How many millimoles of H+ are present in 1.00 L of 1.24 M CF3CO2H solution?
My guess is that you are considering this a strong acid since there is no Ka listed.
moles = M x L
millimoles = M x mL.
To find the number of millimoles of H+ present in the solution, we need to use the concept of molarity (M). Molarity is defined as the number of moles of solute per liter of solution.
Given:
Volume of solution (V) = 1.00 L
Molarity of CF3CO2H (M) = 1.24 M
To calculate the number of millimoles of H+, we need to determine the number of moles of CF3CO2H, as it dissociates into H+ ions in solution. The molecular formula of CF3CO2H is CHF3O2.
Step 1: Calculate the number of moles of CF3CO2H:
Moles of CF3CO2H = Molarity × Volume
= 1.24 M × 1.00 L
= 1.24 moles
Step 2: Convert moles of CF3CO2H to H+ ions:
The balanced chemical equation for the dissociation of CF3CO2H is:
CF3CO2H → H+ + CF3CO2-
From the equation, we can see that 1 mole of CF3CO2H produces 1 mole of H+ ions. Therefore, the number of moles of H+ ions is also 1.24 moles.
Step 3: Convert moles of H+ ions to millimoles:
1 mole = 1000 millimoles
Therefore, the number of millimoles of H+ ions is:
Millimoles of H+ = Moles of H+ × 1000
= 1.24 moles × 1000
= 1240 millimoles
So, there are 1240 millimoles of H+ ions present in 1.00 L of 1.24 M CF3CO2H solution.