The Ksp values of silver chromate Ag2Cro4 and silver iodate Ag(IO3) are given below.Ag2Cro4Ag(IO3)1.12 x 10123.17 x 10°8KspBased on these Ksp values, which of the following is true?In the solution consisting of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42", Ag2Cro4 precipitate will form.In the solution consisting of 1.0 x10-4 MAg* and 1.0 x10-4 M I03", Ag(IO3) precipitate will form.In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3).In the solution consisting of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate first if we add Ag*ions gradually into the above mixture.

As we know, Ksp is less than Qsp , precipitate will form. But in case of Ag2CrO4 and Ag(IO3) both have, Ksp > Qsp So, no precipitation takes place. As we know, due to common ion solubility decreases. So, Solubility in pure water is more. (d) is correct option

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of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42, Ag2CrO4 precipita= of 1.0 x10-4 M Ag* and 1.0 x10-4 M I03", Ag(103) precipitate willf y of Ag2CrO4 is lower than the solubility of Ag(1O3). of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate ove mixture.

of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42, Ag2CrO4 precipita= of 1.0 x10-4 M Ag* and 1.0 x10-4 M I03", Ag(103) precipitate willf y of Ag2CrO4 is lower than the solubility of Ag(1O3). of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate ove mixture.

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The Ksp values of silver chromate Ag2Cro4 and silver iodate Ag(IO3) are given below.
Ag2Cro4
Ag(IO3)
1.12 x 1012
3.17 x 10°8
Ksp
Based on these Ksp values, which of the following is true?
In the solution consisting of 1.00 x10-4 M Ag* and 5.00 x10-5 M Cro42", Ag2Cro4 precipitate will form.
In the solution consisting of 1.0 x10-4 MAg* and 1.0 x10-4 M I03", Ag(IO3) precipitate will form.
In pure water, the solubility of Ag2CrO4 is lower than the solubility of Ag(IO3).
In the solution consisting of 0.200 M CrO42- and 0.200 M 103', Ag2(CrO4) will precipitate first if we add Ag*
ions gradually into the above mixture.

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