9. ( 2 points) Calculate the molar concentrations of the unknown ionized product of water and its pH. Indicate whether these solutions are neutral, acidic or basic.\begin{tabular}{|c|c|c|c|}\hline[H3O+] & {[OH−]} & pH & Acidic/basic/neutral \\\hline 1.3×10−13 & 7.7×10−2 & 13 & basic \\\hline 1.00×10−6 & & & \\\hline\end{tabular}
Q. 9. ( 2 points) Calculate the molar concentrations of the unknown ionized product of water and its pH. Indicate whether these solutions are neutral, acidic or basic.\begin{tabular}{|c|c|c|c|}\hline[H3O+] & {[OH−]} & pH & Acidic/basic/neutral \\\hline 1.3×10−13 & 7.7×10−2 & 13 & basic \\\hline 1.00×10−6 & & & \\\hline\end{tabular}
Analyze Data for First Solution: Step 1: Analyze the given data for the first solution.Given: [H3O+]=1.3×10−13M, [OH−]=7.7×10−2M, pH=13.Check if the product of [H_3O^+]\(\newline) and \$[OH^-]\(\newline\)) equals \$10^{-14}\) (the ion product of water at \(25\)\(\degree\)C).\(\newline\)Calculation: \((1.3 \times 10^{-13}) \times (7.7 \times 10^{-2}) = 1.001 \times 10^{-14}\).
Determine Solution Nature: Step \(2\): Determine the nature of the solution based on pH. \(\newline\)\(pH = 13\), which is greater than \(7\).\(\newline\)This indicates a basic solution.
Analyze Data for Second Solution: Step \(3\): Analyze the given data for the second solution.\(\newline\)Given: \([\text{H}_3\text{O}^+] = 1.00 \times 10^{-6} \, \text{M}\).\(\newline\)To find \([\text{OH}^-]\), use the ion product of water.\(\newline\)Calculation: \([\text{OH}^-] = 10^{-14} / [\text{H}_3\text{O}^+] = 10^{-14} / 1.00 \times 10^{-6} = 1.00 \times 10^{-8} \, \text{M}\).
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