A 1.0 M solution of HNO3 was used to neutralize 100.0 mL of 0.20 M Ba(OH)2. Answer the following questions. (a) What was the initial concentration of hydroxide in the Ba(OH)2 solution? (b) How many ml of 1.0 M HNO3 are needed to neutralize 100.0 mL of 0.20 M Ba(OH)2? (c) What is the final concentration of Ba2+?
A 1.0 M solution of HNO3 was used to neutralize 100.0 mL of 0.20 M Ba(OH)2. Answer the following questions. (a) What was the initial concentration of hydroxide in the Ba(OH)2 solution? (b) How many ml of 1.0 M HNO3 are needed to neutralize 100.0 mL of 0.20 M Ba(OH)2? (c) What is the final concentration of Ba2+?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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- A 1.0 M solution of HNO3 was used to neutralize 100.0 mL of 0.20 M Ba(OH)2. Answer the following questions.
(a) What was the initial concentration of hydroxide in the Ba(OH)2 solution?
(b) How many ml of 1.0 M HNO3 are needed to neutralize 100.0 mL of 0.20 M Ba(OH)2?
(c) What is the final concentration of Ba2+?
Expert Solution
Step 1
A 1.0 M solution of HNO3 was used to neutralize 100.0 mL of 0.20 M Ba(OH)2.
We have to calculate : The initial concentration of hydroxide in the Ba(OH)2 solution.
And Volume of 1.0 M HNO3 are needed to neutralize 100.0 mL of 0.20 M Ba(OH)2.
And final concentration of Ba2+?
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