A solution is prepared at 25 °C that is initially 0.31M in nitrous acid (HNO₂), a weak acid with K-4.5 x 104, and 0.059 M in potassium nitrite (KNO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = X

A solution is prepared at 25 °C that is initially 0.31M in nitrous acid (HNO₂), a weak acid with K-4.5 x 104, and 0.059 M in potassium nitrite (KNO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = X

Chemistry

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Author:Steven S. Zumdahl

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Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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A solution is prepared at 25 °C that is initially 0.31M in nitrous acid (HNO₂), a weak acid with K-4.5 x 104, and 0.059 M in potassium nitrite (KNO₂).
Calculate the pH of the solution. Round your answer to 2 decimal places.
pH =
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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 104) and 0.150 M CH3CH2COOH (Ka = 1.34 105). Calculate the pH of this solution. Because both acids are of comparable strength, the H+ contribution from both acids must be considered.