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Mercury can be toxic but its compounds (indeed, the metal itself) have many useful applications. Some examples include: tooth fillings (as an alloy with silver, copper and tin) and the industrial production of chlorine. However, some compounds must be removed from waste water due to their toxic properties such as mercury (II) nitrate. One way to remove this compound involves reacting the wastewater with sodium sulphide solution to produce a double displacement reaction. In order to test the effectiveness of this procedure, 0.020 L of 0.10 M mercury (II) nitrate reacts with 0.050 L of 0.010 M sodium sulphide. What is/are the limiting reactant(s)?
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- 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 mixtureOne 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 350.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 142.mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.One 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 200.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 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
- Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 50.mL of a 0.027M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.Part B MISSED THIS? Read Section 5.5 (Pages 179 - 183) ; Watch KCV 5.5, IWE 5.6. Complete and balance each of the following equations. If no reaction occurs, enter NOREACTION. NaI(aq) + Hg2 (C,H3 O2)2(aq) → Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer. ? xa X, b DA chemical reaction does not occur for this question. Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Part C (NH4)2SO4(aq) + SrCl2(aq) → Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer. ΑΣφ DA chemical reaction does not occur for this question. Submit Request Answer Part D Al2 (SO4)3 (aq) + A£NO3(aq) → Express your answer as a chemical equation. Enter NOREACTION if no reaction occurs. Identify all of the phases in your answer. - ΑΣφ ? DA chemical reaction does not occur for this question. Submit Request Answer Provide Feedback Next >Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50.mL of a 0.081 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
- One 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 300.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 67.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150.mL of a 0.060 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.Sodium hydrogen carbonate NaHCO3 , also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H2O (l) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150.mL of a 0.045 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits.
- Dilute the stock solution: Using the solutions in the burets, carefully measure the following quantities of Co(NO3)2 solution and water into 5 large test tubes, to a total of 5.00 mL in each test tube. Yes, the optional video says to make 10.00 mL total, but 5.00 mL is sufficient at this time and generates less waste. Use the buret to measure the cobalt solution and the water. Test tube No. 1 2 3 4 5 mL Co2+ Soln 1.00 2.00 3.00 4.00 5.00 mL H2O 4.00 3.00 2.00 1.00 0.00 Total mL 5.00 5.00 5.00 5.00 5.00 Mix each test tube thoroughly: hold the top of the tube and mix the bottom well. Transfer a portion of each diluted sample into a clean, dry sample cuvette. fill the concentration table and do calculations pleaseMercury as an amalgam with copper, silver, and tin is used fro fillings in teeth and in the production of chlorine. Soluble mercury compounds can be toxic and must be removed from wastewater. Aqueous mercury (II) nitrate is a toxic compound formed in wastewater and must be removed. To remove this compound, an aqueous sodium sulfide (Na2S) solution is added to wastewater to form a solid mercury (II) sulfide (HgS) precipitate and aqueous sodium nitrate in solution. From the analysis, 0.051 L of 0.010 M mercury (II) nitrate was reacted with 0.020 L of 0.10 M sodium sulfide. Write a balance equation for this chemical reaction. Determine the limiting reactant. How many grams of mercury (II) sulfide form? How many grams of excess reactant remain after the reaction is finished?One method for chemical analysis involves finding a reactant that will precipitate the species of interest, but not the other species. The mass of the precipitate is then used to determine the mass of the species of interest present in the original sample. For example, calcium ions can be precipitated from an aqueous solution by adding of sodium oxalate Na2C2O4. The balanced equation is: Ca2+(aq) + Na2C2O4 (aq) --> CaC2O4 (s) + 2 Na+ (aq) Suppose you had a solution with approximately 15.0 g of calcium ions. Show by calculation whether the addition of 15.0 g of sodium oxalate will precipitate all of the calcium ions present in the sample.
