Consider these slightly soluble salts: 1. PbS Ksp = 8.4 x 10-28 2. PbSO4 Ksp = 1.8 x 10-8 3. Pb(IO3)2 Ksp = 2.6 x 10-13 i. Which is the most soluble? ii. Calculate the concentration (M), in moles/L, for Pb*2 in Pb(IO3)2. What can you do to decrease the concentration of Pb in a saturated solution of PbSO4?
Consider these slightly soluble salts: 1. PbS Ksp = 8.4 x 10-28 2. PbSO4 Ksp = 1.8 x 10-8 3. Pb(IO3)2 Ksp = 2.6 x 10-13 i. Which is the most soluble? ii. Calculate the concentration (M), in moles/L, for Pb*2 in Pb(IO3)2. What can you do to decrease the concentration of Pb in a saturated solution of PbSO4?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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![Consider these slightly soluble salts:
1. PbS
Ksp = 8.4 x 10-28
2. PBSO4
Ksp = 1.8 x 10-8
3. Pb(IO3)2
Ksp = 2.6 x 10-13
i.
Which is the most soluble?
ii.
Calculate the concentration (M), in moles/L, for Pb* in Pb(IO3)2.
+2
What can you do to decrease the concentration of Pb*² in a saturated solution of PbSO4?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F008c4733-be09-42d0-a876-85b5c0e09ce2%2F25dfffef-1831-4136-8d5f-d95a8e96dff8%2Fmn2jiqf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider these slightly soluble salts:
1. PbS
Ksp = 8.4 x 10-28
2. PBSO4
Ksp = 1.8 x 10-8
3. Pb(IO3)2
Ksp = 2.6 x 10-13
i.
Which is the most soluble?
ii.
Calculate the concentration (M), in moles/L, for Pb* in Pb(IO3)2.
+2
What can you do to decrease the concentration of Pb*² in a saturated solution of PbSO4?
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