a) A 400 mL solution contains 0.138 g NaCl. Calculate the ppm concentration of NaCl. b) 32.0 g of concentrated solution that contains 57% w/w H₂SO, was diluted with water to 250 mL. Calculate. i. The %w/v concentration of H₂SO, in the diluted solution. ii. The molarity of H₂SO, in the diluted solution. c) Describe the preparation of 500 mL 0.25 M HNO, from 6.0 M HNO,

a) A 400 mL solution contains 0.138 g NaCl. Calculate the ppm concentration of NaCl. b) 32.0 g of concentrated solution that contains 57% w/w H₂SO, was diluted with water to 250 mL. Calculate. i. The %w/v concentration of H₂SO, in the diluted solution. ii. The molarity of H₂SO, in the diluted solution. c) Describe the preparation of 500 mL 0.25 M HNO, from 6.0 M HNO,

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 115QRT

See similar textbooks

Similar questions

Please answers this question. What is the molarity of a solution that contains 14.5 g of NaCl in 500. mL water? 2. How many moles of NaCl are present in 25.0 mL of 1.00 M NaCl? 3. If 15.00 mL of 2.00 M NaCl is diluted to 25.00 mL, what is the molarity of NaCl in the dilute. Thanks.
Hannah needs to make a solution of KMnO4 to be used in a chemistry experiment. On the shelf in her supply room is a bottle with 9.02 M KMnO4 already made. However, she only needs 9.8 mL of 1.01 M for her experiment. How many mL of WATER will she need to add to the 9.02 M solution to dilute it to the concentration she needs? [Hint - you will calculate how many mL of concentrated solution to use, and you know the total volume of solution.
5.300. mL of a 18.0 M solution of H2SO4 acid has enought water added to it to make a new volume of 1.00 L. What is the new concentration? Numerical answer: Unit: Label: Blank 1: Blank 2: Blank 3: 6.What is the concentration, in ppm, if 0.00021 g of Arsenic (As) was found in 3126 g of drinking water? Numerical answer: Unit: Label: Blank 1: Blank 2: Blank 3:
Concentrated hydrochloric acid has a concentration of 12.0 M. What volume of this solution should be used to prepare 3.42 L of 0.720 M HCl? Question options: a. 105 mL b. 205 mL c. 2.05 mL d. 20.5 mL
Please show your solution. Thank you! Question: A 100kg salt solution originally 4% by weight NaCl in water is evaporated until the concentration is 5% by weight NaCl. What percentage of the water in the original solution is evaporated?
1. Answer the following: a. the concentration of ammonia in the White River water sample was found to be 8 ppm (parts per million). Parts per million is another unit of concentration, typically used to describe very dilute solutions. Given that 1 ppm = 1 mg of solute per 1 kg of solution, convert 8 ppm of ammonia in the water sample to its concentration in molarity, assuming that 1 kg of solution = 1 L of solution. Hint: since 8 ppm = 8 mg of ammonia/1 kg of water sample, determine the moles of ammonia present in the water sample and convert 1 kg to L in order to calculate molarity. b. Several highly toxic substances were found in the White River, including heavy metal waste from plating solutions and sludge. These heavy metal ions (Cu 2+, Cr 3+, and Ni 2+) can be removed by reacting with sodium hydroxide to form insoluble metal hydroxides. Write balanced chemical equations for the following precipitation (double displacement) reactions: CuSO 4 + NaOH → Cr 2(SO 4) 3 + NaOH →…
Four different solutions were prepared in the laboratory. One was prepared by dissolving 28 g of potassium permanganate in enough water to make 200 milliliters of solution. Another was prepared by diluting 100mL of 5.8 molar of potassium permanganate solution to 500 mL. The third solution was prepared by aliquoting 5 mL each from the first two solutions and diluting it with 50mL. The fourth solution was prepared by adding thirty-five grams of potassium permanganate with 50 mL sample of the first solution and diluting it to 100mL. For the final solution, 18 mL aliquot from the first solution, 12 ml aliquot from the second solution 41 mL aliquot from the third solution and 19 mL of the fourth solution were mixed. * What is the molarity of the first solution? * Compute the molarity of the second solution. * How many molars is the third solution? * Determine the molarity of the fourth solution. * What is the concentration of the final solution?
Four different solutions were prepared in the laboratory. One was prepared by dissolving 28 g of potassium permanganate in enough water to make 200 milliliters of solution. Another was prepared by diluting 100ml of 5.8 molar of potassium permanganate solution to 500 mL. The third solution was prepared by aliquoting 5 mL each from the first two solutions and diluting it with 50mL. The fourth solution was prepared by adding thirty-five grams of potassium permanganate with 50 mL sample of the first solution and diluting it to 100mL. For the final solution, 18 mL aliquot from the first solution, 12 ml aliquot from the second solution 41 mL aliquot from the third solution and 19 mL of the fourth solution were mixed. What is the molarity of the fourt solution? What is the concentration of the final solution?
Part 1: A solution of sulfuric acid was made by dissolving 20.0g of 98% sulfuric acid in 250mL of water. (H2SO4 = 98.078 g/mol; H2O = 18.015 g/mol)Answer these items 1-4 for part 1:1. Express the concentration of this solution in % by weight. Additional information for items 2-3: What if the solution has a total volume of 262mL?2. Express the concentration in molarity3. Express the concentration in normality4. Express the concentration in molality Part 2: An alcohol, Ethanol (C2H5OH), is present in 1L of wine that is 12% alcohol by volume. The density of the solution is 0.984 g/mL, and the density of pure alcohol is 0.789 g/mL. (C2H5OH = 46.07 g/mol)Answer these items 1-2 for part 2:1. What is the weight of the alcohol present in wine?2. What is the molarity of the solution?
10 items multiple choice 20. What is the concentration, in mass percent, of a solution that contains 20.0 grams of NaCl dissolved in 250.0 grams of water? A. 6.76% B. 7.41% C. 8.00% D. 8.25% 21. Which of the following statements is TRUE for an unsaturated solution? A. Undissolved solute must be present. C. The solubility limit for solute has been reached. B. No undissolved solute may be present. D. Solid crystallizes out if the solution is stirred. 22. For which of the following solutions is the concentration 1.0 molar? A. 0.050 mol of solute in 25 mL solution C. 3.0 mol of solute in 1.5 L solution B. 2.0 mol of solute in 500 mL solution D. 0.50 mol of solute in 500 mL solution 23. Which is the measure of the mole of solute dissolved in a liter of solution? A. molality B. molarity C. normality D. mole fraction 24. What is the osmotic pressure is exerted by a 1.82 M solution at 18ᵒC? A. 43.48 atm B. 2.69 atm C. 1.0 atm D. 0.49 atm 25. It is the temperature at which a solution’s…
a) A 10.0mL sample of concentrated (pure) sulfuric acid (H2SO4) contains 17.7g of H2SO4. Determine the molarity of concentrated sulfuric acid. b) A hydrochloric acid (HCl) solution is prepared by dissolving 1.97g of hydrogen chloride gas in 27.3mL of water and then diluting that mixture to a total volume of 250.00mL. Calculate the molarity of the resulting solution. c) The concentration of NaClO in Clorox is 0.705M. Calculate the mass of NaClO present in 1.0mL of Clorox.
Typical seawater contains 2.7 g of salt (sodium chloride, NaCl) per deciliter (5 dL 5 0.1 L). What is the molarity of NaCl in the ocean? (b) MgCl2 has a typical concentration of 0.054 M in the ocean. How many grams of MgCl2 are resent in 25 mL of seawater?