Part A Calculate the concentration of an aqueous solution of NaOH that has a pH of 10.87. Express your answer in molarity to two significant figures. —| ΑΣΦ [NaOH] = Submit Provide Feedback Request Answer ? Review | Const M
Part A Calculate the concentration of an aqueous solution of NaOH that has a pH of 10.87. Express your answer in molarity to two significant figures. —| ΑΣΦ [NaOH] = Submit Provide Feedback Request Answer ? Review | Const M
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Acid-Base Equilibria Assignment Example:**
**Problem Overview:**
This exercise focuses on calculating the concentration of an aqueous solution of sodium hydroxide (NaOH) based on its given pH level. The target pH is 10.87.
**Task:**
Calculate the concentration of NaOH in molarity (M), ensuring that your final answer has two significant figures.
**Input Area:**
- Text box to input the concentration value of NaOH.
**Buttons:**
- Submit: To input your answer.
- Request Answer: To seek help or answers if needed.
**Instructions:**
1. Understand the relationship between pH, pOH, and hydroxide ion concentration.
2. Use the formula: \[ \text{pOH} = 14 - \text{pH} \]
3. Convert pOH to hydroxide concentration using: \[ [\text{OH}^-] = 10^{-\text{pOH}} \]
4. Input the calculated concentration of NaOH in the box provided and submit.
**Feedback:**
- A "Provide Feedback" option is available to leave any comments or suggestions.
This exercise is a practical example of applying acid-base equilibrium concepts to determine the concentration of a basic solution given its pH value.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd28bb5a8-7114-481e-95e9-134d2c6aa143%2Fdedf6e51-9d97-46a6-a803-66d70ed71637%2F6cnk4c_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Acid-Base Equilibria Assignment Example:**
**Problem Overview:**
This exercise focuses on calculating the concentration of an aqueous solution of sodium hydroxide (NaOH) based on its given pH level. The target pH is 10.87.
**Task:**
Calculate the concentration of NaOH in molarity (M), ensuring that your final answer has two significant figures.
**Input Area:**
- Text box to input the concentration value of NaOH.
**Buttons:**
- Submit: To input your answer.
- Request Answer: To seek help or answers if needed.
**Instructions:**
1. Understand the relationship between pH, pOH, and hydroxide ion concentration.
2. Use the formula: \[ \text{pOH} = 14 - \text{pH} \]
3. Convert pOH to hydroxide concentration using: \[ [\text{OH}^-] = 10^{-\text{pOH}} \]
4. Input the calculated concentration of NaOH in the box provided and submit.
**Feedback:**
- A "Provide Feedback" option is available to leave any comments or suggestions.
This exercise is a practical example of applying acid-base equilibrium concepts to determine the concentration of a basic solution given its pH value.
Transcribed Image Text:**Part D**
**Problem Statement:**
Give the conjugate acid of the following Brønsted-Lowry base: \( \text{H}_2\text{AsO}_4^- \).
**Instruction:**
Express your answer as a chemical formula.
**Answer Input Field:**
There is an input box where the answer should be typed in a chemical formula format. Below the input box, there is an option: "A chemical reaction does not occur for this question."
**Submission:**
There are buttons labeled "Submit" and "Request Answer" for submitting the answer or asking for help.
---
**Explanation for Educational Purpose:**
In Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors. The conjugate acid is formed by adding a proton (\( \text{H}^+ \)) to the base. For the given base \( \text{H}_2\text{AsO}_4^- \), its conjugate acid is \( \text{H}_3\text{AsO}_4 \).
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