A solution is prepared that is initially 0.090M in pyridine (CHN), a weak base, and 0.50M in pyridinium bromide (C-H5NHBr). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH-]. You can leave out the M symbol for molarity. initial change final [C₂H₂N] [C₂H₂NH*] 0 0 0 [OH-] 0 0 X
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Bronsted Lowry Base In Inorganic Chemistry
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![A solution is prepared that is initially 0.090 M in pyridine (C\(_5\)H\(_5\)N), a weak base, and 0.50 M in pyridinium bromide (C\(_5\)H\(_5\)NHBr). Complete the reaction table below, so that you could use it to calculate the pH of this solution.
Use \( x \) to stand for the unknown change in [OH\(^-\)]. You can leave out the \( M \) symbol for molarity.
\[
\begin{array}{|c|c|c|c|}
\hline
& [\text{C}_5\text{H}_5\text{N}] & [\text{C}_5\text{H}_5\text{NH}^+] & [\text{OH}^-] \\
\hline
\text{initial} & & & \\
\hline
\text{change} & & & \\
\hline
\text{final} & & & \\
\hline
\end{array}
\]
In the table above, fill in the initial concentrations and indicate the changes using \( x \) where appropriate. Use these changes to determine the final concentrations, helping calculate the pH of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabd5e741-0235-409f-80de-883f5f0e5da7%2F919e8d85-95ff-4b85-934e-e0bf75510695%2Fu2kn14v_processed.jpeg&w=3840&q=75)
Given,
Initial,
molarity of C5H5N = 0.090 M
molarity of C5H5NH+ = 0.50 M
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