EXERCISE II- 21. A 2.00 -mL sample of a 0.100 M solution of KMNO, is mixed with 3.00 mL of a 0.800 M solution ofKMNO4 . Calculate the molarity of the final solution, assuming that the volumes are additive.2. 40.0 mL of a 0.150 M HCI solution is mixed with 60.0 mL of 0.200 M NaOH. Is the resulting solutionacidic, basic, or neutral? Calculate the molarity of the reactant which is in excess.3. (a) If 10.0 mL of H2SO4 (sp. Gr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should beadded to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SC4 = 98;SO3 = 80%3D%3D4. A 500-mL graduated flask contains 150 mL of 0.200 N H2SO4. By adding a more concentrated H,SO4,the solution is brought up to mark and after mixing is found to be 0.300 N. What was the normalityof the acid that was added?5. At 25°C, what changes in pH occur when (a) 0.0250 M HCI (b) 0.0250 M NaOH are dilutedwith water by a factor of ten? Assume solutions are ideal.

Answer: This question is based on the mixing of two solutions of different molar concentrations. To…

Answered: 1. A 2.00 -mL sample of a 0.100 M…

1. A 2.00 -mL sample of a 0.100 M solution of KMNO, is mixed with 3.00 mL of a 0.800M solution of KMNO4 . Calculate the molarity of the final solution, assuming that the volumes are additive.

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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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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EXERCISE II- 2
1. A 2.00 -mL sample of a 0.100 M solution of KMNO, is mixed with 3.00 mL of a 0.800 M solution of
KMNO4 . Calculate the molarity of the final solution, assuming that the volumes are additive.
2. 40.0 mL of a 0.150 M HCI solution is mixed with 60.0 mL of 0.200 M NaOH. Is the resulting solution
acidic, basic, or neutral? Calculate the molarity of the reactant which is in excess.
3. (a) If 10.0 mL of H2SO4 (sp. Gr. 1.50, containing 48.7% of combined SO3 by weight) is diluted to
400 mL, what is the normality of the solution as an acid? (b) What volume of 6.00 M H2SO4 should be
added to this in order to make the resulting mixture 1.00N as an acid? FW's : H2SC4 = 98;
SO3 = 80
%3D
%3D
4. A 500-mL graduated flask contains 150 mL of 0.200 N H2SO4. By adding a more concentrated H,SO4,
the solution is brought up to mark and after mixing is found to be 0.300 N. What was the normality
of the acid that was added?
5. At 25°C, what changes in pH occur when (a) 0.0250 M HCI (b) 0.0250 M NaOH are diluted
with water by a factor of ten? Assume solutions are ideal.

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