Use stoichiometric methods to analyze a mixture. A mixture of MgCl, and inert material is analyzed to determine the Mg content. First the mixture is dissolved in water. Then all of the chloride ion is precipitated as AgCl by the addition of an excess of silver nitrate. MgCly(aq) + 2A£NO3(aq) 2A£C(s) + Mg(NO3)½(aq) In one experiment, a 0.5770 g sample of the mixture resulted in 1.3717 g of AgCl. Determine the percent (by mass) of Mg in the mixture. % Mg
Q: Many metal ions are precipitated from solution by the sulfide ion. As an example, consider treating…
A: Given: The reaction is as follows, CuSO4(aq) + Na2S(aq) → CuS(s) + Na2SO4(aq) Molarity of Na2S…
Q: Potassium permanganate, a strong oxidizing agent, is commonly used in titrations because of its…
A: Given, 27.12 mL of 0.1147 M KMnO4
Q: 164.00 mL of 0.200 M Cu(NO3)2(aq) is mixed with 93.000 mL of 0.400 M NaOH(aq). Assuming 100% yield,…
A: The chemical reaction is: Cu(NO3)2 (aq) + 2NaOH (aq) →Cu(OH)2 (s) + 2NaNO3 (aq)
Q: Consider the following reaction: Pb(NO3)2(aq) + 2KI(aq)→ Pbl½(s) + 2KN03(aq) What mass of lead…
A:
Q: To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.130M silver…
A:
Q: A 2.00g sample of limestone was dissolved in hydrochloric acid and all the calcium present in the…
A: Ca2+ + C2O42- ----CaC2O4
Q: To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.260M silver…
A: Given, Concentration of silver nitrate is = 0.260 M. Mass of fluid is = 21 g Final mass of product…
Q: In the precipitation reaction AgNO3 (aq) + KCI (aq) → AgCl (s) + KNO3 (aq), the precipitate is KNO3…
A: When two aqueous solutions react, they sometimes form solids in the solution. The solid is called a…
Q: The precipitation reaction between 25.0 mL of a solution containing a cation (purple) and 35.0 mL of…
A: Precipitation reaction: The chemical reaction in which insoluble salt or precipitate form in…
Q: One way the U.S. Environmental Protection Agency (EPA) tests anions in solution will combine with…
A: Given reactionNiCl2(aq.) + 2 AgNO3 (aq.) → 2 AgCl(s) + Ni(NO3)2 (aq.)Mass of Silver Chloride =…
Q: Based on the solubility rules, which of these processes will occur if solutions of CuSO4(aq) and…
A:
Q: concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue…
A: The question is based on reaction Stoichiometry. we have to determine the concentration of copper…
Q: What is the final concentration of the diluted solution if a student was asked to prepare a new HCl…
A: Given: Concentration of stock HCl solution = 12 M Volume of stock solution taken = 0.50 mL And the…
Q: Which of the following compounds will have the state symbol (aq) when mixed with water? Remember…
A:
Q: To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.380M silver…
A: Given following balanced Chemical equation - Cl-(aq) + AgNO3(aq) ----> AgCl(s) + NO3-(aq) Also…
Q: Write the balanced net ionic equation for the precipitation of cobalt(II) sulfide from aqueous…
A: 1.The balanced net ionic equation for the precipitation of cobalt(II) sulfide from aqueous solution…
Q: In a food and drink industry, sulphur dioxide is often used as a preservative. By gravimetric…
A: Sulfur dioxide is a widely used preservative and antioxidant in food items and drinks. Healthy…
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A: Hi, as you have posted 2 questions and have not mentioned which one you want us to solve for you.…
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A:
Q: A mixture consisting of only sodium chloride (NaCl) and potassium chloride (KCl) weighs 1.0000 g.…
A: When in a mixture two soluble salts are mixed with a precipitating agent, the initial salts get…
Q: mass of 0.284 g. The limiting reactant in the salt mixture was later determined to be CaCl2·2H2O.…
A: since you have posted a question with multiple subparts we are entitiled to answer only first 3…
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A: Here we are required to find the concentration of iron chloride present in the ground water sample
Q: To measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.180M silver…
A:
Q: You are asked to determine the percentage of the components of a mixture containing sodium iodide,…
A: Given that, Mass of BaSO4 recovered = 2.04 gms Total Mass of mixture sample = 4.42 gms Therefore, %…
Q: When a solution of ammonium chloride, NH4Cl, is added to a solution of lead(II) nitrate, Pb(NO3)2, a…
A: Which of the following is the total ionic equation for this reaction?
Q: To measure the concentration of an aqueous solution of H₂O2, an analytical chemist adds strong acid…
A: Given following balanced Chemical equation - 6H+(aq) + 5H2O2(aq) + 2MnO4- (aq) ----> 5O2(g) +…
Q: Indicate which of the following pairs of reactants would yield a precipitation reaction and give the…
A: In a chemical reaction, the reactants react to form the products. Chemical reactions are of…
Q: CaCO3 + HCl →CO2 + CaCl2 + H2O Suppose you collect a 5.00 g sample of impure limestone and want to…
A:
Q: Lead ions can be precipitated from solution with KClKCl according to the following reaction:…
A:
Q: Zinc and magnesium metal each react with HCl according to the following equation: Zn + 2 HCl= ZnCl2…
A:
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A: Given data,Volume of sample=200mLMolarity of AgNO3=77.0mMMass of AgCl=3.3mg
Q: Solutions of magnesium sulfate and potassium phosphate react to form a precipitate. What volume, in…
A:
Q: 30.0 g of NaOH is added to 0.800 L of 1.00 M Zn(NO₃)₂, what mass in grams of Zn(OH)₂ will be formed…
A: Calculate mole of each Reactant them find out limiting reagent.here is NaOH Mass of Zn(OH)2 =…
Q: When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out…
A:
Q: To measure the amount of calcium carbonate (CaCO3) in a seashell, an analytical chemist crushes a…
A:
Q: A student requires 45.0 grams of solid silver chloride to precipitate. What volume of a 0.50 M…
A: As here NaCl is used in excess amount the limiting reagent is AgNO3 from here we can calculate the…
Q: Write the balanced NET ionic equation for the reaction when aqueous calcium chloride and aqueous…
A: The reaction of aqueous calcium chloride with aqueous lead(II) nitrate has been considered. The…
Q: The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II)…
A: The question is based on the concept of solutions. we have to calculate the original concentration…
Q: You are asked to determine the percentage of the components of a mixture containing sodium iodide,…
A: The percent Mg(OH)2 in the original sample mixture is to be calculated. Given: Mass of sample =…
Q: You are asked to determine the percentage of the components of a mixture containing sodium iodide,…
A: (a) Mass of NaI recovered = 0.95g NaI Total mass of mixture = 4.82 g Thus, percent NaI in sample =…
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaninants in water is…
A:
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A: we have to calculate the concentration of copper(II)chloride
Q: (a) When a solution of calcium chloride (CaCl2) is mixed with a solution of sodium carbonate…
A: (a) First balanced Molecular equation : When one equivalent of CaCl2 react with one equivalent of…
Q: Lead ions can be precipitated from solution with KCI according to the following reaction: Pb (ag) +…
A: Given data mass of KCl = 28.7 g mass of Pb2+ = 25.8 g Reaction : Pb2+ + 2 KCl → PbCl2 + 2 K+…
Q: In an experiment of "Gravimetric Methods of Analysis: Determination of %SO3 in a Soluble Sample",…
A: The amount of an analyte can be determined through the measurement of mass in the technique call…
Q: You are asked to determine the percentage of the components of a mixture containing sodium iodide,…
A: Given: mass of mixture sample = 4.82 g mass of NaI recovered = 0.95 g mass of BaSO4 recovered = 2.04…
Q: The strength of the eggshell of birds is determined by the calcium carbonate content of the…
A:
Q: Write the balanced molecular equation for this reaction AND determine the concentration of the…
A: Given volume of HCl solution is 20.00 mL Given volume of NaOH solution is 30.50 mL and strength of…
Q: One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is…
A: The balanced equation is:
- In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it bad a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.The concentration of arsenic in an insecticide can be determined gravimetrically through its precipitation as MgNH4AsO4. After the formation of the precipitate, it must be ignited for total conversion to Mg2As2O7, which is then cooled and weighed. Considering that a sample of 1,627 g of the insecticide produced 106.5 mg of Mg2As2O7, determine the% (m/m) As2O3 in the insecticide. Given the molar masses: Mg2As2O7 = 310.447 g / mol and As2O3 = 197.841 g / molYou are going to standardize your sodium hydroxide by titrating with potassium hydrogen phthalate. As an example, you dissolve 0.3365 g of potassium hydrogen phthalate, otherwise known as KHP (KHC8H4O4) in water in a 250.0 mL Erlenmeyer flask and then add phenolphthalein indicator. You then titrate with your sodium hydroxide solution, which is in a buret, and you determine that the equivalence point is at 12.44 mL of your sodium hydroxide solution. Determine the molarity of your sodium hydroxide solution. What color will the solution of potassium hydrogen phthalate turn to determine when the equivalence point has been reached?
- When titrated with permanganate, the iron oxalate salt studied in the first three experiments reacts as follows: 5C2O42– + 2MnO4– + 16 H+ → 10 CO2 + 2Mn2+ + 8H2O If 12.47 mL of a 0.33 M KMnO4 was used to reach the equivalence point in titrating the oxalate salt, how many moles of the oxalate reacted? You must enter your answer in exponential notation with two decimal places. Example: 2.33e-4One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s)+CuSO4(aq) ----------> Cu(s)+FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 500.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 104.mg.Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 3 significant digits. _______________g/LTo measure the amount of chlorine in a well-boring fluid, an analytical chemist adds 0.3600M silver nitrate AgNO3 solution to a 24.00g sample of the fluid and collects the solid silver chloride AgCl product. When no more AgCl is produced, he filters, washes and weighs it, and finds that 1.28g has been produced. The balanced chemical equation for the reaction is: Cl−(aq) + AgNO3(aq) -> AgCl(s) + NO−3(aq) What kind of reaction is this? If you said this was a precipitation reaction, enter the chemical formula of the precipitate. If you said this was an acid-base reaction, enter the chemical formula of the reactant that is acting as the base. If you said this was a redox reaction, enter the chemical symbol of the element that is oxidized. Calculate the mass percent of Cl in the sample. Be sure your answer has the correct number of significant digits.
- CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) Solve the following: a. Calculate the molarity of hydrochloric acid, HCl, in a solution if 25.00 mL of that solution required35.74 mL of 0.1522 M KOH for complete neutralization in a titration. (Answer: 0.2176 M) b. When aqueous solutions of Ba(NO3)2 and K2SO4 are mixed, a precipitate of BaSO4 results. Writethe molecular, ionic, and net ionic equation for this double displacement reaction. c. 8.50 g of copper (II) sulfate pentahydrate, CuSO4∙5H2O, is dissolved in 250 mL of solution. Whatis the molarity of this solution?In the analysis of H2O2 using KMnO4, the simulation first states that about 20 mL of water is added to the 1.00 mL aliquot of H2O2 to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL H2O2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H2O2 in the original sample? Question 3 options: 10.00mL 20.00mL 11.00mL 21.00mL 1.00mLTwo solutions were made, the first one was made by dissolving 2.27 g of Co(NO3)2 in 100.0 mL of water. Then, to make the second solution, 5.00 mL of this solution was added to the 250 mL volumetric flask, which was filled to the mark with water. What was the molar concentration of the Co(NO3)2 in the two solutions?
- A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixtureYou have a solution containing two metal cations. You want to separate them by slowly and carefully adding a solution of an anion, until one metal cation precipitates as a compound with that anion, leaving the other metal cation still in solution. Your metal cations (M+ and M2+) and your anion M+= Cu^+ M^2+= Cd^2+ Anion= S^2- First Ksp(M+ w/anion)= 2.5 x 10-48 Second Ksp(M2+ w/anion)= 1.0 x 10-28 ----------------------------------------------------------------------------------- Starting concentrations of yourmetal ions in your initial solution: [M+]= 4.00 x 10-5 M [M2+]= 2.50 x 10-5 M Using these values, predict which metal will precipitate first, and at what concentration of anion the precipitation will begin. Clearly state the parameters of your particular problem at the beginning. What is M+, what is M2+, what are your concentrations, what are you solving for?To determine the percentage of bromide in a mixture containing a soluble bromide salt, the procedure from Experiment 10 is used except the bromide is precipitated with aqueous lead (II) nitrate, Pb(NO3)2, forming PbBr2(s). Initially, a 0.7893 g sample of an unknown bromide salt is dissolved in water. Excess Pb(NO3)2 is added to the solution to quantitatively precipitate the bromide from the solution. The resulting mixture is filtered through a piece of filter paper weighing 1.3587 g. After several days of drying, the filter paper and precipitate weighed 1.8257 g. Calculate the percent bromide in the original sample. Pb(NO3)2 Mw = 331.2 g/mol PbBr2 Mw = 367.0 g/mol