Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb²* (aq) + 2 Cl¯ (aq) Suppose you add 0.2478 g of PbCl2 (s) to 50.0 ml of water. When the solution reaches equilibrium, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of Cl (aq) is 0.0318 M. What is the value of the equilibrium constant, Ke for the dissolution of PbCl2?

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Consider the reversible dissolution of lead(II) chloride.
PbCl2 (s) – Pb²+ (aq) + 2 Cl¯ (aq)
Suppose you add 0.2478 g of PbCl2 (s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+ (aq) is 0.0159 M and the
concentration of CI¯ (aq) is 0.0318 M.
What is the value of the equilibrium constant, Ke for the dissolution of PbCl2 ?
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Transcribed Image Text:Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) – Pb²+ (aq) + 2 Cl¯ (aq) Suppose you add 0.2478 g of PbCl2 (s) to 50.0 mL of water. When the solution reaches equilibrium, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of CI¯ (aq) is 0.0318 M. What is the value of the equilibrium constant, Ke for the dissolution of PbCl2 ? Type answer: Queton of P Type here to search 11:02 A 3/1/202 PrtScn Home End PgUp PgDn F12
Calculate the molarity of HCl in a solution if it is prepared when 5.56 mL of 4.049 M HCI is mixed with 4.44 mL of water.
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Transcribed Image Text:Calculate the molarity of HCl in a solution if it is prepared when 5.56 mL of 4.049 M HCI is mixed with 4.44 mL of water. Type answer: Question & ofa BACK e Type here to search
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