A saturated solution of silver carbonate contains 0.0159 g Ag2CO3 in 500.0 mL of solution. What is the concentration of the Ag2CO3 solution? The molar mass of Ag2CO3 is 275.75 g/mol. [Ag2CO3] = [?] × 10 M Coefficient (green) Exponent (yellow) Enter
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![**Problem: Calculation of the Concentration of Silver Carbonate (Ag₂CO₃) in a Saturated Solution**
*A saturated solution of silver carbonate contains 0.0159 g Ag₂CO₃ in 500.0 mL of solution. What is the concentration of the Ag₂CO₃ solution?*
The molar mass of Ag₂CO₃ is 275.75 g/mol.
\[ \text{Concentration of Ag}_2\text{CO}_3 \text{ in mol/L} = \left[\text{Ag}_2\text{CO}_3\right] = [\text{?}] \times 10^{?} \, \text{M} \]
**Interactive Section:**
- **Coefficient (green)**
- [Input box]
- **Exponent (yellow)**
- [Input box]
[Enter Button]
This exercise involves determining the molarity of a silver carbonate solution, given its mass and volume, and the molar mass of the compound. Input the appropriate values in the coefficient and exponent boxes to calculate the concentration in molarity (M).
To perform the calculations, follow these steps:
1. **Convert the mass of Ag₂CO₃ to moles:**
\[ \text{Moles of Ag}_2\text{CO}_3 = \frac{0.0159 \, \text{g}}{275.75 \, \text{g/mol}} \]
2. **Convert milliliters of solution to liters:**
\[ 500.0 \, \text{mL} = 0.500 \, \text{L} \]
3. **Calculate the molarity (M):**
\[ \text{Molarity (M)} = \frac{\text{Moles of Ag}_2\text{CO}_3}{\text{Volume of solution in L}} \]
Fill in the resulting values for the coefficient and exponent to find the molar concentration of the Ag₂CO₃ solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F514063a5-d76c-41ba-8f9b-be49f83b3fde%2F1570264d-453e-42af-93d4-59f1a6369cf6%2Fxteaxa_processed.jpeg&w=3840&q=75)
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