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3. Barium hydroxide reacts with phosphoric acid to form barium phosphate and water. Write the balanced equation for this reaction. Include states. a. 3 BalOH)a t e Hs POq IS) b. How many mL of 0.2195 M barium hydroxide would be required to titrate 12.57 mL 5M of phosphoric acid. The density of phosphoric acid is 1.834 g/mL.

3. Barium hydroxide reacts with phosphoric acid to form barium phosphate and water. Write the balanced equation for this reaction. Include states. a. 3 BalOH)a t e Hs POq IS) b. How many mL of 0.2195 M barium hydroxide would be required to titrate 12.57 mL 5M of phosphoric acid. The density of phosphoric acid is 1.834 g/mL.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need help with number b on number 3.
Ba 0 HIP 3 lo 2 EXPERIMENT 6 ACID-BASE TITRATIONS 12 14 Barium hydroxide reacts with phosphoric acid to form barium phosphate and water. Write the balanced equation for this reaction. Include states. 3. a. 3_ BalOH)a t ? Ho POa 1 3 b. How many mL of 0.2195 M barium hvdroxide would be required to titrate 12.57 mL of phosphoric acid. The density of phosphoric acid is 1.834 g/mL. BAOH = 0.2195 M 12.57mL HoPDn d=1.834 mL 4. A 10.00 mL sample of a solution of acetic acid in water was titrated to the endpoint by the addition of 15.89 mL of 0.2432 M NaOH. a. Calculate the molarity of the acetic acid solution. b. Calculate the grams of acetic acid present per liter of the unknown solution. c. Calculate the percent acetic acid in the solution. Assume the density of the solution is 1.00 g/mL. d. Calculate the volume of this NaOH solution that would be required to titrate 50.00 mL of vinegar. Vinegar is 5.00 % (by mass) acetic acid. Assume that the density of the vinegar solution is the same as that of water. 86
Transcribed Image Text:Ba 0 HIP 3 lo 2 EXPERIMENT 6 ACID-BASE TITRATIONS 12 14 Barium hydroxide reacts with phosphoric acid to form barium phosphate and water. Write the balanced equation for this reaction. Include states. 3. a. 3_ BalOH)a t ? Ho POa 1 3 b. How many mL of 0.2195 M barium hvdroxide would be required to titrate 12.57 mL of phosphoric acid. The density of phosphoric acid is 1.834 g/mL. BAOH = 0.2195 M 12.57mL HoPDn d=1.834 mL 4. A 10.00 mL sample of a solution of acetic acid in water was titrated to the endpoint by the addition of 15.89 mL of 0.2432 M NaOH. a. Calculate the molarity of the acetic acid solution. b. Calculate the grams of acetic acid present per liter of the unknown solution. c. Calculate the percent acetic acid in the solution. Assume the density of the solution is 1.00 g/mL. d. Calculate the volume of this NaOH solution that would be required to titrate 50.00 mL of vinegar. Vinegar is 5.00 % (by mass) acetic acid. Assume that the density of the vinegar solution is the same as that of water. 86
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