If you mix 50.0 mL of a 0.500 M solution of calcium nitrate with 150. mL of a 0.250 M solution of potassium nitrate, what would be the resulting molarity of nitrate ions in the final mixed solution ?
To determine the resulting molarity of nitrate ions in the final mixed solution, we need to understand the concept of moles and molarity and use the formula for calculating the molarity of a solution.
Molarity (M) is defined as the number of moles of solute dissolved in one liter of solution. The formula for calculating molarity is:
Molarity (M) = moles of solute / volume of solution (in liters)
To find the resulting molarity of nitrate ions in the final mixed solution, we first need to calculate the moles of nitrate ions present in each solution.
For the calcium nitrate solution:
Molarity (Ca(NO3)2) = 0.500 M
Volume (V1) = 50.0 mL = 50.0 mL / 1000 mL/L = 0.0500 L
Moles (n1) = Molarity (M1) * Volume (V1)
Moles (n1) = 0.500 M * 0.0500 L
For the potassium nitrate solution:
Molarity (KNO3) = 0.250 M
Volume (V2) = 150. mL = 150. mL / 1000 mL/L = 0.150 L
Moles (n2) = Molarity (M2) * Volume (V2)
Moles (n2) = 0.250 M * 0.150 L
Now, we can calculate the total moles of nitrate ions in the final mixed solution by adding the moles from both solutions:
Total moles of nitrate ions = moles (n1) + moles (n2)
Finally, we can calculate the resulting molarity of nitrate ions in the final mixed solution using the formula:
Molarity (M) = Total moles of nitrate ions / Total volume of solution (in liters)
Total volume of solution (Vtotal) = Volume (V1) + Volume (V2)
Now, you can plug in the values and calculate the resulting molarity of nitrate ions in the final mixed solution.