Welcome to Westonci.ca, where you can find answers to all your questions from a community of experienced professionals. Connect with a community of experts ready to help you find accurate solutions to your questions quickly and efficiently. Get precise and detailed answers to your questions from a knowledgeable community of experts on our Q&A platform.
Sagot :
Answer:
Let's tackle the problem step-by-step to find the molarity of the concentrated acid solution and the volume needed to prepare the 0.2000 M dilute solution.
### Step 1: Calculate the Molarity of the Concentrated Acid Solution
Given:
- Density of the concentrated sulphuric acid (\(\rho\)) = 1.804 g/cm³
- Purity = 98%
- Molar mass of \( \text{H}_2\text{SO}_4 \) = 98 g/mol
First, convert the density to g/L:
\[ \text{Density} = 1.804 \, \text{g/cm}^3 \times 1000 \, \text{cm}^3/\text{L} = 1804 \, \text{g/L} \]
Calculate the mass of \( \text{H}_2\text{SO}_4 \) in 1 L:
\[ \text{Mass of pure } \text{H}_2\text{SO}_4 = 1804 \, \text{g/L} \times 0.98 = 1767.92 \, \text{g/L} \]
Now, find the molarity (M) of the concentrated acid:
\[ \text{Molarity} = \frac{\text{Mass of } \text{H}_2\text{SO}_4}{\text{Molar mass of } \text{H}_2\text{SO}_4} = \frac{1767.92 \, \text{g/L}}{98 \, \text{g/mol}} = 18.04 \, \text{M} \]
So, the molarity of the concentrated \( \text{H}_2\text{SO}_4 \) is 18.04 M.
### Step 2: Calculate the Volume of Concentrated Acid Needed to Prepare 1 L of 0.2000 M Dilute Solution
We need to dilute the concentrated acid to get a solution of 0.2000 M. We use the dilution formula:
\[ M_1V_1 = M_2V_2 \]
where:
- \( M_1 \) = molarity of concentrated acid = 18.04 M
- \( V_1 \) = volume of concentrated acid needed
- \( M_2 \) = molarity of dilute solution = 0.2000 M
- \( V_2 \) = volume of dilute solution = 1 L = 1000 mL
Rearranging the formula to solve for \( V_1 \):
\[ V_1 = \frac{M_2V_2}{M_1} = \frac{0.2000 \, \text{M} \times 1000 \, \text{mL}}{18.04 \, \text{M}} \approx 11.09 \, \text{mL} \]
Therefore, approximately 11.09 mL of the concentrated \( \text{H}_2\text{SO}_4 \) is needed to prepare 1 L of 0.2000 M \( \text{H}_2\text{SO}_4 \).
### Step 3: Calculate the Molarity of the Acid Solution Prepared by the Student
The student measured 10.00 mL of the concentrated acid and diluted it to 1000 mL. Using the dilution formula again:
Given:
- \( M_1 \) = 18.04 M (molarity of concentrated acid)
- \( V_1 \) = 10.00 mL
- \( V_2 \) = 1000.00 mL
We need to find \( M_2 \):
\[ M_2 = \frac{M_1V_1}{V_2} = \frac{18.04 \, \text{M} \times 10.00 \, \text{mL}}{1000.00 \, \text{mL}} = 0.1804 \, \text{M} \]
So, the molarity of the acid solution prepared by the student is 0.1804 M.
Visit us again for up-to-date and reliable answers. We're always ready to assist you with your informational needs. Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Westonci.ca is your go-to source for reliable answers. Return soon for more expert insights.
