1. A 0.875 g sample of an unknown acid requires 32.1mL of a 0.182M barium hydrox
ID: 815675 • Letter: 1
Question
1. A 0.875 g sample of an unknown acid requires 32.1mL of a 0.182M barium hydroxide solution for neutralization. Assuming the acid is diprotic, calculate the molar mass of the acid
2. A 44.0mL sample of 0.186M HNO2 is titrated with 0.266M KOH . (Ka for HNO2 is 4.5710?4 .) Determine the pH at the equivalence point for the titration of HNO2 and KOH .
3. Consider these three titrations:
(i) the titration of 25.0 mL of a 0.100 M monoprotic weak acid with 0.100 M NaOH
(ii) the titration of 25.0 mL of a 0.100 M diprotic weak acid with 0.100 M NaOH
(iii) the titration of 25.0 mL of a 0.100 M strong acid with 0.100 M NaOH
Which statement is most likely to be true?
C) All three titrations have the same pH at their first equivalence point.
4. Calculate the molar solubility of CaF2 in a solution containing 0.210M Ca(NO3)2 . (Ksp=1.4610?10 )
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A) All three titrations have the same initial pH. B) All three titrations require the same volume of NaOH to reach their first equivalence point.C) All three titrations have the same pH at their first equivalence point.
4. Calculate the molar solubility of CaF2 in a solution containing 0.210M Ca(NO3)2 . (Ksp=1.4610?10 )
Please answer all 4 questions if you can! Will rate highly! Thank You!
Explanation / Answer
1). Step.1 : Calculate moles of barium hydroxide.
Molarity of Ba(OH)2 solution = 0.182 M
Volume of Ba(OH)2 solution = 32.1 mL = 32.1 /1000
= 0.0321 L
Moles of Ba(OH)2 = 0.182*0.0321
= 0.005842 moles
Step 2. Calculate moles of acid.
As given in the problem, the acid is diprotic.
So, 1 mole of acid will require 1 mole of Ba(OH)2 for its complete nutralization.
So, moles of acid = moles of Ba(OH)2
= 0.005842 moles
Step 3. Calculate molar mass of acid.
Given mass of acid = 0.875 grams
Molar mass of acid = given mass / moles of acid
= 0.875 / 0.005842
= 149.77 g/mol
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