Enter your answer in the provided box. A 0.2523-g sample of a monoprotic acid neutralizes 21.6 mL of a 0.07941 M KOH solution. Calculate the molar mass of the acid. g/mol
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![**Buffer Solution Analysis**
The pH of a bicarbonate-carbonic acid buffer is 6.95. Calculate the ratio of the concentration of carbonic acid (\( \text{H}_2\text{CO}_3 \)) to that of the bicarbonate ion (\( \text{HCO}_3^- \)).
*(\( K_{a1} \) of carbonic acid is \( 4.2 \times 10^{-7} \).)*
\[ \frac{[\text{H}_2\text{CO}_3]}{[\text{HCO}_3^-]} = \boxed{\phantom{0}} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8e7ecd1-00b2-4f87-97f4-1e990180b5ce%2Fdf3addb4-de8b-4b23-bb83-ef47ceed937f%2Fh5im8kc_processed.jpeg&w=3840&q=75)
![**Problem Statement:**
Enter your answer in the provided box.
A 0.2523-g sample of a monoprotic acid neutralizes 21.6 mL of a 0.07941 M KOH solution. Calculate the molar mass of the acid.
[Input Box] g/mol
**Instructions:**
Calculate the molar mass of the acid based on the information provided. Use the formula for molarity and the relationship between moles and mass to solve for the molar mass.
**Key Information:**
- Sample weight of the monoprotic acid: 0.2523 g
- Volume of KOH solution used: 21.6 mL
- Molarity of KOH solution: 0.07941 M
**Steps:**
1. Convert the volume of KOH from milliliters to liters.
2. Use the molarity formula to find the moles of KOH.
3. Since the acid is monoprotic, use the stoichiometry to relate moles of KOH to moles of the acid.
4. Calculate the molar mass of the acid using the mass of the acid sample and the number of moles calculated.
Enter the final answer in the box provided.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe8e7ecd1-00b2-4f87-97f4-1e990180b5ce%2Fdf3addb4-de8b-4b23-bb83-ef47ceed937f%2F00ng64_processed.jpeg&w=3840&q=75)
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