You are given a sample containing , both with concentrations of 0.020 M. Some of the figures shown on the next page represent a series of snapshots of what molecular-level views of the sample would show as a 0 .200 M Pb ( NO 3 ) 2 ( a q ) solution is slowly added. In these figures, Br - is red-brown, and Cl - is green. Also, spectator ions are not shown, nor are ions whose concentrations are much less than the other ions. The constants for PbCl 2 and PbBr 2 are 1.7 × 10 –5 and 6.6 × 10 –6 , respectively. (1) Arrange the figures in a time sequence to show what happens as the lead(II) nitrate solution is added, excluding any that do not “make sense.” (2) Explain why you excluded any figures that did not belong in the observed time sequence.
You are given a sample containing , both with concentrations of 0.020 M. Some of the figures shown on the next page represent a series of snapshots of what molecular-level views of the sample would show as a 0 .200 M Pb ( NO 3 ) 2 ( a q ) solution is slowly added. In these figures, Br - is red-brown, and Cl - is green. Also, spectator ions are not shown, nor are ions whose concentrations are much less than the other ions. The constants for PbCl 2 and PbBr 2 are 1.7 × 10 –5 and 6.6 × 10 –6 , respectively. (1) Arrange the figures in a time sequence to show what happens as the lead(II) nitrate solution is added, excluding any that do not “make sense.” (2) Explain why you excluded any figures that did not belong in the observed time sequence.
You are given a sample containing
, both with concentrations of 0.020 M. Some of the figures shown on the next page represent a series of snapshots of what molecular-level views of the sample would show as a
0
.200
M
Pb
(
NO
3
)
2
(
a
q
)
solution is slowly added. In these figures,
Br
-
is red-brown, and
Cl
-
is green. Also, spectator ions are not shown, nor are ions whose concentrations are much less than the other ions. The constants for
PbCl
2
and
PbBr
2
are 1.7 × 10–5 and 6.6 × 10–6, respectively. (1) Arrange the figures in a time sequence to show what happens as the lead(II) nitrate solution is added, excluding any that do not “make sense.” (2) Explain why you excluded any figures that did not belong in the observed time sequence.
Consider an analyte solution of 50.0mL of 0.050M hydrochloric acid, HCl, titrated against
0.10 M sodium hydroxide, NaOH (the titration you will be performing in the lab!).
(a) What is the chemical equation representing the titration reaction?
(b) At the start of the titration, before any NaOH is added, what ions or molecules are present in the solution? You only need to list chemical species that are present in appreciable quantities - anything that is considered a small enough concentration to where you’d make a small-change approximation on an ICE table doesn’t need to be included.
(c) Which of species you identified in part (b) will determine the pH of the solution?
(d) After adding 12.50mL of the NaOH, halfway to the equivalence point, what ions or molecules are present in the solution?
(e) At the equivalence point, after adding 25.00mL of NaOH, what ions or molecules are present in the solution?
(f) Which of the species you identified in part (e) will determine…
Solid potassium hydroxide is slowly added to 50.0 mL of a 0.329 M manganese(II) bromide solution until the concentration of hydroxide ion is 0.0117 M.
What's the percent of manganese(II) ion remaining in solution?
Ag+(aq) + Cl-(aq) —> AgCl(s)
What volume un milliliter a of 8.75 x 10^-2M sodium chloride solution (Nacl) would be required to completely precipitate the Ag+ ion from one liter of waste water that is 9.00 x 10^-4M in Ag+ ion?
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