1. For each of the following species, indicate whether the resulting solution would be acidic, basic,...

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1. For each of the following species, indicate whether the resulting solution would be acidic, basic,...

1. For each of the following species, indicate whether the resulting solution would be acidic, basic, or neutral, if 1.00 mole of each were dissolved in 1.0 liter of water. Provide the predominant acid-base reaction that occurs to explain your choice.

(a) NH₄NO₃

(b) K₂CO₃

(c) NaF

(d) Al₂(SO₄)₂

(e) KClO₄

2. Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of each of the following from its solubility product:

(a) Ag₂SO₄ (K_sp= 1.2 x 10^-5)

(b) KClO₄ (K_sp= 1.05 x 10^-2)

(c) PbBr₂ (K_sp= 4.6 x 10^-6)

(d) AgI (K_sp= 1.5 x 10^-16)

(e) Cr(OH)₃ (K_sp= 3.0 x 10^-29)

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Answer 1

Answer #1

FROM KClO4 WE WILL GET KOH( STRONG BASE) AND HClO4 (STRONG ACID) SO THE SOLUTION IS NEUTRAL.

YOU DIDN'T MENTION IN WHICH UNIT SHOULD I CALCULATE MOLAR SOLUBILITY SO I DID IN TWO DIFFERENT UNIT.

YOU CAN KEEP THE ANSWER IN MOLARITY FOR SIMPLICITY.

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Answer 2

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