Question

Consider the titration of a 25.0?mL sample of 0.175M CH3NH2 with 0.145M HBr. Determine each of the following.

the pH at 6.0mL of added acid

Answer #1

CH3NH2
+ HBr --------------
> CH3NH3Br

Before rxn 0.025 L *0.175
M 0.145 M *
0.006L
0

= 0.004375 mols
=0.00087 mols

Afterrxn
0.004375 mols -0.00087 mols
0
0.00087mols

= 0.003505 mols

= 0.003505 mols /( 0.025 + 0.005 ) L

C = 0.116 M

CH3NH2 is a weakbase with Kb = 4.38*10 ^ - 4 .

[OH-] = ? Kb * C

= ? 4.38*10 ^ - 4 . * 0.116 M

= 0.7127 * 10 ^ -2 M

pOH = - log ( 0.7127 * 10 ^ -2 )

= 2.14

pH = 14 - 2.14

= 11. 85 ==>11.9

Consider the titration of a 25.0 −mL sample of 0.180 M CH3NH2
with 0.155 M HBr. Determine each of the following.
a. the pH at one-half of the equivalence point
b. the pH at the equivalence point
c. the pH after adding 6.0 mL of acid beyond the equivalence
point
i already found that the initial pH is 11.95, the volume of acid
added to reach equivelance point is 29.0mL, and the pH og 6.0mL of
added acid is 11.23

Consider the titration of a 28.0?mL sample of 0.180M CH3NH2 with
0.150M HBr. Determine each of the following.
A.) the initial pH
B.) the volume of added acid required to reach the equivalence
point
C.) the pH at 6.0mL of added acid
D.) the pH at one-half of the equivalence point
E.) the pH at the equivalence point
F.) the pH after adding 6.0mL of acid beyond the equivalence
point
Some help & direction would be great very confused! Thank...

Consider the titration of a 26.0 −mL sample of 0.175 M CH3NH2
with 0.150 M HBr. Determine each of the following.
1. the pH at 4.0 mL of added
acid
2.the pH at the equivalence point
3.the pH after adding 6.0 mL of acid beyond the equivalence
point

Consider the titration of a 26.0-mL sample of 0.170 M CH3NH2
with 0.145 M HBr. (The value of Kb for CH3NH2 is 4.4×10−4.)
Initial pH- 11.94
Volume of added acid required to reach the equivalence point:
30.5 mL
Determine the pH after adding 5.0 mL of acid beyond the
equivalence point.

Consider the titration of a 26.0-mL sample of 0.180 M CH3NH2
with 0.145 M HBr. (The value of Kb for CH3NH2 is
4.4×10−4.)
Part A
Determine the initial pH.
Part B
Determine the volume of added acid required to reach the
equivalence point. answer to 3 sig figs
Part C
Determine the pH at 6.0 mL of added acid
Part D
Determine the pH at one-half of the equivalence point.
Part E
Determine the pH at the equivalence point.
Part...

Consider the titration of a 27.0 −mL sample of 0.180 M CH3NH2
with 0.145 M HBr. Determine the pH after adding 6.0 mL of acid
beyond the equivalence point.

Consider the titration of a 81.9 mL sample of 0.172 M CH3NH2 ,
methylamine, with 0.2 M HBr. The Kb of methylamine is 4.4x10−4.
Determine the volume (mL) of added acid required to reach the
equivalence point

Consider the titration of a 27.0 −mL sample of 0.175 MCH3NH2
with 0.150 M HBr. Express answers using two decimal places.
Determine each of the following.
A) the initial pH
B) the volume of added acid
required to reach the equivalence point
C) the pH at 6.0 mL of
added acid
D) the pH at one-half of the equivalence point
E) the pH at the equivalence point
F) the pH after adding 4.0 mL of acid beyond the equivalence
point

Consider the titration of a 25.0 −mL sample of 0.110 M HC7H5O2
with 0.120 M KOH. Determine each of the following.
The Ka of HC7H5O2 is 6.5 × 10−5.
Part A: the pH at 5.00 mL of added base pH= ?

consider a
strong acid - strong base titration OF 35.00 mL sample of 0.175 m
HBr with 0.200 m KOH
what is the ph of a solution
after 10.00 ml of the KOH has been added? Stichiometry only, no
equilibrium

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