4. Calculate the normality of Mg(OH)2 solution that contains 119.35 mg
Mg(OH)2 per 0.10 L of solution.
Answers
Answered by
1
Answer:
normality = mass/equavelent mass x 1000/volume(ml)
0.11935/29.2 x 1000/100 ml
normality = 0.0408
Explanation:
Answered by
0
The pH of Mg(OH)
2
solution is 10.45 at 25
∘
C . The solubility product of magnesium hydroxide will be:
A
2.24×10
−11
M
3
B
1.12×10
−11
M
3
C
3.36×10
−11
M
3
D
5.60×10
−12
M
3
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ANSWER
The pH of the magnesium hydroxide solution is 10.45
Hence pOH=14−10.45
=3.55
[OH
−
]=antilog(−3.55)
=0.000282 M.
[Mg
2+
]=
2
0.000282
=0.000141 M.
The expression for the solubility product is K
sp
=[Mg
2+
][OH
−
]
2
=0.000141×(0.000282)
2
=1.12×10
−11
M
3
.
Option B is correct.
Answer By
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Toppr
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2
solution is 10.45 at 25
∘
C . The solubility product of magnesium hydroxide will be:
A
2.24×10
−11
M
3
B
1.12×10
−11
M
3
C
3.36×10
−11
M
3
D
5.60×10
−12
M
3
HARD
Share
Study later
ANSWER
The pH of the magnesium hydroxide solution is 10.45
Hence pOH=14−10.45
=3.55
[OH
−
]=antilog(−3.55)
=0.000282 M.
[Mg
2+
]=
2
0.000282
=0.000141 M.
The expression for the solubility product is K
sp
=[Mg
2+
][OH
−
]
2
=0.000141×(0.000282)
2
=1.12×10
−11
M
3
.
Option B is correct.
Answer By
avatar
Toppr
SHARE
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Related Questions to study
Solubility products of the salts of types MX, MX
2
M
3
X at temperature T are 4×10
−8
, 3.2×10
−14
and 27×10
−16
respectively. Solubility (moldm
−3
) of the salts at T are in the order:
Study later
View Answer
The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively :
Study later
View Answer
VIEW MORE
Revise with Concepts
Calculating solubility product
EXAMPLE
DEFINITIONS
FORMULAES
20,000+
Learning videos
8,000+
Fun stories
10,000+
Fundamental concepts
8,00,000+
Homework Questions
SIGNUP FOR FREE
Learn with Videos
Derivation and Problems on Solubility Products
Derivation and Problems on Solubility Products
15 min
BROWSE BY
ClassesBoardsExams
MODULES
Online ClassesMock TestsAdaptive PracticeLive Doubts
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About Us
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