Ionic EquilibriumHard
Question
Which of the following mixtures will act as buffer ?
Options
A.H2CO3 + NaOH (1.5 : 1 molar ratio)
B.H2CO3 + NaOH (1.5 : 2 molar ratio)
C.NH4OH + HCl (5 : 4 molar ratio)
D.NH4OH + HCl (4 : 5 molar ratio)
Solution
(A) H2CO3 + OH- → HCO3- + H2O
moles 1.5 1
0.5 - 1
so it is a buffer solution.
(B) H2CO3 + OH- → HCO3- + H2O
moles1.5 2
- 0.5 1.5
HCO3- + OH- → CO32- + H2O
moles 1.5 0.5
- - 0.5
so it is a buffer solution.
(C) NH4OH + H+ → NH4+ + H2O
moles 5 4
1 - 4
so it is a buffer solution.
moles 1.5 1
0.5 - 1
so it is a buffer solution.
(B) H2CO3 + OH- → HCO3- + H2O
moles1.5 2
- 0.5 1.5
HCO3- + OH- → CO32- + H2O
moles 1.5 0.5
- - 0.5
so it is a buffer solution.
(C) NH4OH + H+ → NH4+ + H2O
moles 5 4
1 - 4
so it is a buffer solution.
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
Approximate pH of 0.1 M aqueous H2S solution when K1 and K2 for H2S at 25oC are 1 × 10-7 and 1.3 × 10-13 respe...The solubility of Pb(OH)2 in water is 6.0 × 10–6 M. The solubility of Pb(OH)2 in a buffer solution of pH = 8 is...When 10 mL of 0.1 M acetic acid (pKa = 5.0), is titrated against 10mL of 0.1 M ammonia solution (pKa = 5.0), the equival...What will be the percentage error in measuring hydrogen ion concentration in a 10−6 M-HCl solution on neglecting the con...Which of the following statement(s) is/are incorrect?...