 2.2 Name 5 requirements of a compound that will be used as a primary standard in titrimetry0.0585g of Na2C2O4, 10 mL of distilled water, 2 M H2SO4 was added to adjust the KMnO4 solution prepared as 0.1M, heating was performed and 8.4mL of titrant was spent as a result of titration. Calculate the true concentration of potassium permanganate accordingly.
- The titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? Given that the chemical reaction is 2MnO4- + 5C2O42- + 16H+ -----> 2Mn2+ + 10CO2 + 8H2O Provide a detailed solution.Neutralization Titration In the standardization of HCI solution using 10.00 ml of 0.02 Na,co, according to the equation M of Na,CO, 2 HCI 2NaCl + H₂O+CO, 15.0 ml of HCI is required to reach the end point using Bromocresol green indicator the molarity of HCI (mol/L) would be al 0.032 b) 0.027 20.013 d) 0.008 e) 0.064The composition of a hydrated sodium-salt of a chromium(III)-oxalate complex ion conforms to the general formula: NaxCr(C2O4)3·wH2O A 0.2547-g sample of this compound required 21.99 mL of 0.02925 M KMnO4 solution for the titration of all of the oxalate. a)What is the value of x? b)What is the value of w?