pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H], of a solution: pH = -log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the K of water: K = [H+][OH-] = 1.00 × 10-¹4 where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 pH + pOH Submit ✔ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. Part B 0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. What is the pH of this solum Express the pH numerically to two decimal places. View Available Hint(s) pH = 11.45 Buben't Previous Answers Part C ✓ Correct Because the concentration had two significant figures, the pH has two digits after the decimal point. POH = Previous Answers What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. Submit VG ΑΣΦ Request Answer ?

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### pH of a Strong Acid and a Strong Base

**pH Definition:**
pH is a logarithmic scale used to indicate the hydrogen ion concentration, \([H^+]\), of a solution:

\[ \text{pH} = -\log[H^+] \]

**Relationship Between pH and pOH:**
Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, \([OH^-]\), are related to each other by the ion product constant of water, \(K_w\):

\[ K_w = [H^+][OH^-] = 1.00 \times 10^{-14} \]

Here, \(1.00 \times 10^{-14}\) is the value at approximately 297 K. Based on this relationship, pH and pOH are related as follows:

\[ 14.00 = \text{pH} + \text{pOH} \]

---

**Part B: Calculating pH**

0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. To find the pH of this solution, express the pH numerically to two decimal places. The calculated pH is:

\[ \text{pH} = 11.45 \]

The answer is marked as correct with a note explaining that because the concentration had two significant figures, the pH has two digits after the decimal point.

---

**Part C: Calculating pOH**

Given the solution in Part B, calculate the pOH. Express the pOH numerically to two decimal places. Input the calculated pOH in the provided field.

--- 

This educational page outlines the fundamental relationships between pH, pOH, and the concentration of ions in a solution, using the example of sodium hydroxide to illustrate calculation methods.
Transcribed Image Text:### pH of a Strong Acid and a Strong Base **pH Definition:** pH is a logarithmic scale used to indicate the hydrogen ion concentration, \([H^+]\), of a solution: \[ \text{pH} = -\log[H^+] \] **Relationship Between pH and pOH:** Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, \([OH^-]\), are related to each other by the ion product constant of water, \(K_w\): \[ K_w = [H^+][OH^-] = 1.00 \times 10^{-14} \] Here, \(1.00 \times 10^{-14}\) is the value at approximately 297 K. Based on this relationship, pH and pOH are related as follows: \[ 14.00 = \text{pH} + \text{pOH} \] --- **Part B: Calculating pH** 0.90 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 8.0 L of solution. To find the pH of this solution, express the pH numerically to two decimal places. The calculated pH is: \[ \text{pH} = 11.45 \] The answer is marked as correct with a note explaining that because the concentration had two significant figures, the pH has two digits after the decimal point. --- **Part C: Calculating pOH** Given the solution in Part B, calculate the pOH. Express the pOH numerically to two decimal places. Input the calculated pOH in the provided field. --- This educational page outlines the fundamental relationships between pH, pOH, and the concentration of ions in a solution, using the example of sodium hydroxide to illustrate calculation methods.
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