Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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This series demonstrates the addition of 0.25 M solution of lead (II) nitrate (??(?? ) ) to 0.5 M solution of potassium chromate (? ??? ).
1.What observations indicate that a chemical reaction has occurred? 2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?
This series demonstrates a drop-by-drop addition of 0.5 M barium chloride solution (???? ) to 0.5 M sodium carbonate solution (?? ?? 1.
1. What observations indicate that a chemical reaction has occurred?
2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?
VOLUMENTRIC ANALYSIS
Instructions: Answer each of the problems below by showing your solutions neatly and logically. Copy and answer each problem and please box your final answers.
4. If a 1.2500 g sample of zinc oxide, 95.0% ZnO were treated with 50.00 mL of 1.1230 N sulfuric acid in the usual way, what volume of 0.9765N sodium hydroxide would be required in the back titration.
NOTE: KINDLY WRITE THE SOLUTIONS ON A SEPARATE SHEET OF PAPER
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- Sulfuric acid is listed in a catalog with a concentration of 95-98%. A bottle of the acid in the stockroom states that 1.00 L has a mass of 1.84 kg. To determine the concentration of sulfuric acid in the stockroom bottle, a student dilutes 5.00 mL to 500. mL She then takes four 10.00-mL samples and titrates each with standardized sodium hydroxide (c = 0.1760 M). (a) What is the average concentration of the diluted sulfuric acid sample? (b) What is the mass percent of H2SO4 in the original bottle of the acid?arrow_forwardIn 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.arrow_forwardA student had 1.00 L of a 1.00-M acid solution. Much to the surprise of the student, it took 2.00 L of 1.00 M NaOH solution to react completely with the acid. Explain why it took twice as much NaOH to react with all of the acid. In a different experiment, a student had 10.0 mL of 0.020 M HCI. Again, much to the surprise of the student, it took only 5.00 mL of 0.020 M strong base to react completely with the HCl. Explain why it took only half as much strong base to react with all of the HCl.arrow_forward
- A student performed an experiment on the determination of dissolved oxygen in a water sample using the Winkler Titration Method. What is the amount of (A) dissolved oxygen and (B) oxygen in the water sample? Use the data and results recorded by the student in the table below. (A) What is the amount of dissolved oxygen in the water sample? * a) 4.0864 mg/L b)0.4085 mg/L c)2.6198 mg/L d)0.2620 mg/L (B) What is the amount of oxygen in the water sample? * a)4.0864 mg b)0.4085 mgc)2.6198 mg d)0.2620 mgarrow_forwardIn the first part of this experiment, sodium percarbonate will be dissolved in water: Na2CO3·n H2O2(s) → 2 Na+(aq) + CO32–(aq) + n H2O2(aq) The hydrogen peroxide thus generated will be consumed by iodide and sulfuric acid: H2O2(aq) + 2 H+(aq) + 3 I– → 2 H2O(l) + I3–(aq) Finally, the triiodide anion will be consumed by added thiosulfate: 2 S2O32–(aq) + I3–(aq) → S4O62–(aq) + 3 I–(aq) Considering these chemical equations, if 0.437 millimoles of thiosulfate were needed to completely consume all of the triiodide generated in reaction 2, how many millimoles of hydrogen peroxide were present in the original sodium percarbonate sample?arrow_forwardIn the first part of this experiment, sodium percarbonate will be dissolved in water: Na2CO3·n H2O2(s) → 2 Na+(aq) + CO32–(aq) + n H2O2(aq) The hydrogen peroxide thus generated will be consumed by iodide and sulfuric acid: H2O2(aq) + 2 H+(aq) + 3 I– → 2 H2O(l) + I3–(aq) Finally, the triiodide anion will be consumed by added thiosulfate: 2 S2O32–(aq) + I3–(aq) → S4O62–(aq) + 3 I–(aq) Considering these chemical equations, if 0.416 millimoles (mmol) of thiosulfate were needed to completely consume all of the triiodide generated in reaction 2, how many millimoles of hydrogen peroxide were present in the original sodium percarbonate sample? Enter your response to the nearest 0.001 mmol.arrow_forward
- A student used a pipette to place 25.00 mL of HCl into an Erlenmeyer flask. Then the student diluted the acid with distilled water and added a few drops of phenolphthalein to the flask. The sample was titrated with a sodium hydroxide solution until a faint pink color became permanent. The procedure was repeated 4 more times. The following results were obtained: Volumes of NaOH used for each trial: Trial 1 37.22 mL Trial 2 36.14 mL Trial 3 36.13 mL Trial 4 36.15 mL Trial 5 36.12 mL Which of the following is the most probable explanation for the variation in the student's results for Trial 1? A. Water in the pipette B. Water in the burette C. Water in the flask D. Misread a 7 for a 6 on the burette.arrow_forwardA stock solution of 8uM dye is provided. While making one of the standard solution, a student records: Initial buret reading: 2.46, DI water: 1.48 Final buret reading 8.68, DI water 6.44 What is the concentration of the dye in the standard?arrow_forwardThe reaction between lead(II) nitrate and potassium iodide solution is shown below Pb(NO3)2(aq) + 2 KI(aq) → 2 KNO3(aq) + PbI2 Calculate the mass of lead(II) iodide precipitated when 5.00 cm3 of 4.00 mol dm–3 lead(II) nitrate solution is mixed with 7.50 cm3 of 5.00 mol dm–3 potassium iodide solution. [Mr / g mol–1: PbI2 = 461.01]arrow_forward
- Initial Volume of Vinegar: 0.01 mL Final Volume of Vinegar: 15.18mL Initial Volume of NaOH: 0.21 mL Final Volume of NaOH: 24.30mL Molarity of NaOH: 0.50M Using this data, for this trial what was the molarity of acetic acid in vinegar?arrow_forwardThe reaction of perchloric acid (HClO4) with lithium hydroxide (LiOH) is described by theequation:HClO4 + LiOH → LiClO4 + H2OSuppose 100 mL of perchloric acid is neutralized by exactly 46.9 mL of 0.75 M lithiumhydroxide. What is the concentration of the perchloric acid? A. 0.35 MB. 0.47 MC. 0.63 MD. 1.60 Marrow_forwardIf your concentrations of acetic acid and sulfuric acid were the same, would you have to add the same or different amounts of titrant? Explain your answer using the chemicals formulas and the acid/base neutralization reactions involved in this experiment. Molarity acetic acid: 0.985 Molarity of Sulfuric acid: 0.519Marrow_forward
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY