A solution is prepared by dissolving 0.5892 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliquot (portion) of this solution is then diluted to a final volume of 250.0 mL. What is the final molarity of the diluted oxalic acid solution?
I do not know if the answer of 0.00187 or 1.87 x 10^ -3 is correct. It is incorrect in my perspective, so i do not expect that answer, if you think it is, explain why.
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A solution is prepared by dissolving 0.5892 g oxalic acid (H2C2O4) in enough water to make...
(10 pts) A solution is prepared by dissolving 1.239 grams of hydrochloric acid, HCI, in enough water to make 250.0 mL of solution. A 25.00 mL sample of this solution is diluted with water to a final volume of 100.0 mL. Now, you take 10.00 mL of that solution and dilute it to 100.00 mL What is the molarity of the final solution? (HCI 36.45 g/mol)
A solution is prepared by dissolving 17.75 g sulfuric acid, H2SO4, in enough water make 100.0 mL. What is the molarity? A) 1.940 M H2SO$ B) 0.1810 M H2SO4 C) 1.810 M H2SO4 D) 0.1775 M H2SO4
A sample of oxalic acid (a diprotic acid of the formula H2C2O4) is dissolved in enough water to make 1.00 L of solution. A 100.0 mL sample of this solution is titrated with a solution of sodium hydroxide of concentration 0.750 M and requires 20.0 mL of sodium hydroxide to reach the end point. Calculate the mass of the original oxalic acid sample.
A student prepared a solution of oxalic acid by sufficiently dissolving a dark chocolate bar in a 100-mL volumetric flask. In the experiment, 8.989-mL of 0.152 M NaOH was required to reach the equivalence point of a 10-mL aliquot of this oxalic acid solution. Assuming the average mass of a dark chocolate bar is 3.00-oz (and that oxalic acid is the only acid present in appreciable amounts), determine the % mass of Oxalic Acid in a normal dark chocolate bar.
A solution is prepared by dissolving 27.75 g sulfuric acid, H2SO4, in enough water to make exactly 200.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is 1. Weight % of H2SO4 in the solution? 2. Mole fraction of H2SO4 in the solution? 3. Molarity of H2SO4 in the solution? 4. Molality of H2SO4 in the solution?
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6. A solution is prepared by dissolving 571.6 g of H2SO4 in enough water to make 1000.0 mL of solution. The solution has a density of 1.3294 g/mL. Determine the molarity and molality of the solution.
A student prepared a stock solution by dissolving 5.00 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted itwith enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution?A) 0.137 MB) 7.30 MC)5.61 MD) 0.178 M
A barium hydroxide solution is prepared by dissolving 3.15 g of Ba(OH)2 in water to make 27.4 mL of solution. What is the concentration of the solution in units of molarity? concentration: M? If 30.0 mL of the barium hydroxide solution was needed to neutralize a 4.21 mL aliquot of the perchloric acid solution, what is the concentration of the acid? concentration:
3. Consider a solution prepared by dissolving 30.000 g of BaCl, in enough water to make a 200 ml solution. a. Determine the molarity of the BaCl, solution. b. Determine the molarity of Ba2+ ions. c. Determine the molarity of Chions. A chemist adds 800 mL of a 0.140 M NaCl solution to the existing 200 mL solution. d. Determine the new total volume of solution. e. Determine the new molarity of Ba2+ ions. f. Determine the new molarity of...