More Examples• How many grams of ammonia are dissolved in 1.34 L ofwater at 25 °C if the pressure of NH3 above the water is0.250 atm? The Henry's constant for NH3 in water at 25 °Cis 5.8 M/atm.• Mixture of two gases, carbon dioxide and nitrogen exhibit atotal pressure of 0.30 atm above 2.00 L of water at 25 °C.The water has 20.00 mg of nitrogen and 41.01 mg of carbondioxide dissolved in it. What is the molar composition ofthis gas mixture? The Henry's constants for carbon dioxideand nitrogen in water at 25 °C are 0.034 M/atm and6.1x10 M/atm respectively.• Carbon dioxide has Henry's Law constant 0.034 M/atm.What volume of the solution (in mL) will be needed todissolve 4.40 g of this gas under a pressure of 1.25 atm?

Amount of ammonia dissolved can be figure out from the concentration of solution. Note: As you…

Answered: How many grams of ammonia are dissolved…

How many grams of ammonia are dissolved in 1.34 L of water at 25 °C if the pressure of NH3 above the water is 0.250 atm? The Henry's constant for NH3 in water at 25 °C is 5.8 M/atm.

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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Concept explainers

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.

Question

More Examples
• How many grams of ammonia are dissolved in 1.34 L of
water at 25 °C if the pressure of NH3 above the water is
0.250 atm? The Henry's constant for NH3 in water at 25 °C
is 5.8 M/atm.
• Mixture of two gases, carbon dioxide and nitrogen exhibit a
total pressure of 0.30 atm above 2.00 L of water at 25 °C.
The water has 20.00 mg of nitrogen and 41.01 mg of carbon
dioxide dissolved in it. What is the molar composition of
this gas mixture? The Henry's constants for carbon dioxide
and nitrogen in water at 25 °C are 0.034 M/atm and
6.1x10 M/atm respectively.
• Carbon dioxide has Henry's Law constant 0.034 M/atm.
What volume of the solution (in mL) will be needed to
dissolve 4.40 g of this gas under a pressure of 1.25 atm?

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