A 25.0-ml sample of 1.00M KBr and a 75.0-ml are mixed. The solution is then heated to evaporate water until the total volume is 50.0 ml. What is the Molarity of the KBr in the final solution
so you diluted it by half? then it is .5M? I assume the 75ml added was water.
0.3
To find the molarity of KBr in the final solution, we need to calculate the moles of KBr in the initial solution and the total volume after water evaporation.
Here's how you can calculate it step by step:
1. Calculate the moles of KBr in the initial solution:
Molarity (M) = Moles (mol) / Volume (L)
Given:
Volume of KBr solution = 25.0 ml = 0.025 L
Molarity of KBr solution = 1.00 M
Moles of KBr = Molarity * Volume
Moles of KBr = 1.00 M * 0.025 L
2. Calculate the total volume after water evaporation:
Initially, the total volume of the solution is 25.0 ml + 75.0 ml = 100.0 ml
However, after water evaporation, the total volume becomes 50.0 ml.
3. Convert the total volume to liters:
Total volume = 50.0 ml = 0.050 L
4. Calculate the final molarity of KBr in the solution:
Molarity (M) = Moles (mol) / Volume (L)
Moles of KBr remains the same as in the initial solution.
Final molarity of KBr = Moles of KBr / Total Volume
Final molarity of KBr = (1.00 M * 0.025 L) / 0.050 L
Now, solve the above equation to find the final molarity of KBr in the solution.