What is the pH a 0.0253 M Ca(OH)_2 solution at 25 degree C? What is the percent

Question

What is the pH a 0.0253 M Ca(OH)_2 solution at 25 degree C? What is the percent ionization of a solution of 2.5 M HNO_2 that has a pH of 1.47? Consider the titrations below. Which one is expected to have a pH >7 at the equivalent point? Titration of a weak base with a strong acid Titration of a strong acid with a strong base Titration of a strong base with a strong acid Titration of a weak acid with a strong base Which of the following is the correct solubility product (Ksp) expression for Cr(OH)_3? A solution containing equal number of moles of which of the following pairs of substances will make a buffer? The pH of a 0.20 M solution of a weak acid HA is 3.67 at 25 degree C. What is the Ka tor the acid?

Explanation / Answer

19)CaO + H2O ---> Ca(OH)2
Ca(OH)2 -------> Ca2+ + 2OH-
Calcium hydroxide solution is alkaline.
From equation, each mole of CaO gives 2 moles OH-
so concentration of OH- = 0.0506 moles per litre
we use Kw = 1 x10-14 = [H+] x [OH-]

= 10^-14/0.0506 = [H+]

= pH = 12.70

20) Dissociation = 10^-1.47 = 0.033 M

so the % ionisation = 0.033M / 2.5 *100 = 1.355 ANS

21) D

22) A

23) D

24) [H+] = squareroot(C*Ka)

= 2.28*10^-7

25)[H+] = squareroot(C*Ka)

= 2.21*10^-6

pH = 5.65

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