Question
In: Chemistry
What is the pH change of a buffer that has 0.100 mol HC2H3O2 and 0.130 mol...
What is the pH change of a buffer that has 0.100 mol HC2H3O2 and
0.130 mol NaC2H3O2 in 1.00 L after 0.010 mol HCl added to it? pKa =
4.74
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Calculate the pH of 0.100 L of the buffer 0.110 M CH3COONa/0.130 M CH3COOH before and...
Calculate the pH of 0.100 L of the buffer 0.110 M CH3COONa/0.130
M CH3COOH before and after the addition of the following species.
(Assume there is no change in volume.)
(a) pH of the starting buffer:
(b) pH after addition of 0.0030 mol HCl:
(c) pH after addition of 0.0040 mol NaOH (added to a fresh
solution of the starting buffer):
A 360.0 ml buffer solution is 0.130 mol/L in HF and 0.130 mol/L in NaF.
A 360.0 ml buffer solution is 0.130 mol/L in HF and 0.130 mol/L in NaF.
Part A : what mass of NaOH could this buffer neutralize before the PH rises above 4.00?
Part B: If the same volume of the buffer was 0.370mol/L in NaF, what mass of NaOH could be handled before the pH rises above 4.0?
the Ka of HF is 3.5*10^-4 this is all the information given, I can look up more ka or...
B) For 530.0 mL of a buffer solution that is 0.130 M in HC2H3O2 and 0.115...
B) For 530.0 mL of a buffer solution that is 0.130 M in
HC2H3O2 and 0.115 M in NaC2H3O2, calculate the initial pH
and the final pH after adding 0.020 mol of HCl.
C) For 530.0 mL of a buffer solution that is 0.165 M in
CH3CH2NH2 and 0.150 M in CH3CH2NH3Cl, calculate the
initial pH and the final pH after adding 0.020 mol of HCl.
Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH....
Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2
with 0.130 M NaOH. Determine each of the following. a. the volume
of added base required to reach the equivalence point b.the pH
after adding 6.00 mL of base beyond the equivalence point Express
your answer using two decimal places.
Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH....
Consider the titration of a 20.0 −mL sample of 0.100 M HC2H3O2
with 0.130 M NaOH. Determine each of the following. a. the volume
of added base required to reach the equivalence point b.the pH
after adding 6.00 mL of base beyond the equivalence point Express
your answer using two decimal places.
Consider the titration of a 22.0 −mL sample of 0.100 M HC2H3O2 with 0.130 M NaOH....
Consider the titration of a 22.0 −mL sample of 0.100 M HC2H3O2
with 0.130 M NaOH. Determine each quantity: (For acetic acid,
HC2H3O2, Ka = 1.8 × 10^-5)
A) The initial pH.
B) The volume of added base required to reach the equivalence
point.
C) The pH at 4.0 mL of added base.
D) The pH at the equivalence point.
E) The pH after adding 6.0 mL of base beyond the equivalence
point.
A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100 molNaC2H3O2. The value of Ka for HC2H3O2...
A 1.0-L buffer solution contains 0.100 molHC2H3O2 and 0.100
molNaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5 Calculate the
pH of the solution upon addition of 39.8 mL of 1.00 MHCl to the
original buffer.
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.130 M in NH4Br. Part...
A 130.0 −mL buffer solution is 0.100 M in NH3 and 0.130 M in
NH4Br.
Part A :
What mass of HCl can this buffer neutralize before the pH falls
below 9.00?
Part B:
If the same volume of the buffer were 0.255 M in
NH3 and 0.400 M in NH4Br, what mass of HCl could be
handled before the pH falls below 9.00?
A) Calculate the pH of a buffer that is 0.225M HC2H3O2 and 0.162M KC2H3O. The Ka...
A) Calculate the pH of a buffer that is 0.225M
HC2H3O2 and 0.162M
KC2H3O. The Ka for
HC2H3O2 is 1.8x10-5
B) A 1.00L buffer solution is 0.250M in HF and
0.250M in NaF. Calculate the pH of the solution after the addition
of 0.100 moles of solid NaOh. Assume no volume chane uon the
addition of base. Ka for HF= 3.5x10-4
C) A 100.0ml sample of 0.20M HF is
titrated with 0.10M KOH. Determine the pH of the solution after...
Determine the pH change when 0.093 mol HCl is added to 1.00 L of a buffer...
Determine the pH change when
0.093 mol HCl is added to
1.00 L of a buffer solution that is
0.497 M in HNO2 and
0.311 M in
NO2-.
pH after addition − pH before addition = pH change
= ___________________
Determine the pH change when
0.115 mol KOH is added to
1.00 L of a buffer solution that is
0.457 M in HNO2 and
0.256 M in
NO2-.
pH after addition − pH before addition = pH change
=_____________
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