How many moles of NH4Br are present in 88.9 mL og 0.228M solution
The correct answer and explanation is:
To find the number of moles of NH₄Br present in the given solution, we can use the formula: Moles=Molarity×Volume\text{Moles} = Molarity \times Volume
Where:
- Molarity (M) is the concentration of the solution, which is 0.228 M.
- Volume (V) is the volume of the solution, which is given as 88.9 mL. However, we need to convert this volume to liters because molarity is expressed in moles per liter. Since 1 L = 1000 mL, the volume in liters is:
88.9 mL=88.91000 L=0.0889 L88.9 \, \text{mL} = \frac{88.9}{1000} \, \text{L} = 0.0889 \, \text{L}
Now, we can substitute the values into the formula: Moles of NH₄Br=0.228 M×0.0889 L\text{Moles of NH₄Br} = 0.228 \, \text{M} \times 0.0889 \, \text{L} Moles of NH₄Br=0.0203 moles\text{Moles of NH₄Br} = 0.0203 \, \text{moles}
So, the number of moles of NH₄Br in the 88.9 mL of 0.228 M solution is approximately 0.0203 moles.
Explanation:
The molarity of a solution represents the number of moles of solute (in this case, NH₄Br) per liter of solution. By multiplying the molarity by the volume of the solution in liters, you can calculate the total number of moles of solute in the solution. Since the volume is initially given in milliliters, it must first be converted into liters to align with the molarity units. After this, multiplying the molarity by the volume gives the number of moles, which tells you how much NH₄Br is present in the solution.