Author Question: 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 ... (Read 71 times)

vicky · **on:** Mar 21, 2021

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?

K_sp	AgI	= 1.5 × 10^–16
K_sp	AgBr	= 5.0 × 10^–13
K_sp	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	K_sp
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 · **Reply #1 on:** Mar 21, 2021

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