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- . You have been assigned to prepare 50.0 mL of a (1.0 %(v/v) solution in a volumetric flask from a 20.0% (v/v) Red Food Coloring (RFC) stock solution provided. a. Calculate the volume of Red Food Coloring you will need. b. What size of volumetric flask do you need? c. How do you transfer 20.0% of Red food coloring to volumetric flask? d. Describe the technique you use in diluting to volume?Zinc may be directly leached from zinc-lead sulphide concentrates by reaction with sulphuricPbS(s) + H2SO4 + 1 O2(g) → PbSO4(solid) + S° + H2O 21ZnS(s) + H2SO4 + 2 O2(g) → ZnSO4(aq) + S° + H2Oacid and oxygen. In addition, lead sulphide will be oxidized to give insoluble lead sulphate:Assume that a plant is to treat 400 t/day of concentrate containing 20.0 weight % Zn as ZnS and 110.0 weight % Pb and PbS. The concentrate and leach solution enters the leaching vessel at 32.0% solids. During the leach, 85.0% of the zinc is extracted and all the lead sulphide is oxidized. After the leaching step, the slurry passes to a thickener.(a) Calculate the concentration of Zn (in g/L) in the solution passing to metal recovery. Assume a solution density of 1.11 g/mL.(b) Calculate the tonnes per day of elemental sulphur produced.NOTE: â% solidsâ is the solids content of a slurry (consisting of particles and solution) and is defined as…If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)
- 2V is applied across an electrolytic cell containing 1.0M NaNO3. What reaction occurs at the anode? Show your work What reaction occurs at the cathode? Show your work Diagram the cell (assume the two electrodes are in 1 beaker). How many minutes does it take to form 10.0L of your anodic product measured at 99.8kPa and 28oC if a current of 1.3A is passed through the electrolytic cell?One kind of battery used in watches contains mercury(II) oxide. As current flows, the mercury(II) oxide is reduced to mercury. HgO(s) + H2O(l) + 2e– →Hg(l) + 2OH–(aq). If 2.3 ´ 10–5 amperes flows continuously for 1200 days, what mass of Hg(l) is produced?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…
- A medication order for a patient calls for 17 mEq of potassium chloride (MW 74.5, valence 1) in 1000 mL D5W. How many milliliters of a 10% w/v concentrated potassium chloride stock solution should be added to the D5W?Convert 61840 Coulombs to Faradays.Write the equation for the reaction, if any, that occurs when each of the following experiments is performed under standard conditions. (a) Sulfur is added to mercury. (b) Manganese dioxide in acidic solution is added to liquid mercury. (c) Aluminum metal is added to a solution of potassium ions.
- The amount of lactic acid, HC3H5O3, produced in a sample of muscle tissue was analyzed by reaction with hydroxide ion. Hydroxide ion was produced in the sample mixture by electrolysis. The cathode reaction is given below. 2 H2O(l) + 2 e− → H2(g) + 2 OH− (aq) Hydroxide ion reacts with lactic acid as soon as it is produced. The endpoint of the reaction is detected with an acid-base indicator. It required 104 s for a current of 13.1 mA to reach the endpoint. How many grams of lactic acid (a monoprotic acid) were present in the sample?Which of the following correctly describes the values of % AE and the E-factor for the synthesis of FeCl3 by the reaction below? 2 Fe + 3 Cl2 ⟶ 2 FeCl3Zinc(s) (MW=65.38), with a mass of 0.825 g, was reacted with 25.00 mL of NaClO (MW=74.44) according to the following unbalanced ionic equation. Determine the normality of NaClO.Zn(s) + ClO- → Zn(OH)2 + Cl- (in basic medium)