A)what is the balanced reaction between barium hydroxide and hydorochloric acid?

Question

A)what is the balanced reaction between barium hydroxide and hydorochloric acid?

B) Calculate the molarity of a barium hydroxide solution if a 55.00 mL portion of this solution is nutralized by 55.00mL of 0.5000 M HCL?

C) In Standardizing a potassium hyroxide solution, a student finds that 24.55mL of the base solution is needed to titrate 0.5002 gram of KHP to a phenolphthalein end point. In another titration, 29.40 mL of this same base solution is needed to titrate 0.2777 grams of an unknown solid monoprotic acid.Determine the molarity of the base solution and determine the molar mass of the unknown solid monoprotic acid.

'

Explanation / Answer

A)

Ba(OH)2 + 2Hcl ----> BaCl2 + 2H20

B)

from the reaction

moles of HCl = 2 x moles of Ba(OH)2

we konw that

moles = molarity x volume

so

molarity x volume of HCl = 2 x molarity x volume of Ba(OH)2

0.5 x 55 = 2 x M x 55

M = 0.25

so

molarity of Ba(OH)2 is 0.25 M

C)

moles = mass / molar mass

moles of KHp = 0.5002 / 204.22

moles of KHP = 2.45 x 10-3

the reaction is

KHP + KOH ---> K2P + H20

so

moles of KOH = moles of KHP

moles of KOH = 2.45 x 10-3

we know that

moles = molarity x volume ( L)

2.45 x 10-3 = molarity x 24.55 x 10-3

molarity of KOH = 0.0998 M

now

KOH + HA ---> KA + H20

moles of HA = moles of KOH

given 29.40 ml of KOH

so

moles = molarity x volume (L)

moles of KOH = 0.0998 x 29.40 x 10-3

moles of KOH = 2.934 x 10-3

so

moles of HA = 2.934 x 10-3

mass of HA / molar mass = 2.934 x 10-3

0.2777 / molar mass = 2.934 x 10-3

molar mass = 94.65

so the molar mass of unknow acid is 94.65 g

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.