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    equilibrium shift of the reaction and the pH of solution

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    1. The pressure on each of the following systems is decreased from 5 atm to 1 atm. Which way does the equilibrium shift in each of the following systems?

    a.) 2CO2 (g) --> 2CO (g) + O2 (g)
    b.) H2 (g) + I2 --> 2HI (g)

    2. What is the pH of a solution if the H+ concentration is 7.2 X 10^-14 M?
    Is this neutral, acidic, or basic?

    3. Calculate pKa for the weak acid with a Ka value of 6.3 x 10^-3

    4. Classify the salt NaF as acidic, basic, or neutral? Write a net ionic equation to explain your answer.

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    Solution Preview

    1. The pressure on each of the following systems is decreased from 5 atm to 1 atm. Which way does the equilibrium shift in each of the following systems?

    a.) 2CO↓2 (g) ↔ 2CO (g) + O↓2 (g)

    The equilibrium constant is not changed if only the temperature is changed. It changes with temperature.
    Now assume the total pressure is denoted as P. Then (please see the attached file)
    , where xcO is ...

    Solution Summary

    This solution provides examples of determining the equilibrium shift of the systems. It also shows how to calculate the pH of the solution. The response is detailed and received a rating of '5/5' from the student who originally posted the question.

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