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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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- The percent nitrogen (N) in a protein sample can be determined by reacting the protein with sulfuric acid to produce ammonium sulfate. The ammonium sulfate is reacted with concentrated sodium hydroxide to form ammonia gas. The ammonia gas is collected by bubbling it through a known volume of standardized hydrochloric acid solution (all of the ammonia reacts in this step, is consumed). The unreacted hydrochloric acid is then back-titrated with standardized sodium hydroxide solution. The reactions involved are shown below: Protein-N + H2SO4 (aq) ⟶⟶ (NH4)2SO4 (aq) 2 NH4+(aq) + 2 NaOH (aq) 2 NH3 (g) + 2 H2O NH3 (g) + HCl (excess) NH4Cl (aq) + HCl (unreacted) HCl (unreacted) + NaOH (aq) NaCl (aq) + H2OA 1.85 g sample of the protein required 25.00 mL of 0.1535 M HCl and 21.55 mL of 0.0986 M NaOH. How many moles of NH3 were consumed by the standardized HCl? A. 8.55 x 10-4 B. 1.71 x 10-3 C. 2.13 x 10-3 D. 3.84 x 10-3 E. 5.97 x 10-3 What is the mass percent nitrogen in…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)? Question 9 options: mercury (II) sulphide sodium sulphide mercury (II) nitrate & sodium sulphide mercury (II) nitrateMercury 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 sulfide. How many grams of mercury (II) sulphide form? Question 20 options: 0.039 g 0.12 g 0.47 g Not enough information to tell
- Copper metal and aqueous iron (III) chloride were made to react to reduce iron to Fe2+ whileoxidizing copper to Cu2+. What mass (in g) of copper metal is needed to react with 50 mL of 20.5wt.% iron (III) chloride (solution density is 2.9 g/mL)?Titration of 0.1756 grams primary standard sodium oxalate (134.00 g/mol) dissolved in 50 mL water with 5 mL concentrated sulfuric acid required 32.1 mL of a potassium permanganate solution. Which served as the reducing and oxidizing agent? What can be used as an indicator for thetitration? What is the molar concentration of the titrant? What is the total number of electrons involved in the redox reaction? What type of redox method was used?If there is a double displacement between calcium carbonate and hydrogen chloride to yield calcium chloride and carbonic acid. Carbonic acid is highly unstable and immediately falls apart into 1 molecule of water and 1 molecule of carbon dioxide. What would be the balanced equation for the reaction if needed here is the data The volume of HCl 26 mL Mass of beaker 51.9 g Mass of Beaker and Marble Chips 66.0 g Mass of Weighing boat 2.3 g Mass of Weighing boat and Unreacted Marble Chips 15.0 g
- To remove the tarnish (Ag2S) on a silver spoon the following steps are carried out. the spoon is placed in a large pan filled with water so the spoon was totally immersed. A few tablespoonfuls of baking soda (sodium bicarbonate), which readily dissolves. Is added. Some aluminum foil is placed at the bottom of the pan in contact with the spoon and then heated the solution to about 80° After a few minutes, the spoon is removed and rinsed with cold water. The tarnish is gone and the spoon regains its original shiny appearance. Describe with equations the electrochemical basis for the procedure. Adding NaCl instead of NaHCO3 would also work because both compounds arestrong electrolytes. What is the added advantage of using NaHCO3? (Hint: Consider the pH of the solution.) What is the purpose of heating the solution? Some commercial tarnish removers containing a fluid (or paste) that is a dilute HCl solution. Rubbing the spoon with the fluid will also remove the tarnish. Name two…Choi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. A. What is the…Choi is fond of carbonated beverages so he crafted his own soda formulation called “Sodalicious.” Ulan, who is a fellow enthusiast, also made her own formulation which she called “Soda Pop!” to challenge his friend Choi. To know which formulation is better, they sought to determine the carbonic acid content of their soda formulations using titration. In the first part of their experiment, a 0.5 Mlabeled NaOH solution was standardized against 0.350 grams of KHP (MW = 204.22 g/mol) primary standard that is 99.6% pure. The titration required 3.16 mL of the NaOH solution to reach the phenolphthalein endpoint. In the second part of their experiment, Choi and Ulan independently prepared their samples by taking 25.0-mL of their soda sample and diluting it to 30.0 mL. Using the same titrant and indicator, Choi’s “Sodalicious” required 1.39 mL of the standardized titrant to reach the endpoint, while Ulan’s “Soda Pop!” required 0.926 mL of the same titrant to reach the endpoint. D. Calculate…
- Zinc is one of the most valuable metals in the building and construction industry. One of the many ways to obtain zinc is to extract it from natural sources such as ores. The chief ore mineral of zinc is sphalerite (zinc sulfide). Zinc is extracted from sphalerite by performing the following steps: Step 1: The ore is reacted with oxygen gas at around 900ºC in a furnace to form a zinc oxide precipitate and sulfur dioxide gas.Step 2: The precipitate is then reacted with graphite (C(s)) to eventually produce solid zinc and carbon monoxide gas. A. Write the balanced chemical reactions for steps 1 and 2 separately. Indicate the states of the reactants and products (s, l, g). B. In step 2, is graphite acting as the reducing agent or the oxidizing agent? C. Calculate the theoretical yield of solid zinc if 432.4 grams of the sphalerite ore is made to undergo the extraction process outlined above. Express your answer in 4 significant figures. D. If in an actual extraction experiment, a chemist…Zinc is one of the most valuable metals in the building and construction industry. One of the many ways to obtain zinc is to extract it from natural sources such as ores. The chief ore mineral of zinc is sphalerite (zinc sulfide). Zinc is extracted from sphalerite by performing the following steps: Step 1: The ore is reacted with oxygen gas at around 900ºC in a furnace to form a zinc oxide precipitate and sulfur dioxide gas.Step 2: The precipitate is then reacted with graphite (C(s)) to eventually produce solid zinc and carbon monoxide gas. 2ZnS(s) + 3O2(g) -----> 2ZnO(s) + 2SO2(g) ZnO(s) + C(s) ----> Zn(s) + CO(g) a. If in an actual extraction experiment, a chemist obtained 180.0 grams of solid zinc, what is the %yield? Express your answer in 4 significant figures.b. A copper(II) sulfate solution was accidentally spilled into the final solid product obtained from the extraction experiment above. Write the balanced chemical equation for this reaction and identify the type of…Titration of 0.1756 grams primary standard sodium oxalate (134.00 g/mol) dissolved in 50 mL water with 5 mL concentrated sulfuric acid required 32.1 mL of a potassium permanganate solution. redox method used?Which served as the oxidizing agent? Which served as the reducing agent?What is the total number of electrons involved in the redox reaction?What can be used as an indicator for the titration?What is the molar concentration of the titrant?
