At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions?? 1 8 9 10

Question

Umakant biswal · Answer

@kaustabh
i am giving u the correct approach to solve the question ..
as u knws the formula to calculate the olubility constant
ksp = c ^ 2s square
c is given as 10 to the power -3
then
P (oh ) = loh ( oh ) –
apply that equation and u will get the answer /
option no c turns out to be the correct option .
so, answer is 9 .
HOPE U CAN DO IT
AL;L THE BEST ..

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At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions?? 1 8 9 10

At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions??

1

8

9

10

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At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions?? 1 8 9 10

At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions?? 1 8 9 10

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At 25*C , the solubility product of Mg(OH)2 is (1.0 X 10 to the power -13) . At which pH, will Mg+2 ions start precipitating in the form of Mh(OH)2 from a solution of 0.001M Mg+2 ions??

1

8

9

10