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10.0 mL of 0.065 M pyridine (C5H5N) is titrated with 0.065 M HCl.

What is the pH of the weak base C5H5N before any HCl is added?

What volume of HCl, in mL, is required to reach the equivalence point?

What is the pH when 70% of the required HCl has been added?

What is the pH at the equivalence point?   

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Related questions

Pyridine is a weak organic base and readily forms a salt with hydrochloric acid.

C5H5N (aq) HCl (aq)  C5H5NH+] (aq) Cl- (aq)

Pyridine                            Pyridinium ion

What is the pH of a 0.025 M solution of pyridinium hydrochloride [C5H5NH+]Cl-?

25.0 ml of a 0.100 m solution of nh3 is titrated with 0.15 hcl determine the ph in the titration flask for the following
A . Before any hcl is added
B. After 10ml hcl added
C. At the equivalence point
D. After 20 ml hcl added
E. Which indicator could you use

Ammonia (NH3) is a weak base with a pKb of 4.75. Its conjugate acid, ammonium (NH4+) has a pKa of 9.25. Set up a titration using 20.00 mL of HCL to titrate 20.00 mL of aqueous ammonia solution.

Concentration of HCl soln: 0.1044 mol/L 

Initial buret reading (mL): 0.00

Buret reading at equivalence pt (mL): 14.41

Calculate the following:

a.) Moles of HCl added at equivalence pt

b.) Moles of NH3 in sample

c.) NH3 concentration (mol/L)

d.) pH at equivalence point

e.) pH at half the volume required to reach equivalence

 

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