. A 20.0g sample of NaCl was dissolved in 125mL of water (density = 1.00g/mL). Calculate the weight percent concentration (w/w) of NaCl in the resulting solution. Remember to calculate the total solution mass! a. 86.2 b. 19.0 c. 16.0 d. 13.8 e. no correct response
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. A 20.0g sample of NaCl was dissolved in 125mL of water (density = 1.00g/mL). Calculate the weight percent concentration (w/w) of NaCl in the resulting solution. Remember to calculate the total solution mass!
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- Which of the following statements concerning a saturated solution is incorrect? a. undissolved solute must be present b. undissolved solute may or may not be present c. undissolved solute, if present, is in equilibrium with dissolved solvent d. no correct responseAdding a nonvolatile solute to a pure solvent produces which of the following effects? a. vapor-pressure lowering b. freezing-point elevation c. boiling-point depression d. no correct responseFigure 1:Experimental results Mass of empty weighing dish,g 2.2522g Mass of weighing dish + CaCl2 · 2H2O,g 6.2540g Mass of CaCl2 · 2H2O, g 4.0018g [Na₂CO₃], mol⋅L−1 0.3330 mol⋅L−1 Volume of the CaCl2 solution used, mL 10.00mL Volume of the Na₂CO₃ solution used, mL 10.00mL Mass of the filter paper + watch glass, g 51.3999g Mass of the filter paper + watch glass + dry product (final), g Weight 1=51.7235g Weight 2=51.7058g Figure 2:Calculated data Mass of dry product, g 0.3059g Moles of CaCl2 used, mol 0.02721mol Moles of Na₂CO₃ used, mol 0.02721mol [CaCl2], mol⋅L−1 0.3330 mol⋅L−1 Limiting reagent Calculated mass of excess reagent remaining in the mixture after reaction, g Theoretical yield, g % yield I need help in my lab. The number of mols of cacl2 and na2co3 gives me the same number. If I need to calculate the limiting reagent, how would I be able to do that if they have…
- What is the concentration of NaOH (sodium hydroxide), in ppm (m/m), in a solution prepared by dissolving 32 mg of NaOH in 5.8 kg of water? Report your result in decimal notation and to the proper number of significant figures. All numbers are measured. a) 0.18 ppmb) 1.8 ppmc) 0.55 ppmd) 5.5 ppme) no correct response(a) During the analysis of water sample by argentometric titration, results obtained are as follows: Experiment1 2 3 4 Volume 15.5, 15.2 ,15.1 ,15.4 A)Calculate average deviation and relative average deviation for the given data. (b)Calculate the molecular weight of an unknown acid if 8.5 g of it is dissolved in 200.0 ml of water and requires 50.0 ml of 1.5 M sodium hydroxide for complete neutralization .When 60.0 mL of a 1.00 M solution is diluted by adding 30.0 mL of water, the amount of solute present a. increases b. decreases c. remains the same d. no correct response
- ab experiment by adding drops of KMno4 to a solution of distilled water and Iron (II) ammonium sulfate. I measured the iron ammonium sulfate in grams and added the same amounts into two flasks. I then added 25mL of distilled water and mixed. Then I added 5 mL of H2SO4 (sulfuric acid) into the solution. After that, I slowly added drops of KMno4 until the solution turned a pink color (reached end point). I measured the initial and final volume of KMno4. What would be the balanced equation for this reaction? How can I find the moles of KMno4 solution needed to react with all of the 0.100M FeSO4 solution? How do I calculate the molarity of KMno4?PROCEDURE 1000 mg L-asocrbic acid tablet (pulverized into fine powder) Molar mass of tablet = 176.12 g/mol 1. Add the necessary amount of distilled water to make the desired concentration of stock solution. [Note: Assume that the volume of the solute is negligible compared to the volume of the solution.] Concentration of STOCK SOLUTION, M Concentration of DILUTED SOLUTION, M 0.8 M 0.16 M 2. Mix and stir the powder with the distilled water until homogeneous. 3. Get ready for the dilution. Refer to the table above. 4. Compute and add more solvent to achieve the desired dilution. Use the prepared stock solution to prepare an aliquot assigned to your group. Make sure to place the computations used for dilution (C1V1 = C2V2) in the data sheet. 5. After dilution, label the aliquot with its concentration and total volume of solution. 6. Complete the data sheet with relevant solutions in solving for the amounts needed in the experiment. PLEASE FILL IN THE MISSING TABLES IN THE DATA…PROCEDURE 1000 mg L-asocrbic acid tablet (pulverized into fine powder) Molar mass of tablet = 176.12 g/mol 1. Add the necessary amount of distilled water to make the desired concentration of stock solution. [Note: Assume that the volume of the solute is negligible compared to the volume of the solution.] Concentration of STOCK SOLUTION, M Concentration of DILUTED SOLUTION, M 0.8 M 0.16 M 2. Mix and stir the powder with the distilled water until homogeneous. 3. Get ready for the dilution. Refer to the table above. 4. Compute and add more solvent to achieve the desired dilution. Use the prepared stock solution to prepare an aliquot assigned to your group. Make sure to place the computations used for dilution (C1V1 = C2V2) in the data sheet. 5. After dilution, label the aliquot with its concentration and total volume of solution. 6. Complete the data sheet with relevant solutions in solving for the amounts needed in the experiment. PLEASE FILL IN THE MISSING TABLES IN THE DATA…
- Test Data: Part 1: Preparation of the Primary Citric Acid Standard Mass of empty 250-mL glass beaker: 100.7g Mass of 250-mL beaker and anhydrous citric acid First weighing : 103.4 g Second weighing: 106.1 g Third weighing 3. Total volume of citric acid solution: 75.0 mL help me with this part Part 1: Preparation of the Primary Citric Acid Standard Mass of Citric Acid _________________________ Volume of Citric Acid Solution ____________ Moles of Citric Acid _________________ (Molar Mass = 192.0 g/mol) Molarity of Citric Acid Solution ____________The word like in the solubility rule like dissolves like refers to a. like polarity b. like physical state c. like boiling point d. no correct responseAn EDTA solution was prepared by dissolving the disodium salt in 1 L of water. It was standardized using 0.5063 gram of primary standard calcium carbonate (MM: 100.08) and consumed 28.50 mL of the solution. The standard solution was used to determine the hardness of a 2 L sample of mineral water, which required 35.57 mL of EDTA solution. 1. What is the analyte in the analysis? Answer 2. What is concentration (M) of the EDTA solution used in the analysis? Answer 3. What is the concentration (ppm) of CaCO3 in the sample?