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Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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A solution is prepared by mixing 100.0 ml of 0.2 M NaSCN with 100.0 ml of 0.2 M Pb(NO3)2. If the Ksp of Pb(SCN)2 is 4.42x10-23 will a precipitate occur? If so, how much will precipitate? And what is the equilibrium concentration of Pb2+?
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- Consider a mixture of 75.0 mL of 1.00 × 10−6 M thallium nitrate (TlNO3(aq)) and 100.0 mL of seawater (0.51 M in NaCl(aq)) (a) What sparingly soluble compound may form? Write out the chemical equation for its solubility equilibrium, its Ksp expression and the value of its Ksp. (b) Will a precipitate form from this mixture? Justify your answer.arrow_forwardSolid NaBr is slowly added to a solution that is 0.012 M in Cu+ and 0.012 M in Ag+ Which compound will begin to precipitate first? AgBr NaBr What percent of Ag remains in solution at the point when CuBr just begins to precipitate?arrow_forwardFor PbCl2, Ksp = 0.0000137 What is the molar solubility of PbCl2.arrow_forward
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