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| Weak Acid Strong Base Titrations | 34 mins | 0 completed | Learn |
| Weak Base Strong Acid Titrations | 17 mins | 0 completed | Learn |
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| Titrations of Diprotic and Polyprotic Acids | 27 mins | 0 completed | Learn |
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| Additional Practice |
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| Equivalence Point |
| Acid Base Indicators |
| Selective Precipitation |
| Formation Constant |
| Additional Guides |
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| Henderson Hasselbalch Equation (IGNORE) |
Associated with any ionic compound is the solubility product constant, which measures how soluble the compound will be in a solvent.
Molar Solubility
Concept #1: Understanding the Solubility Product Constant.
Transcript
Hey guys, in this new video, we’re going to take a look at a new concept – the solubility product constant. We’re used to so many Ks up to now. We've seen Ka, we’ve seen Kb. But now we're going to be dealing with Ksp which we’re going to refer to as our solubility product constant. We're going to say here that solubility was the maximum amount of solute that could successfully be dissolved in a solvent. Remember, another name for solubility is molarity. Another name for molarity is concentration. Solubility, molarity, and concentration – all three, different words but all mean the same exact thing. How much solute can I get to dissolve in my given solvent.
Now we're going to say in this section we’re going to learn about associated with any type of solid. Any solid is the Ksp value. We’re going to say the Ksp’s value stands for what we've been saying – the solubility product constant. We’re going to say the larger our Ksp value is, then the more soluble the solid is in its given solvent. We're going to say the smaller our Ksp value, then the less soluble the solid is in its given solvent.
Ksp is just the measurement of solubility, how soluble is your solid. If you’re ever giving Ksp for a compound, you should know automatically since this compound is given a Ksp value, the compound has to be a solid.
The general rule is that the greater the solubility product constant for a compound then the more soluble the compound.
Example #1: Consider the following compounds. Which has the highest concentration of OH- ions?
a) Co(OH)2 Ksp = 1.3 x 10-15
b) Cu(OH)2 Ksp = 2.2 x 10-20
c) Ni(OH)2 Ksp = 6.0 x 10-16
d) Fe(OH)2 Ksp = 4.1 x 10-15
e) Zn(OH)2 Ksp = 3.0 x 10-16
Transcript
Now we're going to say example 1. Consider the following compounds. Which has the highest concentration of OH- ions? What we should realize here is that all of them have two OH- involved. Because they all have the same number of OH-, that means that is not a deciding factor, so just ignore that. That means just look at the Ksp value. We're going to say the one that has the highest Ksp value would be the most soluble, which means it breaks up into the most ions. The one that breaks up into the most ions would have the highest concentration of OH- ions. All we got to do here is look to see which Ksp is the biggest. Here we have two that are to the negative 15. But this one is 4.1 and this one is just 1.3. So, D would be our correct answer.
Another way your professor could have worded this is remember, associated with OH- ions is basicity. The more OH- you have, the more basic you are. I could have worded this as which is the most basic. You should have read into that and said, “Okay, he means most basic so that means who has the highest amount of OH-.” I could have also said least acidic, which of the following is least acidic, which would have mean who has the lowest amount of H3O+ ions or who has the highest concentration of OH- ions, different ways. Three different ways that ask the same exact question. Remember, because all of them had two OH-, we didn't have to look at the number of ions. We only looked at the KSP. If they had different number of OH- ions, then we’d have to do calculations in order to find their molar solubility which is x. We'll learn how to do that a little bit later on.
Example #2: The solubility of silver sulfate, Ag2SO4, is 0.025 M at 25oC. Calculate its solubility product constant, Ksp.
Whenever the question refers to the solubility then that value represents our “x” variable.
Example #3: Find the solubility of CoCl3 (Ksp = 2.8 x 10-13) in:
a) pure water
Whenever we deal with the solubility product constant we use an ICE Chart and since the reactant will always be a solid then we can ignore it.
If our compound dissolves in a solution with similar ions then the Common Ion Effect takes place.
Example #4: Find the solubility of CoCl3 (Ksp = 2.8 x 10-13) in:
b) 0.20 M NaCl.
Example #5: What is the molar solubility of Fe(OH)3 (s) in a solution that is buffered at pH 3.50 at 25 oC? The Ksp of Fe(OH)3 is 6.3 x 10–38 at 25 oC.
Example #6: Find the pH of a saturated solution of Aluminum hydroxide, Al(OH)3. The Ksp of Al(OH)3 is 1.9 x 10-10.
Example #7: Will a precipitate form when 0.150 L of 0.100 M Pb(C2H3O2)2 and 0.100 L of 0.20 M KCl are mixed? The Ksp value of PbCl2 is 1.2 x 10-5.
Example #8: Two flasks containing 7.12 x 10-6 M silver nitrate, AgNO3, and 8.33 x 10-4 M strontium bromide, SrBr2 respectively, are mixed together into a larger flask. If the Ksp of silver bromide, AgBr, is 5.35 x 10-13 what will happen?
- A precipitate of Sr(NO3)2 will form.
- The solution is saturated but will remain clear.
- The solution is not saturated and no precipitate will form.
- A precipitate of silver bromide will form, with silver and bromide ions as well.
- A precipitate of silver bromide will form.
Example #9: A saturated solution of AlCl3 contains 5.15 x 10-4 M chloride ions. What is the solubility product constant, Ksp?
Example #11: The solubility of CaF2 is 53.2 g/mL at 25 oC. Calculate its solubility product constant, Ksp.
Example #12: The concentration of chloride and iodide ions present in the solution are [Cl –] = 0.073 M and [I –] = 0.060 M. The use of silver, Ag, can be used to precipitate these two ions. If the Ksp value of AgCl is 1.77 x 10-10 and AgI is 8.51 x 10-17.
a) Which ion will precipitate out first?
b) At what concentration will this ion from Part A begin to precipitate out?
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Videos in Ksp
Concept #1: Understanding the Solubility Product Constant.
Example #1: Consider the following compounds. Which has the ...
Example #2: The solubility of silver sulfate, Ag2SO4, is 0.0...
Example #3: Find the solubility of CoCl3 (Ksp = 2.8 x 10-13)...
Example #4: Find the solubility of CoCl3 (Ksp = 2.8 x 10-13)...
Example #5: What is the molar solubility of Fe(OH)3 (s) in a...
Example #6: Ksp and pH
Example #7: The Reaction Quotient & Ksp
Example #8: Q vs Ksp
Example #9: Ksp Determination
Example #10: Molar Solubility of Ions
Example #11: Ksp and solubility
Example #12: Selective Precipitation
Additional Problems
In which of the following solutions would PbBr2 be expected to be the least soluble at a given temperature.
A. 0.1M CaBr2
B. 0.1M HBr
C. 0.1M NaBr
D. 0.1M KNO3
Which of the following compounds will have the highest molar solubility in pure water?
A. NiS Ksp = 3.00x10 -20
B. PbS Ksp = 9.04x10 -29
C. MgCO3 Ksp = 6.82x10 -6
D. AgCN Ksp = 5.97x10 -17
E. PbSO4 Ksp = 1.82x10 -8
When a solution of weak electrolyte is altered by adding one of its ions from another source, the ionization of the weak electrolyte is suppressed. The behavior is termed the ___________.
Which reagent(s) INCREASES the solubility of Zn(OH) 2 when added to a saturated aqueous solution of Zn(OH)2?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NH 3
d. a and c
e. all of the above
Which reagent(s) DECREASES the solubility of Ni(OH) 2 when added to a saturated aqueous solution of Ni(OH)2?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NiCl 2
d. a and c
e. all of the above
If 147 g of ZnF2 (Ksp = 0.0300) is added to water to make a 1.00 L solution, what is the [F− ] concentration in the solution in molarity?
A. 0.173
B. 0.196
C. 0.391
D. 1.42
E. 2.84
A solution begins with 0.100 M of NaF dissolved in water. What is the concentration of Magnesium ion in the solution, if MgF2 was added in excess? Ksp (MgF2) = 5.2 X 10 −11
A. 5.2 x 10 −13
B. 5.2 x 10 −11
C. 5.2 x 10 −9
D. 0.00023
E. 0.00047
The molar solubility of Cd(OH)2 in water is 1.7 x 10 -5 mol/L at 25°C. The Ksp value for Cd(OH)2 is:
A. 2.0 x 10 -14
B. 4.9 x 10 -15
C. 5.8 x 10 -10
D. 2.9 x 10 -10
E. none of these
Which of the following salts shows the lowest solubility in water?
Ksp values are as follows:
Ag2S = 1.6 x 10 -49
Bi2S3 = 1.0 x 10 -72
HgS = 1.6 x 10 -54
Mg(OH)2 = 8.9 x 10 -12
MnS = 2.3 x 10 -13
A. Bi2S3
B. Ag2S
C. MnS
D. HgS
E. Mg(OH)2
The solubility of CaF2 (s) [Ksp= 4.0 x 10 -11] in 1.0 L of a 1.0 x 10 -2 M solution of NaF is:
A. 4.0 x 10 -9 moles
B. 1.0 x 10 -7 moles
C. 7.0 x 10 -4 moles
D. 4.0 x 10 -7 moles
E. none of these
The concentration of OH - in a saturated solution of a certain metal hydroxide, M(OH)2 , is 3.6x10 -4 M . The Ksp of M(OH)2 is:
A. 1.3 x 10 -7
B. 4.7 x 10 -11
C. 1.2 x 10 -11
D. 3.6 x 10 -4
E. none of these
What is the molar solubility of Co(OH) 2 when buffered at a pH of 13.20?
a. 1.4 x 10 -5 M
b. 8.5 x 10 -6 M
c. 1.6 x 10 -12 M
d. 1.0 x 10 -13 M
e. 1.6 x 10 -14 M
Which salt is NOT more soluble in acidic solution than it is in pure water?
a. CdCO3 Ksp = 5.2 x 10 -12
b. Cd(OH)2 Ksp = 2.5 x 10 -14
c. Cd(OH)2 Ksp = 2.5 x 10 -15
d. AgI K sp = 8.3 x1 0 -17
e. ZnCO3 Ksp = 1.4 x 10 -11
Which reagent can be used to separate silver and copper from an aqueous solution of AgNO3 and Cu(NO3)2?
a. 1.0 M H2SO4
b. 1.0 M HCl
c. 1.0 M NaCl
d. b and c
e. all of the above
Which reagent can be used to separate cobalt and copper from an aqueous solution of Co(NO3)2 and Cu(NO3)2?
a. 5% thioacetamide in HNO3 (aq), heated to ~80°C
b. 1.0 M HCl
c. 1.0 M NH3
d. a and b
e. a and c
Which reagent can be used to separate the solids Al(OH) 3 and Fe(OH)3?
a. 1.0 M NaOH
b. 1.0 M HCl
c. 1.0 M NaCl
d. a and b
e. none of the above
Solve for the concentration of Magnesium ions when 1.29 moles of Mg(OH) 2) is added to a 1.00 L solution that is initially at pH = 11.00. Ksp (Mg(OH)2) = 5.6 X 10-12
A. 5.6 X 10-9
B. 5.6 X 10-6
C. 1.1 X 10-5
D. 1.1 X 10-4
E. 1.3
Which of the following solubility product expressions is incorrect?
A. Ksp (Ag2S) = [Ag+]2[S-2]
B. Ksp ( CaF2) = [Ca2+][F-]2
C. Ksp (PbCl2) = [Pb2+][Cl-]2
D. Ksp (CuS) = [Cu2+][S2-]
E. Ksp (Ag3PO4) = [Ag+]3[P] [O3-]4
What is the ksp expression for Mg 3(PO4)2? (Look at all the answers carefully. Some of them are very similar)
(a) [Mg2+]3[PO43-]2
(b) [Mg2+]2[PO43-]3
(c) [Mg]3[PO4]2
(d) [Mg]3[PO4]2
[Mg3(PO4)2]
(e) [Mg3(PO4)2]
[Mg]3[PO4]2
Would you expect the solubility of Mg 3(PO4)2 to be greater than, less than, or the same in a 0.10 M Na3PO4 solution compared to pure water?
(a) greater than (b) less than (c) the same
Give the expression for the solubility product constant for BaF 2.
Describe the solubility of Al(OH)3 with respect to pH.
A) soluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
B) soluble at low pH, insoluble in pH-neutral solution, and insoluble at high pH
C) insoluble at low pH, insoluble in pH-neutral solution, and soluble at high pH
D) insoluble at low pH, in pH-neutral solution, and at high pH
E) pH has no effect on the solubility
In which of the following solutions would PbBr 2 be expected to be the least soluble at a given temperature?
0.1M CaBr2
0.1M HBr
0.1M NaBr
0.1M KNO3
A solution of sodium fluoride is added dropwise to a solution that is 0.0144 M in ionic barium. At what concentration of fluoride ion will barium fluoride start to precipitate? Neglect volume changes, the Ksp for barium fluoride is 1.7x10 –6.
A. 2.4 x 10 –8
B. 1.1 x 10 –2
C. 1.2 x 10 –4
D. 5.9 x 10 –5
E. 2.7 x 10 –3
Which of the following compounds will have the highest molar solubility in pure water?
NiS Ksp = 3.00x10 –20
PbS Ksp = 9.04x10 –29
MgCO3 Ksp = 6.82x10 –6
AgCN Ksp = 5.97x10 –17
PbSO4 Ksp = 1.82x10 –8
What is the molar solubility of magnesium hydroxide in a basic solution with pH of 12.50? The Ksp for magnesium hydroxide is 5.6 x 10-12.
2.40x10-6 M
1.10x10-4 M
1.80x10-10 M
5.60x10-9 M
Given the following Ksp values, which statement about solubility in water is correct?
K sp
PbCrO4 2.0 x 10 -16
Zn(OH)2 4.5 x 10 -17
Pb(OH)2 1.2 x 10 -15
MnS 2.3 x 10 -13
a) PbCrO4, Zn(OH)2, and Pb(OH)2 have equal solubility in water.
b) PbCrO4 has the lowest solubility in water.
c) The solubility of MnS in water will not be pH dependent.
d) MnS has the highest molar solubility in water.
e) A saturated PbCrO4 solution will have a higher [Pb2+] than a saturated Pb(OH)2 solution.
Which of the following salts has the highest concentration of silver ion when dissolved in water?
a) AgCl Ksp = 1.6 x 10-10
b) Ag2CO3 Ksp = 8.1 x 10-12
c) AgBr Ksp = 5.0 x 10-13
Which salt precipitates first and what is the minimum concentration of Ag + necessary to cause this precipitation in a solution containing 7.5 mL of 0.025 M NaCl and 7.5 mL of 0.025 M Na3PO4?
(Hint: dilution occurs)
Ksp(AgCl) = 1.8 x 10-10
Ksp(Na3PO4) = 1.3 x 10-20
a) AgCl 8.7 x 10 -7 M
b) Ag3PO4 2.3 x 10 -7 M
c) AgCl 1.4 x 10 -8 M
d) Ag3PO4 7.2 x 10 -8 M
e) None of these answers are correct
The solubility of CaCO3 (formula weight 100.1) is 0.0095 g in 1800 mL. What is the Ksp?
A. 2.8 x 10 -5
B. 2.8 x 10 -9
C. 5.2 x 10 -5
D. 5.2 x 10 -9
E. 3.8 x 10 -7
In which solution is Ag3PO4 least soluble?
a. In pure water
b. 0.50 M AgNO3
c. 0.50 M Na3PO4
d. AgPO4 is least soluble equally in b and c
e. AgPO4 is equally soluble in all of the above
What is the molar solubility of silver (I) carbonate in the presence of 0.20 M Na 2CO3?
a. 3.18 x 10 -6M
b. 4.50 x 10 -6M
c. 1.27 x 10 -4M
d. 1.42 x 10 -5M
e. 5.68 x 10 -5M
What is the solubility product, Ksp of Mg(OH)2 if its solubility in water is 1.6 x 10 -4 mol•L-1?
a) 1.6 x 10-11
b) 2.6 x 10-8
c) 3.2 x 10-4
d) 4.1 x 10-12
A saturated solution of MgF2 contains 1.6 x 10-3 mol of MgF2 per liter at a certain temperature. What is the Ksp, of MgF2 at this temperature?
a) 2.7 x 10-6
b) 1.6 x 10-8
c) 3.1 x 10-9
d) 6.2 x 10-9
The addition of solid Na 2SO4 to an aqueous solution in equilibrium with solid BaSO 4 will cause
a) no change in [Ba 2+] in solution.
b) more BaSO4 to dissolve.
c) precipitation of more BaSO4.
d) an increase in the Ksp of BaSO4.
How many grams of CuCl (MW = 99.0 g mol –1) can be dissolved in 5.00 L of water before a precipitate forms? Ksp(CuCl) = 1.0 x 10–6
(a) 0.10 g
(b) 0.22 g
(c) 0.49 g
(d) 0.98 g
(e) 1.10 g
Silver iodide has very low solubility as shown by the following reaction equation.
Agl (s) ↔ Ag+ (aq) + I - (aq)
Which of the following statements is/are true?
i. K < l
ii. the concentration of Ag+ will be large
iii. K > l
a. i only
b. ii only
c. iii only
d. i and ii
e. ii and iii
What is the pH of a standard solution of iron (II) hydroxide, Fe(OH) 2. Ksp = 4.87 x 10-17 for the Iron (II) hydroxide.
a. 5.64
b. 8.36
c. 5.34
d. 8.66
e. 8.76
The solubility of lead (II) iodide is 0.064 g / 100 mL at 20°C. What is the solubility product for lead (II) iodide?
A) 1.1 x 10-8
B) 3.9 x 10-6
C) 1.1 x 10-11
D) 2.7 x 10-12
E) 1.4 x 10-3
Determine the molar solubility of Al(OH)3 in a solution containing 0.050 M KOH.
Ksp (Al(OH)3) = 1.9 x 10 -33
A) 1.0 x 10-11 M
B) 5.0 x 10-7 M
C) 4.75 x 10-36 M
D) 1.5 x 10-29 M
E) 0.050 M
Give the expression for the solubility product constant for Hg 2Cl2.
A) [Hg22+][Cl-]2 / [Hg2Cl2]
B) [Hg2Cl2] / [Hg22+][Cl-]2
C) [Hg22+][Cl1-]2
D) [Hg22+]2[Cl-] / [Hg2Cl2]
E) [Hg22+]2[Cl1-]
Determine the molar solubility of CuCl in a solution containing 0.050 M KCl.
Ksp (CuCl) = 1.0 x 10-6
A) 1.0 x 10-12 M
B) 5.0 x 10-7 M
C) 2.0 x 10-5 M
D) 1.0 x 10-3 M
E) 0.050 M
Which of the following compounds will have the highest molar solubility in pure water?
A) PbSO4, Ksp = 1.82 x 10-8
B) MgCO3, Ksp = 6.82 x 10-6
C) AgI, K sp = 8.51 x 10-17
D) PbS, K sp = 9.04 x 10-29
E) FeS, K sp = 3.72 x 10-19
The solubility of silver (I) iodate is 0.0027 g/100 mL at 20 oC. What is the solubility product for silver iodate? (MWt AgIO3 = 273 g/mole)
A) 1.0 × 10–8
B) 3.9 × 10–6
C) 9.8 × 10–9
D) 2.7 × 10–12
E) 1.4 × 10–3
The Ksp equation for sodium bicarbonate (NaHCO3) should be written as:
Determine the molar solubility of some salt with the generic formula AB 2 if Ksp = 2.56x102 .
10 M
0.1 M
4 M
1 M
A hypothetical compound MX3 has a molar solubility of 0.00562 M. What is the value of Ksp for MX3?
3.16 x 10-5
2.99 x 10-9
9.48 x 10-5
2.69 x 10-8
A solution begins with 0.100 M of NaF dissolved in water. What is the concentration of Magnesium ion in the solution, if MgF2 was added in excess? Ksp (MgF2) = 5.2 X 10 −11
A. 5.2 * 10−13
B. 5.2 * 10 −11
C. 5.2 * 10 −9
D. 0.00023
E. 0.00047
Calculate the molar solubility of silver (I) carbonate ( Ksp=8.1x10–12) in water at 25 ̊C.
a. 8.1x10–12 M
b. 2.0x10–6 M
c. 1.3x10–4 M
d. 1.6x10–4 M
e. 2.6x10–4 M
Calcium hydroxide has a molar solubility of 0.0118 M in water. How much Ca(OH) 2 (in mg) is soluble in 100.0 mL of water?
a. 6.5x10–6 mg
b. 0.0118 mg
c. 0.0235 mg
d. 0.874 mg
e. 87.4 mg
What is the molar solubility of a saturated solution of PbCl 2 (Ksp=1.7x10–5)?
a. 1.5x10–5 M
b. 2.9x10–3 M
c. 4.1x10–3 M
d. 0.016 M
e. 0.020 M
6.5 mg of calcium fluoride is soluble in 250.0 mL of water at 25 ̊C. What is its Ksp?
a. 1.1x10–7
b. 1.5x10–10
c. 3.7x10–11
d. 2.3x10–12
e. 5.8x10–13
What pH should an aqueous solution of Co(OH) 2 (Ksp=1.1x10–15) be adjusted to so that the concentration of Co2+ is 1.0 x 10–9 M.
a. 8.04
b. 8.81
c. 10.72
d. 11.02
e. 11.32
What is the pH of a saturated aqueous solution of Cd(OH) 2 (Ksp=2.5x10–14)?
a. 9.57
b. 9.47
c. 9.27
d. 7.35
e. 4.73
What is the molar solubility of silver (I) carbonate ( Ksp=8.1x10–12) in the presence of 0.20 M Na2CO3?
a. 3.18 × 10−6 M
b. 4.50 × 10−6 M
c. 1.27 × 10−4 M
d. 1.42 × 10−5 M
e. 5.68 × 10−5 M
The solubility of silver sulfate (MW 311.8) is 4.73 g/L at 25°C. Calculate solubility product constant.
a) 1.4 x 10-5
b) 6.5 x 10-8
c) 2.3 x 10-4
d) 8.1 x 10-9
e) 3.4 x 10-6
The equilibrium constant for the reaction:Ag2SO4(s) ⇌ 2Ag+ (aq) + SO42- (aq)is Kc = 1.8x10 −10. If the SO42- concentration is 1.2x10−6 M, what is the Ag+ concentration?a) 0.221b) 1.50x10 −4c) 2.25x10 −8d) 1.22x10 −2e) 8.66x10 −6
Two compounds with general formulas AX and AX 2 have Ksp = 1.5 x 10 -5. Which of the two compounds has the higher molar solubility? Explain your choice.
What is the correct expression for the solubility product constant for iron (III) hydroxide?
(a) Ksp = [Fe3+(aq)] [OH− (aq)]
(b) Ksp = [Fe3+(aq)] [OH− (aq)] 3
(c) Ksp = [Fe3+(aq)] 3 [OH− (aq)]
(d) Ksp = [Fe3+(aq)] 3[OH− (aq)]
(e) Ksp = [Fe3+(aq)] 3 [OH− (aq)] 3
Which of the following compounds has the lowest solubility in water? A. AgI, Ksp = 8.5 × 10 −17B. PbBr2, Ksp = 6.6 × 10 −6C. Sr3(PO4)2, Ksp = 4 × 10 −28D. Ag(CH3COO), Ksp = 4.4 × 10 −3
Ksp = 4.64 × 10 −3 for Ba(NO3)2. What is the concentration of the nitrate ion in a saturated Ba(NO3)2 solution? A. 0.105 MB. 0.167 MC. 0.210 MD. 0.333 ME. 0.068 MF. 0.136 M
The solubility of PbBr2 is 8.44 g/L at 20°C. What is Ksp for this compound? A. 1.1 × 10 −6B. 5.3 × 10 −4C. 1.0 × 10 −3D. 4.9 × 10 −5E. 1.2 × 10 −5
You have an aqueous solution that contains a wide array of different ions along with a solid chunk of Ag3PO4 (Ksp = 9.8 × 10 −21) in it. The concentration of PO 43− in the solution is 2.0 × 10 −2 M. What is the concentration of the silver ion?A. 9.9 × 10 −6 MB. 4.4 × 10 −6 MC. 7.9 × 10 −7 MD. 2.6 × 10 −7 ME. 2.3 × 10 −6 M
Calculate the solubility of silver oxalate, Ag 2C2O4, in pure water. [Ksp = 1.0 x 10-11]A) 1.4 x 10-4 MB) 8.2 x 10-5 MC) 5.4 x 10-5 MD) 3.2 x 10-6 ME) 2.5 x 10-12 M
Which is the ion product expression for magnesium ammonium phosphate, MgNH4PO4.a) [Mg2+][NH4+][PO43-] b) [PO43-] / [Mg2+][NH4+]c) [Mg2+NH4+][PO43-]d) [Mg2+][NH4+] / [PO43-] e) 1 / [Mg2+][NH4+][PO43-]
Arrange the compounds in increasing order of molar solubility.
If 147 g of ZnF2 (K sp = 0.0300) is added to water to make a 1.00 L solution, what is the [F− ] concentration in the solution in molarity?
A. 0.173
B. 0.196
C. 0.391
D. 1.42
E. 2.84
What is the pH in a saturated solution of hypothetical metal (III) hydroxide, M(OH) 3, Ksp = 1.9 x 10-16?A. 3.81B. 10.19C. 9.71D. 4.29E. 10.31
The concentration of silver ions, [Ag+], in a saturated solution of Ag 2CO3 is 2.5x10-4 M at 25.0°C. Determine the Ksp for Ag 2CO3 at this temperature.A. 5.0 x 10-10B. 1.3 x 10-7C. 3.1 x 10-8D. 6.3 x 10-11E. 7.8 x 10-12
Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. K sp (AgBr) = 7.7 × 10-13.
What is the molar solubility of barium nitrate, Ba(NO 3)2, which has a Ksp value of 4.6 × 10−3 ?
What is Ksp for PbCrO4, if its molar solubility is 1.3 × 10−7 mol/L?
Solid silver phosphate is allowed to equilibrate with water at 25°C until the solution is saturated. What is the silver ion concentration in this saturated solution? Ksp for Ag3PO4 is equal to 8.9 × 10−17 .
Enter the Ksp expression for the solid AB 2 in terms of the molar solubility x. Express your answer in terms of x.
Silver carbonate, Ag2CO3 is a salt of low solubility. When placed in water, it dissolves until an equilibrium is reached:Ag2CO3 (s) ⇋ 2 Ag+ (aq) + CO32- (aq).Write an expression for the solubility product constant, Ksp, of Silver Carbonate?
Silver Chromate, Ag2CrO4, has a Ksp of 9.0 x 10 -12. Calculate the solubility, in moles per liter, of silver chromate.
C2D3 has a solubility product constant of 9.14 x 10 -9. What is the molar solubility of C2D3?
Enter the solubility-product expression for Mg 3(PO4)2(s). Include Charges.
Enter the Ksp expression for A2B3(s) in terms of [A] and [B].
Enter the Ksp expression for AC4(s) in terms of [A] and [C].
If the Ksp of a Ag3PO4 is 1.8 x 10-18, what is the silver ion concentration in a saturated solution of silver phosphate?a. 4.8 x 10 -5 Mb. 1.2 x 10 -5 Mc. 1.6 x 10 -5 Md. 3.2 x 10 -5 M
Consider the following chemical equation:AaBb(s) → aA+(aq) + bB-(aq)In this case, the Ksp is given by:a. Ksp = a [A+] b [B-]b. Ksp = ([A+] / a) ([B-] / b)c. Ksp = [A+] [B-] / [AaBb]d. Ksp = [A+]a [B-]be. Ksp = [A+]a [B-]b / [AaBb]
Enter the Ksp expression for C2D3 in terms of the molar solubility x.
Select the false statement below regarding PbI 2 (Ksp = 7.9 x 109) and PbCO3 (Ksp = 7.4 x 1014).A. the molar solubility of PbI 2 can be calculated by taking the cube root of (K sp/4)B. PbCO3 is more soluble in 1.0 M HCl than in pure waterC. PbI2 is less soluble in 1.0 M NaI than in pure waterD. PbCO3 is more soluble in 1.0 M Pb(NO 3)2 than in pure waterE. PbI2 is more soluble in 1.0 M NaOH than in pure water (Kf of Pb(OH) 2 = 8 x 1013)
Calculate the molar solubility of barium fluoride in each of the following. Express all answers using three significant figures.Part A pure water.Part B 0.10 M Ba(NO3)2Part C 0.15 M NaF
Consider the reactionYZ(s) ⇌ Y(aq) + Z(aq)at equilibrium. If Ksp < [Y][Z], precipitation occurs.The reaction quotient, Q, is also equal to [Y][Z]. Q is equal to Ksp only at equilibrium. When Q is less than Ksp, the solution is unsaturated; when Q is greater than Ksp the solution is supersaturated and precipitation could occur.a. Enter the Ksp expression for A 2B3(s) in terms of [A] and [B].b. Enter the Ksp expression for AC 4(s) in terms of [A] and [C].Express your answer in terms of [A] and [C].
What concentration of SO32– is in equilibrium with Ag2SO3(s) and 1.00 × 10-3 M Ag+?
The Ksp of AgCl is 1.6 x 10-10. What is the solubility of AgCl in 0.10 M AgNO 3?
What concentration of SO32- is in equilibrium with Ag 2SO3(s) and 2.90 x 10-3 M Ag+? The Ksp of Ag2SO3 can be found here: 1.5 x 10-14.
The Ksp for PbI2(s) is 1.4 x 10-8. Calculate the solubility of PbI 2(s) in 0.075 M Nal.
Calculate the molar solubility of lead thiocyanate in 0.500 M KSCN?
What is the Ksp expression for CaF2?
Give the expression for the solubility product constant for PbCl 2.a. [Pb2+][Cl-]2b. [Pb2+]2[Cl-] / [PbCl2]c. [PbCl2] / [Pb2+][Cl-]2d. [Pb2+]2[Cl-]e. [Pb2+][Cl-]2 / [PbCl2]
Calculate the molar solubility of CaF2. Given; Ksp = 4.0 x 10 -11.
Which of the following compounds will have the highest molar solubility in pure water?a. Ag2S, Ksp = 6.0 × 10−51b. ZnS, Ksp = 2.0 × 10−25c. ZnSe, Ksp = 3.6 × 10−26d. PbS, Ksp = 9.04 × 10−29e. Fe(OH)3, Ksp = 2.79 × 10−39
Determine the molar solubility of BaF 2 in a solution containing 0.0750 M LiF. K sp (BaF2) = 1.7 × 10 -6.a. 2.3 × 10 -5 Mb. 1.2 × 10 -2 Mc. 8.5 × 10 -7 Md. 3.0 × 10 -4 Me. 0.0750 M
Lead thiocyanate, Pb(SCN)2, has a Ksp value of 2.00 × 10−5.Part A. Calculate the molar solubility of lead thiocyanate in pure water. The molar solubility is the maximum amount of lead thiocyanate the solution can hold. Express the molar solubility numerically.Part B. Calculate the molar solubility of lead thiocyanate in 1.00 M KSCN. Express the molar solubility numerically.
Calculate the molar solubility of Ni(OH) 2 when buffered at pH = 8.0. Express your answer using one significant figure.
What is the minimum S2− concentration that will cause ZnS to start precipitating from a 0.10 M solution of Zn(NO3)2, a very soluble salt? Ksp for ZnS is 1.1 × 10−21.
The Ksp of nickel (II) hydroxide, Ni(OH)2, is 5.84 x 10-16. Calculate the solubility of this compound in g/L.
AgCl would be least soluble at 25°C in ______ .
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, 14.0? The Ksp is 4 x 10-16.
Which of the following compounds will have the highest molar solubility in pure water ?a. FeS, Ksp = 3.72 x 10 -19b. PbS, Ksp = 9.04 x 10 -29c. MgCO3, Ksp = 6.82 x 10 -6d. PbSO4, Ksp = 1.82 x 10 -8e. AgI, Ksp = 8.51 x 10 -17
What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO3)2? Ksp = 6.65 × 10−18 for M(OH)2.Calculate the molar solubility of lead (II) thiocyanate in 0.600 M KSCN.? K sp=2.00 x 10-5
What is the solubility of M(OH) 2 in a 0.202 M solution of M(NO 3)2? Ksp = 9.05 x 10 -18
The Ksp for Ag3PO4 is 1.8 x 10-18. Calculate the molar solubility of Ag 3PO4.
Silver Chromate (Ag2CrO4, 331.73 g/mol) has a Ksp of 1.12 x 10 -12.a) Calculate the solubility (in g/L) of silver chromate in water.b) Calculate the solubility (in g/L) of silver chromate in 0.110 M AgNO 3 solution.
Complete the following solubility constant expression for PbF2. Ksp =
Express Ksp in terms of molar solubility, x, for a salt with a formula of
Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal.M(OH)2 (s) ⇌ M2+ (aq) + 2OH- (aq) Ksp = 2 x 10-16M(OH)2 (s) + 2OH- (aq) ⇌ M(OH)42- (aq) Kf = 0.060Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.
What is the Ksp of Al(OH)3 if the concentration of OH– in a saturated solution of Al(OH)3 is 1.6 × 10–8 M?a. 2.6 x 10-16 b. 1.6 x 10-23c. 1.8 x 10-30 d. 2.2 x 10-32
Based on the given value of the Ksp = 5.61 x 10-11, what is the molar solubility of Mg(OH)2 in 0.190 M NaOH?
When excess solid YZ is put in water and allowed to dissolve the following equilibrium reaction occurs and the equilibrium table shown can be set up.The amount of solid that dissolves is called the molar solubility, denoted here by x. Since the concentration of the solid is constant and is not included in the Ksp expression, the equilibrium expression for the reaction is Ksp=[Y][Z], or, in terms of molar solubility, Ksp = x2.Enter the the Ksp expression for the solid AB2 in terms of the molar solubility x.Express your answer in terms of x.
Copper(I) ions in aqueous solution react with NH3(aq) according toCu+(aq) + 2 NH3(aq) → Cu(NH3)2+(aq) Kf = 6.3x1010 Calculate the solubility (in g• L-1) of CuBr(s) (Ksp = 6.3x10-9) in 0.73 M NH3(aq).
At 25°C only 0.0300 mol of the generic salt AB 3 is soluble in 1.00 L of water. What is the Ksp of the salt at 25°C? AB3(s) ⇌ A3+(aq) + 3 B-(aq)
What is the molar solubility of calcium carbonate (CaCO3) in water? The solubility-product constant for CaCO3 is 4.5 x 10-9 a. 9.0 x 10-9 b. 9.5 x 10-5 c. 8.35 d. 2.3 x 10-9 e. 6.7 x 10-5
The Ksp value for silver carbonate, Ag 2CO3 , is 8.10 x 10 -12. Calculate the solubility of Ag2CO3 in grams per liter.
A saturated solution of lead(II) iodide, PbI 2 has an iodide concentration of 3.0 x 10 -3 mol/L.a) What is the molar solubility of PbI2? b) Determine the solubility constant, Ksp, for lead (II) iodide. c) Does the molar solubility of lead (II) iodide increase, decrease, or remain unchanged with the addition of potassium iodide to the solution? Explain.
The Ksp of cobalt (ll) hydroxide, Co(OH)2, is 5.92 x 10-15. Calculate the molar solubility of this compound.
Calculate the molar solubility of CuX (K sp = 1.27 x 10 -36) in each of the following.a. - 0.26 M CuCl 2 b. - 0.19 M Na 2X
Silver sulfate (Ag2SO4) is an ionic solid that is only slightly soluble in water. When it is added to water, the reaction Ag2SO4(s) ⇌ 2 Ag+(aq) + SO42–(aq) takes place.A large amount of Ag2SO4(s) is placed in water at 25°C. Some of it dissolves and the solution at equilibrium contains 0.029 M Ag+(aq). What is the equilibrium constant for the reactionAg2SO4(s) ⇌ 2 Ag+(aq) + SO42–(aq)?A) 1.8 x 10–7B) 6.1 x 10–6C) 1.2 x 10–5D) 2.4 x 10–5E) 8.4 x 10–4
The Ksp of cadmium carbonate, CdCO3 is 1.0 x 10-12. Calculate the solubility of this compound in g/L.
The Ksp of lead(Il) hydroxide, Pb(OH)2, is 1.43 x 10 -20. Calculate the molar solubility of this compound.
The Ksp of BaSO4 is 1.1 x 10-10 at 25 °C. What mass of BaSO4 (molar mass = 233.4 g/mol) will dissolve in 1.0 L of water at 25 °C? (a) 2.6 x 10-8 g(b) 4.5 x 10-8 g (c) 1.0 x 10-5 g (d) 1.6 x 10-4 g (e) 2.4 x 10-3 g
The Ksp of iron(II) hydroxide, Fe(OH)2, is 4.87 x 10-17. Calculate the solubility of this compound in g/L.
i) What is the solubility of M(OH) 2 in pure water? Ksp = 5.45 x 10 -18 ii) What is the solubility of M(OH) 2 in a .202 M solution of M(NO 3)2?
Solid aluminum phosphate, AlPO4, is in equilibrium with its ions in solution:AlPO4 ↔ Al +3 +PO4 3- with Ksp = 1 x10 -22HINT: Note the definition of "solubility product".Find the concentration of phosphate ions (in mg/L)
Enter the solubility-product expression for Al(OH)3(s).
Barium hydroxide, Ba(OH)2, is reported to have a Ksp of 2.55 x 10-4 at 25 degrees celsius.a. What is the molar solubility of Ba(OH) 2?b. What is the solubility of Ba(OH) 2 in g/L?
The Ksp of zinc hydroxide, Zn(OH)2, is 3.00 x 10 -17. Calculate the molar solubility of this compound.
The Ksp of calcium hydroxide, Ca(OH)2, is 5.02 x 10-6. Calculate the molar solubility of this compound.
Calculate the solubility of Co(OH)2 (g/L) in water at 25°C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits.
The Ksp of scandium fluoride, ScF3, is 5.81 x 10-24. Calculate the molar solubility of this compound.
The molar solubility of ZnS is 1.6 x 10–12 M in pure water. Calculate the Ksp for ZnS.a. 3.2 x 10-12 M b. 1.6 x 10-35 M c. 2.6 x 10-24 M d. 8.0 x 10-13 M
What concentration of the lead ion, Pb2+, must be exceeded to precipitate PbF2 from a solution that is 1.00x102 M in the fluoride ion, F? Ksp for lead(II) fluoride is 3.3x108.