### Determining the pH of a 0.30 M HCl Solution#### Question:What is the pH of 0.30 M HCl solution?#### Chemical Equation:\[ \text{HCl}_{(aq)} + \text{H}_2\text{O}_{(l)} \rightarrow \text{H}_3\text{O}^+_{(aq)} + \text{Cl}^-_{(aq)} \]#### Formula:\[ \text{pH} = \text{[ ? ]} \]#### Instruction:To find the pH, enter the calculated value in the provided field and press the "Enter" button.#### Visual Explanation:- Below the formula, there is a text box where you can input the calculated pH value.- Next to the text box is an "Enter" button to submit your answer.#### Calculation Guide:- Hydrochloric acid (HCl) is a strong acid and dissociates completely in water.- Therefore, the concentration of \( \text{H}_3\text{O}^+ \) ions is equal to the concentration of HCl.- For a 0.30 M HCl solution, the concentration of \( \text{H}_3\text{O}^+ \) ions is also 0.30 M.- The pH is calculated using the formula: \[ \text{pH} = -\log[\text{H}_3\text{O}^+] \]- Plug in the concentration of \( \text{H}_3\text{O}^+ \) ions into the formula to find the pH:\[ \text{pH} = -\log(0.30) \]Use a scientific calculator to find the pH value and enter it in the text box before pressing "Enter".### Interactive Learning:This exercise helps you learn how to calculate the pH of strong acid solutions, reinforcing the concept of complete dissociation in aqueous solutions.

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What is the pH of 0.30 M HCl solution? HCl(aq) + H₂O(1)→ H3O+ (aq) + Cl- (aq) pH = [?]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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