Problems B
387
(c) 1.00 ml of 1.00 M NaOH is added to 1 liter of 1.00 x 10~
5 M MnSO 4
(d) 1.00 ml of 1.00 M NH 3 is added to 1 liter of 1.00 x 10~
5 M MnSO 4
(e) 1.00 ml of 0.00100 M Ca(NO 3 ) 2 is added to 1 liter of 0.0100 M HF
(f) 1.00 ml of 0.0100 M Ca(NO 3 ) 2 is added to 1 liter of 0.100 vi NaHC 2 O 4
(g) 1.00 mg of Ba(NO 3 ) 2 is added to 1 liter of 0.0100 M K 2 C 2 O 4
31. Calculate the solubility (in moles/liter) of each of the following compounds in
water (neglect hydrolysis effects).
(a) BaC 2 O 4
(d) Ag 2 SO 4
(b) PbSO 4
(e) Ca(OH) 2
(c) AgBr
32. Calculate how many grams of BaSO 4 will dissolve in a liter of (a) water, (b)
0.100 M Na-jSCv (c) 0.100 M Ba(NO 3 ) 2 , (d) 0.0100 M KC1.
33. Calculate how many grams of Cd(OH) 2 will dissolve in 250 ml of (a) water, (b)
0.0100 M KOH, (c) 0.0100 M CdCl 2 .
34. What concentration of Ag
+ is needed to initiate precipitation of the negative
ions from each of the following solutions? Assume in each case that the
negative ion has not reacted with the water.
(a) 0.0500 M NaBr
(d) 2.00 M H 2 SO 4
(b) 0.100 M K 2 CO 3
(e) 0.0200 M KH(IO 3 ) 2
(c) 0.00100 M (NH 4 ) 2 CrO 4
35. What OH~ concentration is needed to commence precipitation of each of the
following metals as the hydroxide if each is present in the amount of 1.00
mg/ml?
(a) Cd
2+
(d) Mn
2+
(b) Fe
2+
(e) Ca
2+
(c) Fe
3+
36. KI is slowly added to a solution that is 0.0200 M in Pb(NO 3 ) 2 and 0.0200 M in
AgN0 3 .
(a) Which ion precipitates first?
(b) What will be its concentration when the second ion begins to precipitate?
37. What is the pH of a water solution saturated with Sn(OH) 2 ?
38. A 1.00ml sample of 0.500 M K 2 CrO 4 is added to 100 ml of a solution saturated
with PbCl 2 . How many milligrams of PbCrO 4 will precipitate?
39. What concentration of I~ is needed to start precipitation of silver from a
saturated solution of AgCl?
40. An analyst wishes to determine the amount of Pb by precipitation as the
sulfate. If her sample contains 40.0 mg Pb
2+ in 300 ml of solution, and if she
adds H 2 SO 4 to give a sulfate concentration of 0.300 M, what percentage of the
Pb
2+ will remain unprecipitated?
41. What will be the concentration of Hg
2+ remaining in solution when Tl
+ first
begins to precipitate as T1 2 S from a solution that was originally 0.100 M in
Hg
2+ and Tl
+ ?
387
(c) 1.00 ml of 1.00 M NaOH is added to 1 liter of 1.00 x 10~
5 M MnSO 4
(d) 1.00 ml of 1.00 M NH 3 is added to 1 liter of 1.00 x 10~
5 M MnSO 4
(e) 1.00 ml of 0.00100 M Ca(NO 3 ) 2 is added to 1 liter of 0.0100 M HF
(f) 1.00 ml of 0.0100 M Ca(NO 3 ) 2 is added to 1 liter of 0.100 vi NaHC 2 O 4
(g) 1.00 mg of Ba(NO 3 ) 2 is added to 1 liter of 0.0100 M K 2 C 2 O 4
31. Calculate the solubility (in moles/liter) of each of the following compounds in
water (neglect hydrolysis effects).
(a) BaC 2 O 4
(d) Ag 2 SO 4
(b) PbSO 4
(e) Ca(OH) 2
(c) AgBr
32. Calculate how many grams of BaSO 4 will dissolve in a liter of (a) water, (b)
0.100 M Na-jSCv (c) 0.100 M Ba(NO 3 ) 2 , (d) 0.0100 M KC1.
33. Calculate how many grams of Cd(OH) 2 will dissolve in 250 ml of (a) water, (b)
0.0100 M KOH, (c) 0.0100 M CdCl 2 .
34. What concentration of Ag
+ is needed to initiate precipitation of the negative
ions from each of the following solutions? Assume in each case that the
negative ion has not reacted with the water.
(a) 0.0500 M NaBr
(d) 2.00 M H 2 SO 4
(b) 0.100 M K 2 CO 3
(e) 0.0200 M KH(IO 3 ) 2
(c) 0.00100 M (NH 4 ) 2 CrO 4
35. What OH~ concentration is needed to commence precipitation of each of the
following metals as the hydroxide if each is present in the amount of 1.00
mg/ml?
(a) Cd
2+
(d) Mn
2+
(b) Fe
2+
(e) Ca
2+
(c) Fe
3+
36. KI is slowly added to a solution that is 0.0200 M in Pb(NO 3 ) 2 and 0.0200 M in
AgN0 3 .
(a) Which ion precipitates first?
(b) What will be its concentration when the second ion begins to precipitate?
37. What is the pH of a water solution saturated with Sn(OH) 2 ?
38. A 1.00ml sample of 0.500 M K 2 CrO 4 is added to 100 ml of a solution saturated
with PbCl 2 . How many milligrams of PbCrO 4 will precipitate?
39. What concentration of I~ is needed to start precipitation of silver from a
saturated solution of AgCl?
40. An analyst wishes to determine the amount of Pb by precipitation as the
sulfate. If her sample contains 40.0 mg Pb
2+ in 300 ml of solution, and if she
adds H 2 SO 4 to give a sulfate concentration of 0.300 M, what percentage of the
Pb
2+ will remain unprecipitated?
41. What will be the concentration of Hg
2+ remaining in solution when Tl
+ first
begins to precipitate as T1 2 S from a solution that was originally 0.100 M in
Hg
2+ and Tl
+ ?