A reagent of known concentration that is often placed inside a buret titrant Chemicals are sold and classified based on their % purity. Arrange the following classifications according to increasing % purity. 1. Chemically pure (CP) II. Primary standard III. Reagent-grade a. l< ll
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- 1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/LA (aq) + ...B(aq) C(s) + D (aq) ... .. Experimental | Volume of B/ mL Mass of Run precipitate/g 1 1.2 5.40 2 1.4 7.24 1.6 9.02 4 1.8 9.90 2.0 10.86 6. 2.2 10.90 7 2.4 10.88 8 2.6 10.84 9. 2.8 10.86 A series of experiment was performed to determine the mole ratio of a given reaction. 1 mL of 1 Molar A added to nine beakers, then the increasing amount of 1 Molar B added to these beakers. Volume of B and mass of precipitate of C are given in the table below. Find the mole ratios through plotting a graph.B. Weight of Na2SO4 Sample 0.3512 g C. Total Vol. of Precipitant (BaCl2) used WITH 1M BaCl2 PLEASE FIND THE calculated volume of BaCl2 precipitant will be calculated using this formula: NVBaCl2 = (weight of sample)(1000)(EW) V(ml)BaCl2 = (weight sample)(1000)N(EW).
- Please answer all parts5. From the stock solutions of 1.00-mol L acetic acid and 1.00-mol L of sodium acetate, six solutions were prepared with the acetic acid and acetate concentrations shown in the table below. The pk of acetic acid is 4.756. [Acetic acid). [Acetate). Final volume, Solutio mol L mol L ml A. 0.10 100 0.0000351 100 0.10 0.10 100 0.010 0.010 100 0.10 0.15 100 0.15 0.10 100 -1 Determine the volume of the stock solutions of 1.00-mol Lacetic acid and 1.00-mol L of sodium acetate needed to prepare the solutions. Write your answer in the table below. a. Vol. acetic acid, ml Vol. of acetate, ml Solution A b. Calculate for the initial pH of the solutions and write the pH in the table below. Solution Initial pH A Which solution(s) have the same pH? C.Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and no precipitate forms. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and no precipitate forms. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube remains red. Select the ions present. Question 5 options: Ba2+ Ca2+ Mg2+ NH41+
- Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and no precipitate forms. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and no precipitate forms. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube turns blue. Select the ions present. Question 4 options: Ba2+ Ca2+ Mg2+ NH41+M req M #3 80 E D Solid barium chloride is slowly added to 75.0 mL of a 0.205 M sodium carbonate solution until the concentration of barium ion is 0.0440 M. The percent of carbonate ion remaining in solution is %. Submit Answer C $ 4 000 888 R F % 5 V [References Use the References to access important values if needed for this question. Retry Entire Group T Cengage Learning | Cengage Technical Support G 6 6 more group attempts remaining MacBook Pro B Y H & 7 U N 11 * +00 8 J 1 M ( - 9 K O ) 0 I 2 L P command Previous Email Instructor { + 11 [ Next Save and Exit 27 option ? 1 ] dele9. An aqueous solution of sulfuric acid is prepared by mixing a secondary standard of sulfuric acid with deionized water. The aforementioned acid is to be used as a titrant hence its concentration must be accurately determined. To do this, Engr. Polinar, standardized the titrant by titrating two liters of ammonia at 0.90 atm and 30 deg C. From the experiment, 134 mL of the titrant was necessary to neutralize the ammonia. Determine the concentration of the acid in terms of normality? 10. Engr. Forcadela is optimizing a plastic formulation by manipulating the phosgene concentration injected as a gas during the reaction. To obtain credible results, he considered the propensity of phosgene to dissociate into carbon monoxide and chlorine gas at 395 deg C. Performing an experiment at the aforementioned temperature, an equilibrium is reached amongst the species where the total pressure is at 3 atm. If the equilibrium constant expression in terms of concentration for the reaction at 395 deg C…
- Please help me2 Trial 1: [4] Volume of NaOH, dispensed (mL) Trial 1: [5] Molar concentration of NaOH (mol/L) Trial 2: [4] Volume of NaOH, dispensed (mL) How Trial 2: [5] Molar concentration of NaOH (mol/L) Trial 3: [4] Volume of NaOH, dispensed (mL) Trial 3: [5] Molar concentration of NaOH (mol/L)Gravimetric analysis of Fe3O4 (MW = 232 g/mole) may be undertaken with the following reactions: Fe3O4 → Fe2O3 → Fe (OH)3. Weight of sample containing 8.00% Fe3O4 that must be taken to obtain a precipitate of Fe(OH)3 (MW = 107 g/mole) that weighs 150 mg is . a. 0.108 g b. 0.325 g c. 1.355 g d. 4.065 g Amount of Fe2O3 (MW = 160 g/mole) from which 150 mg of Fe(OH)3 (MW = 107 g/mole) may be obtained is . a. 0.112 g b. 0.224 g c. 0.448 g d. none of the other choices