Q: A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and 3. strongly…
A:
Q: The quantitative determination of N,H, with KIO, proceeds in a mixture of H,O/CCI, as follows N,H, +…
A: Endpoint: refers to the point at which the indicator changes colour in titration. The endpoint is…
Q: Q4. A 5.00 ml aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by…
A: Permanganate reacts with hydrogen peroxide in acidic medium and reduces to Mn2+ and oxidises…
Q: Find the approximate percentage of chlorine, bromine, and iodine in the original sample?
A: Weight of the soluble salts containing chloride, bromide and iodide = 1.2 g The precipitate after…
Q: 100.0 ml of 0.400 M NICI, is mixed with 100.0 ml of 1.000 M NAOH. A precipitate of Ni(OH)2 results.…
A: The solubility product constant (Ksp) represents the solubility of products at equilibrium for…
Q: A 1.200-g sample of a mixture of NaOH (FW 40.00 g/mol) and NayCO3 (FW 105.99 g/mol) with inert…
A: The reaction between acid and base is termed as neutralization reaction. The products are salt and…
Q: The tetraethyl lead Pb(C2H5)4 in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL of…
A: Calculate the initial number of moles of iodine. n = C × VnI2 = CI2 × VI2nI2 = 0.02179 M × 0.015…
Q: Solve this gravimetric analysis problem. For the determination of Zn (AW = 65) gravimetrically in a…
A: Gravimetry is a process in which the analyte to be considered is converted to a sparingly soluble…
Q: A 55.00 mL solution of 0.3900 M AgNO, was added to a solution of Aso " . Ag, AsO, precipitated and…
A: “Since you have asked multiple question, we will solve the first question for you. If you want any…
Q: 9. The % w/w of I- in a 0.2144-g sample was determined by Volhard titration. After adding 50.00 mL…
A:
Q: 0.3 M AGNO3 solution is added to 50.0 mL of a s. ms immediately. The precipitate is then filtered…
A:
Q: 0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M' pure water, 2 M H2SO4 added,…
A:
Q: A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring…
A:
Q: A 55.00 mL solution of 0.3900 M AGNO, was added to a solution of AsO. Ag, AsO, precipitated and was…
A: Given. the AgNO3 solution is 55 ml or 0.055 L of 0.39M or 0.39 mol/L moles of Ag in the given…
Q: A concentration for the Ni ion was found to be 0.292 M. If you took 0.300 g of nickel sample and…
A:
Q: A 0.5657-g sample of a chlorocarbon compound was analyzed for its chloride content by burning it in…
A:
Q: The tetraethyl lead Pb(C2H5)4 in a 25.00 mL sample of aviation gasoline was shaken with 15.00 mL of…
A: The question is based on the concept of quantitative analysis. we have to quantitatively estimate…
Q: To find the Ce4+ content of a solid, 4.37 g were dissolved and treated with excess iodate to…
A: Here we have to calculate weight percent of Ce in the original solid-
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: If 0.3074 g of a mixture of pure KCl and KBr requires 30.98 mL of 0.1007 M AgNO3 solution for its…
A: From the used silver nitrate we can easily determine how many moles of silver nitrate was used.…
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: The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of…
A: Given reaction AgNO3 + I– → AgI (s) + NO3– Ag+ + SCN– → AgSCN We have to find milli moles of AgNO3…
Q: A 50.0 mL solution of CI (A.wt = 35.5 g/mol) was treated with 65.0 mL of 0.50 M AGNO3. AgCls) was…
A: 1) Volume of Cl- solution=50 mL 2) Concentration of [AgNO3]=0.5M MAgNO3=0.0005 mol/L 3) Colume of…
Q: A 0.6892 g mixture of KCN (MW = 65.116 g/mol) and NaCN (MW = 49.005 g/mol) was dissolved in water.…
A: Given: The mass of the mixture of KCN (potassium cyanide) and NaCN (sodium cyanide) is 0.6892 g The…
Q: The % w/w in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619…
A:
Q: Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.021 M KMnO…
A: the correct answer is as follows:
Q: An excess of potassium iodide is added to a solution of potassium dichromate, and the liberated…
A: K2Cr2O7 is a strong oxidizing agent. It will oxidize the Iodine from Iodide to molecular iodine. The…
Q: A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the…
A:
Q: 3) Now there are three test tubes without labels and the solutions are Na SO4, NA3PO4, and Na2CO3.…
A: We have three equations as follows 1- Reaction of Na2SO4 with Ba(NO3)2 Na2SO4 + Ba(NO3)2→NaNO3…
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: Q.1 :What is the molar concentration of CI in a solution prepared by mixing 25.0 mL of 0.025 M NaCl…
A:
Q: A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of…
A: Given data, Mass = 0.2386 g 48.40 mL of 0.04837M AgNO3 for complete titration Calculating the weight…
Q: 1. If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g, What…
A: Given, If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g,…
Q: PtCl4.2HCl has a secondary valence of 6. Hence, 6 mol of AgCl precipitate will be formed in excess…
A: False PtCl4.2HCl has a secondary valency of 6 indicating that all the substituents are ligands…
Q: chloride does the sample contain? (CI. JJ.J 7. Arsenic in a 5.0 gram sample is converted to H3ASO4…
A: Breathing in high levels of arsenic can cause a sore throat and irritated lungs. Swallowing high…
Q: A solution containing KCl (74.551 g/mol) is analyzed by the Mohr method. A 0.5863 g sample is…
A: Solutions Given that A solution containing KCl (74.551 g/mol) is…
Q: 4. A 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl…
A:
Q: A two-liter sample of mineral water was evaporated to a small volume, following which the potassium…
A:
Q: Ksp nu show, by calculation, that Ag2CrO4 should precipitate when 5 mL of 0.0040 M AgNO3 are added…
A: The question is based on the concept of solubility product Principle. it states that a weak…
Q: The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of…
A: Answer: These questions are based on stoichiometric calculation where we have to convert the moles…
Q: ercent (w/v) acetic acid content. For your experiment, you first standardized your aOH titrant with…
A:
Q: Formula of a compound 261.0 mg of FeCl,-xH,O crystals were dissolved in a diluted hydrochloric acid…
A: FeCl2.xH2O or Fe2+(aq) is oxidized by KMnO4(aq) to FeCl3 or Fe3+(aq). KMnO4(aq) or MnO4-(aq) itself…
Q: 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enough potassium chromate…
A: In a chemical reaction, two or more reactants react with each other to form new substances. This new…
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: the thiourea in a 1.455-g sample of organic material was extracted into a dilute H2SO4 solution and…
A: The balanced chemical equation is written as,
Q: c.) A 25.0 cm portion of sodium ethanedioate (Na CO,) solution of concentration 0.200 moldm is…
A: Given that, M1=0.200 mol/dm3 , V1=25.0 cm3 M2=? , V2=17.2 cm3 so,.
Q: Sulfur containing compound weighing 4.8670 grams was digested and purified to form H,SO4. A 25.00-mL…
A: Moles = Molarity * Volume (L) Mass = Moles * Molar mass
Step by step
Solved in 2 steps
- 1. If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g, What wt of AgCI could have been obtained from the same wt of sample?If a sample of silver coin weighing 0.2500 g gives a precipitate of AgCl weighing 0.2991 g, What wt of AgI could have been obtained from the same wt of sample?0.0585 g Na2C2O4 10 mL to adjust KMnO4 solution prepared in 0.1 M'pure water, 2 M H2SO4 added, heating process and 8.4 mL titrant as a result of titration it's spin out. Calculate the actual concentration of potassium permanganate accordingly
- What mass of AgCI is precipitated from the reaction of 25.0 mL of 0.100M AgNO3 and excess KCIDrops of dichlorofluorescein indicator have been added to a solution containing 0.2500 g sample of KBr whic h required 12.32 mL of standard 0.1700 M silver nitrate. Calculate the purity of K Br (119.00 g/mol) in the sample.1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI 4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2
- What quantity of sample should be taken for the analysis if it contains 16.2% chloride and the analyst wishes to obtain an AgCl precipitate weighing 0.600 g.1. A newly discovered iron ore was weighted (5.408 g) and worked up to produced 0.3785 g of ignited Fe2O3 precipitate. What is the percent purity of the iron in the sample? 2. Distinguish between equivalence point and end point.A 0.2386-g sample contained only NaCI and KBr. It was dissolved in water and required 48.40 mL of 0.04837 M AgN03 for complete titration of both halides [giving AgCI(s) and AgBr(s)]. Calculate the weight percent of Br in the solid sample
- A 1.200-g sample of a mixture of NaOH (FW 40.00 g/mol) and NayCO3 (FW 105.99 g/mol) with inert impurity is dissolved in 100 mL water and titrated with 0.150 M HCI.With phenolphthalein as the indicator, a 50.00 mL aliquot of the solution turns colorless after the addition of 30.00 mL of the acid. Methyl orange is then added, and 7.00 ml more of the acid are required for the color to change to pink. What is the percentage of NaOH in the sample?The chloride in a sample containing approximately 3.5 % NaCl is to be determined gravimetrically as AgCl. What weight of sample must be taken to obtain a precipitate that will weigh about 0.10 g?The % w/w I– in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back titrated with 0.05322 M KSCN, requiring 35.14 mL to reach end point. AgNO3 + I– → AgI (s) + NO3– Ag+ + SCN– → AgSCN How many millimoles of AgNO3 reacted with I–? How many milligrams of I– (MM=126.9 g/mol) were present in the sample? What is the % w/w I– in the sample?