To solve the problem of finding the moles of AgNO₃ in 50.0 mL of 0.250 M (molarity) AgNO₃, we follow these steps:
### Step 1: Convert the Volume from mL to L
First, we need to convert the volume from milliliters (mL) to liters (L) because molarity (M) is defined as moles per liter (mol/L).
[tex]\[ \text{Volume in L} = \frac{\text{Volume in mL}}{1000} \][/tex]
Given:
[tex]\[ \text{Volume in mL} = 50.0 \, \text{mL} \][/tex]
So:
[tex]\[ \text{Volume in L} = \frac{50.0 \, \text{mL}}{1000} = 0.050 \, \text{L} \][/tex]
### Step 2: Use the Molarity to Find the Moles of AgNO₃
Molarity (M) is defined as the number of moles of solute per liter of solution. The number of moles of AgNO₃ can be calculated using the following formula:
[tex]\[ \text{Moles of AgNO₃} = \text{Molarity (M)} \times \text{Volume in L} \][/tex]
Given:
[tex]\[ \text{Molarity (M)} = 0.250 \, \text{M} \][/tex]
[tex]\[ \text{Volume in L} = 0.050 \, \text{L} \][/tex]
So:
[tex]\[ \text{Moles of AgNO₃} = 0.250 \, \text{M} \times 0.050 \, \text{L} \][/tex]
[tex]\[ \text{Moles of AgNO₃} = 0.0125 \][/tex]
### Conclusion:
The number of moles of AgNO₃ present in 50.0 mL of 0.250 M AgNO₃ is 0.0125 moles.
Therefore, the moles of AgNO₃ present are 0.0125 moles.
