A solution is 0.010 M in each of Pb(NO3)2, Mn(NO3)2, and ...

[vicky]

Question 1

A solution contains 0.018 moles each of I^–, Br^–, and Cl^–. When the solution is mixed with 200 mL of 0.24 M AgNO₃, how much AgCl(s) precipitates out?

	Ksp	AgI		= 1.5 × 10–16
	Ksp	AgBr		= 5.0 × 10–13
	Ksp	AgCl		= 1.6 × 10–10

◦ 0.0 g
◦ 1.7 g
◦ 2.6 g
◦ 3.3 g
◦ 5.0 g

Question 2

A solution is 0.010 M in each of Pb(NO₃)₂, Mn(NO₃)₂, and Zn(NO₃)₂. Solid NaOH is added until the pH of the solution is 8.50. Which of the following statements is true?

Salt	Ksp
Pb(OH)2	1.4 × 10–20
Mn(OH)2	2.0 × 10–13
Zn(OH)2	2.1 × 10–16

◦ No precipitate will form.
◦ Only Pb(OH)₂ will precipitate.
◦ Only Mn(OH)₂ will precipitate.
◦ Only Zn(OH)₂ and Pb(OH)₂ will precipitate.
◦ All three hydroxides will precipitate.

[Jayson]

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[vicky]

Great answer, keep it coming

[bigcheese9]

Thanks for the timely response, appreciate it