what concentration of N2H4(aq) must be added to obtain the equivalent pH as a 0.0010M Ca(OH)2 solution at room temperatutre? (25 degrees celcius)
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what concentration of N2H4(aq) must be added to obtain the equivalent pH as a 0.0010M Ca(OH)2 solution at room temperatutre? (25 degrees celcius)
Given:
[Ca(OH)2] = 0.0010 M (or mol/L)
Ca(OH)2 is a strong base, dissociates completely into hydroxide ion.
The dissociation equation is,
Ca(OH)2 (aq) → Ca2+ (aq) + 2 OH- (aq)
As the mole ratio of Ca(OH)2 : 2 OH- is 1 : 2, [OH-] is twice the concentration of Ca(OH)2.
[OH-] = 2 × 0.0010 M (or mol/L)
[OH-] = 0.0020 M (or mol/L)
pOH = - log [OH-]
pH = 14 - pOH
To get the equivalent pH, the pOH of N2H4(aq) solution must be same as that of Ca(OH)2(aq). Consequently the [OH-] obtained by dissociation of N2H4(aq) must equal to [OH-] obtained by dissociation of Ca(OH)2(aq).
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