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Question

The precipitate of $$Ca{ F }_{ 2 }\left( { K }_{ sp }=1.7\times { 10 }^{ -10 } \right) $$ is obtained when equal volumes of which of the following are mixed?


A
104 M Ca2++104 M F
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B
102 M Ca2++103 M F
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C
105 M Ca2++103 M F
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D
103 M Ca2++105 M F
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Solution

The correct option is C $${ 10 }^{ -2 }\ M\ { Ca }^{ 2+ }+{ 10 }^{ -3 }\ M\ { F }^{ - }$$
The ionic product $$\displaystyle IP = [Ca^{2+}][F^-]^2$$

 $$\displaystyle IP= { 10 }^{ -2 } \times ({ 10 }^{ -3 })^2$$

 $$\displaystyle IP={ 10 }^{ -8 }$$ 

 The ionic product exceeds solubility product.
 $$\displaystyle  { K }_{ sp }=\left( 1.7\times { 10 }^{ -10 } \right)$$

A precipitate will be formed when $$\displaystyle IP > SP$$

Chemistry

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