Calculate the ph after the volumes have been added

Reference no: EM13715857

Question- A 30.00 mL sample of 0.1500 M hydroazoic acid (HN3; Ka = 1.9 x 10-5) is titrated with 0.1000 M KOH. Calculate the pH after the following volumes have been added:

a. 0.00 mL

b. 11.25 mL

c. 22.50 mL

d. 33.75 mL

e. 45.00 mL

f. 56.25 mL

I need proficient help to solve the above problem

Reference no: EM13715857

Questions Cloud

If an aqueous solution has a hydronium ion concentration : If an aqueous solution has a hydronium ion concentration ([H3O+]) of 5.10 x 10-9 mol/L, what is the hydroxide ion concentration ([OH-]) in the solution?

Calculate delta h of solution for kht : The International Critical Tables give the heats of formation of solid and aqueous KHT as -1545 and -1497 kj/mol respectively. From the values given, calculate delta H of solution for KHT.

How many millimoles of acetate need to add to solution : You need to produce a buffer solution that has a pH of 5.03. You already have a solution that contains 10. mmol of acetic acid. How many millimoles of acetate will you need to add to this solution. The pKa of acetic acid is 4.74. Express your answe..

Provide a chemically sound explanation for a missing point : Provide a chemically sound explanation for a missing 3rd equivalence point on titration curve of phosphoric acid. Which of the inflection points is more easily observed and why

Calculate the ph after the volumes have been added : A 30.00 mL sample of 0.1500 M hydroazoic acid (HN3; Ka = 1.9 x 10-5) is titrated with 0.1000 M KOH. Calculate the pH after the following volumes have been added:

Calculate the volume of ce4+ : Calculate the volume of 0.0300 M Ce4+ required to reach the equivalence point when titrating 41.0 mL of 0.0200 M C O2 2-4 (oxalate ion).

What is the ph of a solution containing pyridine : What is the pH of a solution containing 50.0 mL of 0.100 M pyridine (C5H5N) and 25.0 mL of 0.100 M HCL. Kb = 1.4 * 10^-9

What will be the ph after addition of rboh : A buffer was made by mixing 0.1488 moles of HCO2H with 0.1800 moles of NaHCO2 and diluting to exactly 1 liter. What will be the pH after addition of 10.00 mL of 0.2412 M RbOH to 50.00 mL of the buffer

Explain what volume of the ch3co2h solution required : A laboratory manager wants to prepare 500.00 mL of a buffer with a pH of 5.280 from equimolar solutions of CH3CO2H (Ka = 1.800e-5) and LiCH3CO2. What volume of the CH3CO2H solution would be required

User Account

All Pages