calculate the PH during the titration of 50.00 ml of 0.300 M HNO3 with 0.600 M KOH after 0, 15.50, 25.00, and 40.00 ml of KOH have been added. Graph the titration curve.

Ph=

calculate the Ph in the titration of 50.00 ml of 0.100 M ammonia with 0.100 M HCl after 0,24.00,50.00, and 74.00 ml acid have been added

Ka((NH3)= 1.8x10^(-5)

PH= ............ when 0 ml added.

PH= ............ when 24.00 ml added

PH= ............ when 50.00 ml added

PH= ............ when 74.00 ml added

millimoles HNO3 = mL x M = 50.00 x 0.3M = 15 millimoles.

mmoles KOH = mL x 0.6M =
mL = 0, 0mmoles KOH
mL = 15.5, 9.3 mmoles
mL = 25.0, 15 mmoles
mL = 40.0, 24 mmoles
I'll do the 15.5 or 9.3 mmoles KOH added.
..........HNO3 + KOH ==> KNO3 + H2O
initial...15......0........0......0
added............9.3...............
change...-9.3...-9.3.......9.3.....9.3
equil....5.7......0.........9.3....9.3

You can see that you have a solution of HNO3 with KNO3 (a salt that does not change the pH of the solution upon hydrolysis). So (H^+) = (HNO3) so convert H^+ to pH.
At the equivalence point (mmoles acid = mmoles base), the pH is determined by the hydrolysis of the salt. An ICE chart will show you how to go about that.
After the equivalence point you will have an excess of the base; convert to OH^-, pOH, and pH.

For the weak base and strong acid, do the same kind of thing (ICE chart etc) but in cases where the weak base is present you must go through an ICE chart for a weak base. At all points between the beginning and the equivalence point, you have a buffered solution and you should use the Henderson[-Hasselbalch equation.

To calculate the pH during the titration process, we can use the concept of neutralization and the principles of acid-base titrations.

1. Determine the moles of HNO3 initially present:
Moles of HNO3 = concentration of HNO3 (M) x volume of HNO3 (L)
Moles of HNO3 = 0.300 M x 0.0500 L

2. Calculate the moles of HNO3 remaining after each volume of KOH is added:
Moles of HNO3 remaining = initial moles of HNO3 - moles of KOH added

3. Determine the moles of HNO3 neutralized by KOH:
Moles of HNO3 neutralized = moles of KOH added
Since the reaction between HNO3 and KOH is 1:1, the moles of HNO3 neutralized are equal to the moles of KOH added.

4. Calculate the concentration of HNO3 remaining after each volume of KOH is added:
Concentration of HNO3 remaining = moles of HNO3 remaining / volume of solution after KOH is added

5. Calculate the pH using the concentration of HNO3 remaining:
pH = -log[H+]
[H+] is the concentration of H+ ions, which can be approximated by the concentration of HNO3 remaining (since HNO3 is a strong acid).

By following these steps, we can calculate the pH at each point during the titration.

To graph the titration curve, plot the pH on the y-axis and the volume of KOH added on the x-axis. Connect the plotted points together to get the titration curve. The shape of the curve will depend on the nature of the acid and base being titrated.