1) An aqueous solution of nitric acid is standardized by titration with a 0.182 M solution of barium hydroxide. If 20.5 mL of base are required to neutralize 26.0 mL of the acid, what is the molarity of the nitric acid solution?M nitric acid2) The hydronium ion concentration in an aqueous solution at 25°C is 8.8×10-2 M. The hydroxide ion concentration is M. The pH of this solution is .The pOH is . The reaction between ammonia and nitrous oxide is given below:2NH3(g) + 3N2O(g) → 4N₂(g) + 3H₂O(g)We therefore know that which of the following reactions can also occur?O4NH3(g) + 6NO(g) → 5N₂(g) + 6H₂O (1)O4N2(g) + 3H₂O(g) → 2NH3(g) + 3N₂O(g)O5N2(g) + 6H₂O(l) → 4NH3 (9) + 6NO(g)O None of the Above Consider the following reaction where K = 83.3 at 500 K:PC13(g) + Cl2(g) →PCI5(g)A reaction mixture was found to contain 4.66x10-2 moles of PCI3(g), 4.54×102 moles of Cl₂(g) and 0.127 moles of PCI5(g), in a 1.00 Liter container.Indicate True (T) or False (F) for each of the following:1. In order to reach equilibrium PCI-(g) must be produced.2. In order to reach equilibrium Kc must increase.3. In order to reach equilibrium PCI3 must be consumed.4. Qc is greater than K.5. The reaction is at equilibrium. No further reaction will occur.

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Answered: 1) An aqueous solution of nitric acid…

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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1) An aqueous solution of nitric acid is standardized by titration with a 0.182 M solution of barium hydroxide.

If 20.5 mL of base are required to neutralize 26.0 mL of the acid, what is the molarity of the nitric acid solution?

M nitric acid

2) The hydronium ion concentration in an aqueous solution at 25°C is 8.8×10^-2 M.

The hydroxide ion concentration is M.

The pH of this solution is .

The pOH is .

The reaction between ammonia and nitrous oxide is given below:
2NH3(g) + 3N2O(g) → 4N₂(g) + 3H₂O(g)
We therefore know that which of the following reactions can also occur?
O4NH3(g) + 6NO(g) → 5N₂(g) + 6H₂O (1)
O4N2(g) + 3H₂O(g) → 2NH3(g) + 3N₂O(g)
O5N2(g) + 6H₂O(l) → 4NH3 (9) + 6NO(g)
O None of the Above

Consider the following reaction where K = 83.3 at 500 K:
PC13(g) + Cl2(g) →PCI5(g)
A reaction mixture was found to contain 4.66x10-2 moles of PCI3(g), 4.54×102 moles of Cl₂(g) and 0.127 moles of PCI5(g), in a 1.00 Liter container.
Indicate True (T) or False (F) for each of the following:
1. In order to reach equilibrium PCI-(g) must be produced.
2. In order to reach equilibrium Kc must increase.
3. In order to reach equilibrium PCI3 must be consumed.
4. Qc is greater than K.
5. The reaction is at equilibrium. No further reaction will occur.

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