**Problem 5:**A titration is setup so that NaOH is in a buret and 25.0 mL of HBr solution is in a flask. The NaOH has a known molarity of 0.250 M. At the end point, 36.3 mL of NaOH has been added to the HBr solution. What is the molarity of the HBr?---**Problem 6:**A second titration is performed using the same 0.250 M NaOH in a buret. This time 25.0 mL of an H₂SO₄ solution is titrated. At the endpoint, 47.8 mL of NaOH has been added to the H₂SO₄ solution. What is the molarity of the H₂SO₄?

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(5) A titration is setup so that NaOH is in a buret and 25.0 ml of HBr soln is in a flask. The NaOH has a known molarity of 0.250 M. At the end point 36.3 mL of NaOH has been added to the HBr soln. What is the molarity of the HBr?

(5) A titration is setup so that NaOH is in a buret and 25.0 ml of HBr soln is in a flask. The NaOH has a known molarity of 0.250 M. At the end point 36.3 mL of NaOH has been added to the HBr soln. What is the molarity of the HBr?

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Chemistry In the burette there is 1.00 mol/L (it is written M) NaOH, this is the titrant. In the flask there is 100 mL of HBr, this is the sample. the average calculated titrant is 22.5 ml the balanced equation given is HBr+NaOH-NaBr+H2O Use the information given and the average calculated to complete the solution stoichiometry to calculate the concentration of the HBr sample.
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