Ionic EquilibriumHard
Question
Which of the following solution will have pH close to 1.0 ?
Options
A.00 ml of M/10 HCl + 100 ml of M/10 NaOH
B.55 ml of M/10 HCl + 45 ml of M/10 NaOH
C.10 ml of M/10 HCl + 90 ml of M/10 NaOH
D.75 ml of M/5 HCl + 25 ml of M/5 NaOH.
Solution
(a) HCI NaOH
No. of mili eq. =
× 100 = 10 
× 100 = 10
So solution is Neutral
(b)
× 55 = 5.5 
× 45 = 4.5
[H+] =
= 10-2 M, pH = 2
(c)
× 10 = 1 
× 90 = 9 Basic
(d)
× 75 = 15 
× 25 = 5
[H+] = 0.1 M, pH = 1
No. of mili eq. =
× 100 = 10 × 100 = 10So solution is Neutral
(b)
× 55 = 5.5 × 45 = 4.5[H+] =
= 10-2 M, pH = 2 (c)
× 10 = 1 × 90 = 9 Basic(d)
× 75 = 15 × 25 = 5[H+] = 0.1 M, pH = 1
Create a free account to view solution
View Solution FreeMore Ionic Equilibrium Questions
At 298 K, a certain buffer solution contains equal concentrations of $X^{-}$and $HX,K_{b}$ for $X^{-}$is $10^{- 10}$. Wh...The dissociation constant of formic acid is 0.00024. The hydrogen ion concentration in 0.002 M-HCOOH solution is nearly...When excess oxalic acid is added to CaCl2 solution, CaC2O4 is precipitated and the solution still contains some unprecip...The solubility of CaCO3 is 7 mg/litre. Calculate the solubility product of BaCO3 from this information and from the fact...Silver nitrate solution is gradually added to an aqueous solution containing 0.01 M each of chloride, bromide and iodide...