with these titrations can you help with the questions below? And for like number 2: is it something like this? 0.2568 M x 0.1 ml/(14.25 + 14.25) ml and if it is i dont understand why its (14.25 + 14.25) ml twice? can you possibly explain?
It could be the volume salt of the diprotic acid (inital) = 14.25 mL (which is not given in the question)
Intial volume of diprotic acid salt = 14.25 mL
and after the second equivalence point, you reach to a volume = 14.25 mL + 14.25 mL
To calculate the molarity of H+ in the solution after addition of 0.2568 M , 0.1 ml HCl; ; use M1V1 = M2V2
M2 = 0.2568 M x 0.1 ml/ 14.25 mL + 14.25 mL
M2 = 0.0009 M
pH = -log[H+] = -log(0.0009) = 3.05
with these titrations can you help with the questions below? And for like number 2: is...
Please help with the prelab questions! thank you!!!! Especially 2 and 3! Pre-Lab Questions 1. Calculate the theoretical equivalence point (the volume!) in terms of ml NaOH adde each of the titrations. Assume the concentration of acid is 0.81 M and the concentration of base is 0.51 M. 2. Which equation can be used to find the pH of a buffer? Calculate the pH of a buffer containing 0.20 M CH3COOH and 0.20 M CH3COONa. What is the pH after...
PLEASE HELP WITH THE WHITE BOX QUESTIONS & THE HIGHLIGHTED YELLOW AREA. BOLD THE ANSWERS PLEASE E H M N o R D dph/dvol Activity: 2.88 g of an unknown diprotic acid H2A were weighted and dissolved in delonised water to a final volume of 250 ml. 25 ml of this H2A solution was titrated with a standardized solution of NaOH 0.100 M. The table shows the titration data of pH as a function of NaOH added. Show your calculation...
I am looking for help with just trial one. I am not sure what equations to use or how to go about even answering these questions. I figure if I can get help with trial 1 I should be able to do trial 2 on my own. ( This week has been really bad, I lost my grandfather, so if you could "dumb" down the steps as much as possible I would appreciate it, my brain is just not working...