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17 Nov 2019
The volume added from a buret can typically be determined to the 0.05 or even 0.01 mL. True False After cleaning and filling your buret, you take an initial reading of the volume and determine it to be 0.15 mL. You add some of the solution to a beaker, and take a final reading of the buret at 27.90 mL. What volume of solution did you add to the beaker?" Suppose that you use the indicator phenolphthalein when performing this experiment. Phenolphthalein is clear in acidic solutions, and pink in basic solutions. What color would you expect the following solutions to be if phenolphthalein was present: 2500 mL of 0.100 M HCl pink 25.00 mL of 1.00 M NaOH clear An antacid table is added to 25.00 mL of 1.00 M HCl, then heated until it is dissolved. Alter the endpoint of the titration of the of the antacid/HCl solution with 1.00 M NaOH. Suppose an antacid is dissolved in 25.00 mL of 1.00 M HCI solution. The solution is titrated with 1.00 M NaOH solution. The endpoint of the titration is reached when 14.32 mL of NaOH solution have been added. How many moles of acid were neutralized by the antacid? Magenisum carbonate (MgCO_3) is a common active ingredient in antacids. Each mole of magnesium carbonate can neutralize two moles of acid. If one tablet neutralized 0.01 moles of acid, how many milligrams of active ingredient were in the tablet?
The volume added from a buret can typically be determined to the 0.05 or even 0.01 mL. True False After cleaning and filling your buret, you take an initial reading of the volume and determine it to be 0.15 mL. You add some of the solution to a beaker, and take a final reading of the buret at 27.90 mL. What volume of solution did you add to the beaker?" Suppose that you use the indicator phenolphthalein when performing this experiment. Phenolphthalein is clear in acidic solutions, and pink in basic solutions. What color would you expect the following solutions to be if phenolphthalein was present: 2500 mL of 0.100 M HCl pink 25.00 mL of 1.00 M NaOH clear An antacid table is added to 25.00 mL of 1.00 M HCl, then heated until it is dissolved. Alter the endpoint of the titration of the of the antacid/HCl solution with 1.00 M NaOH. Suppose an antacid is dissolved in 25.00 mL of 1.00 M HCI solution. The solution is titrated with 1.00 M NaOH solution. The endpoint of the titration is reached when 14.32 mL of NaOH solution have been added. How many moles of acid were neutralized by the antacid? Magenisum carbonate (MgCO_3) is a common active ingredient in antacids. Each mole of magnesium carbonate can neutralize two moles of acid. If one tablet neutralized 0.01 moles of acid, how many milligrams of active ingredient were in the tablet?
Irving HeathcoteLv2
26 Sep 2019