3. Calculate the solubility of PbBr. in 0.10 M NaBr. The K of PbBr, is 4.6 X 10% at 25 °C. (Answer: 4.6 x 10-M) KSP = [Pb²+] [-]²s (0.010)² 4.6×104 S = = 0.10² 4.6x10-4M 4. Compare this result to the problem in the previous practice (the solubility of PbBr in water). Is this result to be expected when compared to the solubility of PbBr, in water? Why?
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![3. Calculate the solubility of PbBr. in 0.10 M NaBr. The K of PbBr₂ is 4.6.X 10% at 25 °C.
(Answer: 4.6 x 10+ M) KSP = [Pb²+] [Br-]²s (0.010)2
4.6×10-4
S = =0,10²
= 14.6×10-4 M²
4. Compare this result to the problem in the previous practice (the solubility of
PbBr, in water). Is this result to be expected when compared to the solubility of
PbBr, in water? Why?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3be27534-32b3-458e-8ab1-b03426024b28%2F5a7a2b37-5077-409f-8860-c188f64e3e6b%2Fv4o7fq_processed.jpeg&w=3840&q=75)
![The Kof PbBr₂ is 4.6 x 10 at 25°C.Calculate the solubility of PbBr, at 25°C.
2.
2
Answer: 1.1 × 10³M Ksp = [Pb²+] [Br] ³² = 45³ > 4(4.6x10-6)3
кор
x
3
Ksp =1.05x10
-2](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3be27534-32b3-458e-8ab1-b03426024b28%2F5a7a2b37-5077-409f-8860-c188f64e3e6b%2Fo7nlfta_processed.jpeg&w=3840&q=75)
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