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WorksheetsBuffer solutions
Total questions: 17
Worksheet time: 13mins
The buffer solution is able to maintain pH by some events, except . . .
The addition of a little acid
The addition of a little base
Dilution
Addition of water
The addition of excess acid
The following solution mixture which is/are buffer . . .
NaH2PO4 and Na2HPO4
NH3 and (NH4)2SO4
HCOOH and Ba(HCOO)2
H3PO4 and NaH2PO4
NaOH and Ba(HCOO)2
The following mixture of solutions that form a buffer solution is . . .
50 mL CH3COOH 0.2 M and 50 mL NaOH 0.1 M
50 mL CH3COOH 0.2 M and 100 mL NaOH 0.1 M
50 mL HCl 0.2 M and 100 mL NH4OH 0.1 M
50 mL HCl 0.2 M and 50 mL NH4OH 0.1 M
50 mL HCl 0.2 M and 100 mL NaOH 0.1 M
The pH solution that consist of CH3COOH 0.01 M and CH3COONa 0.01 M with Ka = 10-5 is . . .
4
5
6
8
9
Which of the following statements ARE TRUE about buffer solution?
(you may choose more than one answer)
pH of buffer solution will never change despite addition of small amount of base or acid
Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid
Buffer has acid and base components that can work specifically to resist pH change
the closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change
What statements CAN BE TRUE about acidic buffer?
(you may choose more than one answer)
It's made of a mixture of weak acid and salt of its conjugate base
Concentration of H+ ions in acidic buffer is greater than concentration of OH- ions which is present in the solution
Dilution of buffer by adding small amount of water doesn't change the pH of buffer solution
acidic buffer usually works effectively at pH range of above 7
What statement is true about basic buffer?
basic buffer usually works effectively at pH range of above 7
It's made of a mixture of strong base and salt of its conjugate acid
adding small amount of strong acid to the solution of basic buffer can significantly alter the pH of the buffer solution
diluting solution of basic buffer cause pH of that solution to change drastically
a buffer solution is made of mixture of aqueous methanoic acid, HCOOH, with aqueous sodium methanoate, NaHCOO.
the equilibrium reaction takes place in buffer solution is :
HCOOH ↔ HCOO- + H+
small amount of NaOH is then added to that buffer solution.
What reaction take places at the buffer solution to resist change of pH caused by addition of base?
HCOOH + H+ → HCOOH2
HCOO- + H+ → HCOOH
HCOOH + OH- → HCOO- + H2O
HCOO- + OH- → COO2- + H2O
a buffer solution is made of mixture of aqueous ethanoic acid, CH3COOH, with aqueous potassium ethanoate, KCH3COO.
the equilibrium reaction takes place in buffer solution is :
CH3COOH ↔ CH3COO- + H+
small amount of HCl is then added to that buffer solution.
What reaction take places at the buffer solution to resist change of pH caused by addition of acid?
CH3COO- + H+ → CH3COOH
CH3COO- + OH- → CH2COO2- + H2O
CH3COOH + H+ → CH3COOH2
CH3COOH + OH- → CH3COO- + H2O
Which of the following mixture that may produce buffer solution to work at pH of below 7?
NaOH (in excess) + HCN
KOH + NaCH3COO
KOH + HF (in excess)
HCOOH + CH3COOH
Which of the following mixture that may produce buffer solution to work at pH of above 7?
(you may choose more than one answer)
HCl + NH3 (in excess)
Mg(OH)2 + HF (in excess)
NaCN + HCN
NH3 + NH4NO3
H2SO4 (in excess) + NH3
a buffer solution is made by mixing HA, a weak acid, with salts containing A- ions.
HA ↔ H+ + A-
a formula that can be used for the calculation of the pH of this buffer solution is
Equilibrium reaction of carbon dioxide (CO2) and hydrogencarbonate (HCO3-) ions in blood is one of the important buffer system that contribute to stabilise pH of the blood
CO2(aq) + H2O(l) ↔ H+(aq) + HCO3-
Which one take place on the buffer system when blood are slightly acidic than it would be normally ?
equilibrium of the buffer system shifts to the right
more hydrogencarbonate (HCO3-) ions are consumed in reaction with excess acid to produce more dissolved CO2
more dissolved CO2 are consumed from the blood to remove excess acid and produce more hydrogencarbonate (HCO3-) ions
No shift of the equilibrium take place on the buffer system
