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- Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?The titration of 0.314 g of potassium hydrogen phthalate (KHP) requires 13.16 mL of a NaOH solution. What is the molarity of the NaOH solution?5. Suppose there was a large air bubble in the tip of the acid burette during the titration and it was dislodged toward the end of your titration. Explain the effect that this would have on the calculated value of the acid's molarity. 6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially filled to the 2.30 mL mark on the burette. Once the level in the burette reached 50.00 mL, the student wasforced to refill the burette and did so to the 5.06 mL mark. The endpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on the burette. What is the molarity of the acid solution? Show work. 7. How many milliliters of a 0.250 M sulfuric acid solution would be required to completely react with 2.398 grams of solid aluminum hydroxide? Work must be shown.
- For an experiment, I titrated NaOH with an unknown sample that had acetylsalicylic acid. In my few trials I found the average concentration and moles for the NaOH and asked to find the mass of acetylsalicylic acid in the sample I measured. How do I do that?In an experiment, a 500.0 mL solution of approximately 0.250 M KOH (56.106 g/mol) solution was prepared. The actual concentration was then determined by standardizing against 1.0050 g of KHP (204.22 g/mol), which required 19.45 mL of the KOH solution. One mole of KOH reacts with one mole of KHP. How would you prepare the KOH solution? After standardization, what will be the exact molarity of the KOH solution? The KOH solution was then used to analyze a sample containing oxalic acid, H2C2O4 (90.03 g/mol). If the titration required 11.33 mL KOH, how many grams of oxalic acid is in the sample? Oxalic acid releases two protons during the reaction.For a tablet containing 1000 mg of vitamin C, calculate the minimum concentration of the NaOH solution so that the titration would take no more than 45.00 mL of the NaOH from the buret.
- Your lab assignment presentation involves putting together a presentation to show other students on how to perform titration. In other words, your presentation can be used to show other students (next term) how they can perform a titration by following your instructions and calculations. To do this presentation, we are giving you the type of acid, acetic acid, the type of base, NaOH to be used, and you will use phenolphthalein as the indicator. You will use the data given to you to be used as an example of how to solve the mathematical calculations. At the end of your presentation, you will show the unknown concentration of the acetic acid (Molarity) and will also show the % mass/ vol of the Vinegar solution. Part 1 Purpose of a titration, what is titration and why do we perform a titration? Instrumentation- what are the instruments, glassware used when performing a titration. Chemicals and Procedures. What chemicals are needed? List and explain the procedures for this experiment.…In the titration of a solution of sodium hydroxide, an acid titrant was prepared by diluting 125.0 mL of 10.00 mol/L nitric acid into enough distilled water to make 500.0 mL of solution. 30.00 mL of the base was measured, and in the titration, 16.74 mL of the acid titrant was needed to neutralize. Determine the concentration of the sodium hydroxide solution. Previous Page Next Page Page 5 of 5A student used a titration to determine the concentration of acetic acid in vinegar. The vinegar was first diluted with distilled water and samples of the diluted solution were then titrated with sodium hydroxide solution. The titration value was more than expected. Which of the following actions can account for this observation? * A- The inside of the volumetric flask used to prepare the diluted vinegar was rinsed with water and not dried properly prior to use. B- The sodium hydroxide solution had been allowed to stand exposed to air for a long time prior to the titration. C- The inside of the burette used to deliver the sodium hydroxide solution was rinsed with water and not dried properly prior to use. D- None of these actions will increase the titration value. E- All these actions will increase the titration value.
- Write the balanced chemical reaction showing the neutralization of aqueous hydrochloric acid with aqueous sodium hydroxide.Which of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in acidic solution? O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming water and thereby decreasing the concentration of hydroxide ions in solution causing more magnesium hydroxide to dissolve. O Magnesium hydroxide does not dissolve in acidic solutions. O According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming magnesium hydride and causing more magnesium hydroxide to dissolve. O According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide ions and thereby decreasing the concentration of magnesium ions in solution causing more magnesium hydroxide to dissolve. O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a precipitate.A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain
