if you mix 50ml of 0.1 tris acid with 60ml if 0.2m tris base, what will be the resulting pH?
Use the Henderson-Hasselbalch equation.
To determine the resulting pH of the mixture, we need to calculate the concentration of the resulting solution and then use this information to determine the pH.
First, let's calculate the number of moles of Tris acid and Tris base in their respective solutions:
Moles of Tris acid = Volume (in liters) × Concentration
= 0.05 L × 0.1 mol/L
= 0.005 mol
Moles of Tris base = Volume (in liters) × Concentration
= 0.06 L × 0.2 mol/L
= 0.012 mol
The reaction between Tris acid and Tris base is as follows:
Tris acid (C4H11NO3) + Tris base (C4H11NO3) ⇌ C4H11NO3 + H2O
From the balanced equation, we can see that equal moles of acid and base will react to form Tris and water. In this case, we have excess Tris base, so all of the Tris acid will react and be neutralized. Therefore, the amount of acid remaining is zero.
Now, let's find the concentration of the resulting solution by summing the moles of Tris base and dividing by the total volume:
Total moles = Moles of Tris base
= 0.012 mol
Total volume = Volume of Tris acid + Volume of Tris base
= 0.05 L + 0.06 L
= 0.11 L
Concentration of resulting solution = Total moles / Total volume
= 0.012 mol / 0.11 L
= 0.109 M
The concentration of the resulting solution is 0.109 M.
To determine the pH, we need to consider the dissociation of Tris in water. Tris is a weak base, and its pKa value is around 8.06. At this pH, the concentrations of Tris base and Tris acid are equal, resulting in a pH of 8.06. As the resulting solution has a higher pH than the pKa, it will be a slightly basic solution.
So, the resulting pH of the mixture is around 8.06, slightly basic.