A student forgot to add the mass of the unknown solute in trial 1 to the mass of the solute that was weighed for trial 2 and then added to the cyclohexane-solute solution used in trial 1. How would this omission affect the calculated molecular weight of the solute?
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A student forgot to add the mass of the unknown solute in trial 1 to the mass of the solute that was weighed for trial 2 and then added to the cyclohexane-solute solution used in trial 1. How would this omission affect the calculated molecular weight of the solute?
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- In this experiment, a series of solutions are prepared by combining multiple components into a single container. One solution prepared contains 5.00 mL of (1.1x10^-2) molar KI, 10.00 mL of 0.0010 molar Na2S2O3, 15.00 mL of water, 10.00 mL of (3.90x10^-2) molar KBrO3, and 10.00 mL of (1.000x10^-1) molar HCl. What is the concentration of iodide ions in this solution? Note: Your answer is assumed to be reduced to the highest power possible. When answering this problem, report the answer with the appropriate number of significant figures. Enter your answer USING scientific notation. When entering units, use proper abbreviated units with proper capitalizationAverage mass of the precipitate MgNH4PO4·6H2O (s) / g Average phosphate concentration in water sample (mass/volume %) % difference of 2 trialsPART B. Spectrophotometric Determination of the Copper Content of a Penny Mass of penny: 3.1848 Date on penny: 1964 Concentration of standard Cu2 solution: M Volume, Standard Volume, 1 M [Cu] (M) % Transmittance Absorbance Cu (mL) HNO, (mL) (use Eq. 4) 2. O.06 84.3% Test tube 1 0-074 O.IS 60.95% 0.215 Test tube 2 8. 3 0 244 45.3% 0.344 Test tube 3 300M 33.65% Standard O.473 Unknown 52.822 0-277
- In this experiment, you will take a 25.00 mL aliquot of vinegar and dilute it to 250.0 mL. You will then take a 25.00 mL aliquot from this diluted vinegar solution and titrate it against the standardised sodium hydroxide. The titration between acetic acid and sodium hydroxide is a 1:1 stoichiometry. If your standardised sodium hydroxide solution was determined to be 0.060 M, and it required an average titre (titration volume) of 20.3 mL, what is the concentration (in M) of the undiluted vinegar sample (the initial vinegar sample)? Provide your answer to 2 significant figures.You want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample? Solution: You must dilute approximately ten times, taking 10 mL of sample and making up to 100 mL. In this way, 17.20 mL of titrant will be spent.Based on this student data, calculate the average molarity of the NaOH solution. Standard: KHP = potassium hydrogen phthalate, MM 204.4 g/mol Student Data Trial 1 E KHP mL initial: NaOH mL final: NaOH 2.02 0.57 19.25 Trial 2 2.05 19.25 39.80 Trial 3 1.99 1.65 20.75
- Standard Sodium Chloride Weighed mass of NaCI g in 250.0 mL Purity of NaCl = 100.03 % Molar concentration of NaCl using weighed mass and purity mol L-1 Titrations of standard NaCI (25.00 ml aliquots) with the provided AGNO3 Precise Titration # Volume of AGNO3 required (mL) 1 2 3.What is the dilution factor if 10 µL of extract is added to 990 µL distilled water?a 50.0 mL sample of aqueous sodium chloride was analyzed according to the experimental procedure in part E and the following data were obtained. mass of evaporating dish: 37.628 g mass of evaporating dish + solution: 86.623 g mass of evaporating dish + solid NaCl: 41.133 g A) Calculate the percent by mass NaCl in the solution. B) Calculate the Molarity of the solution. C) Calculate the molality of the solution.
- Question 4. New December 18, 2020. The nitrite in a series of standard solutions (mg/L, n = 5) are converted to azo dye and the slope of the calibration curve is 2.0 ppm1. A 10.00-mL mineral water sample is treated in the same way as standards and diluted to a final volume of 100.00-mL. It gives an absorbance of 0.80. The absorbance of blank solution under the same conditions is 0.10. Calculate ppm (mg/L) of NO, (46 g/mol) and the molarity of NaNO2 (69 g/mol) in the original sample В ENG 10:23 PM UK 5/5/2021Details Preparation of Dilute Table Solution Molarity of I₂ Standard Solution Molar Mass (g/mole) Ascorbic Acid Number of Tablets per Analysis Mass (g) Container plus 1 Tablet Mass (g) Container less 1 Tablet Mass (g) of 1 Tablet Volume (mL) of Dilute Tablet Solution Titrimetric Analysis of Dilute Tablet Solution Volume (mL) of Aliquot Portion of Dilute Tablet Solution Titrated Final Buret Reading (mL) Initial Buret Reading (mL) Volume (mL) I₂ Solution Delivered No. of mmol 1₂ Reacted No. of mmol Ascorbic Acid in Aliquot Total No. of mmol Ascorbic Acid Present in the Volumetric Flask Total Mass (mg) of Ascorbic Acid Present in 1 Tablet Average Mass Ascorbic Acid/Tablet Deviation Standard Deviation Coefficient of Variation (%RSD) Reported Composition of Tablet Trial 1 50.00 11.64 0.20 0.02512 M 176.14 1 12.2546 11.7824 0.4722 250.00 Trial 2 50.00 22.80 11.64 Trial 3 250 mg Ascorbic Acid/Tablet 50.00 11.20 0.00 mg Ascorbic Acid/Tablet1. A 0.10 M HNO3 solution will be prepared from concentrated HNO3. a. Using the method outlined in Experiment 5, determine the concentration of a stock bottle of concentrated nitric acid. [density = 1.42 g/mL; 70% by mass HNO3] b. Calculate the volume of concentrated NO3 needed to prepare 500 mL of a 0.10 %3D M solution.