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Solubility

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Wize University Chemistry Textbook > Chemical Reactions

Solubility Rules and Precipitation

4 Activities

Wize High School Grade 12 Chemistry Textbook > Acids and Bases

Solubility Product Constant, Ksp

4 Activities

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A student is preparing to test the molar solubility of PbHPO4 (s) (Ksp=3.5Γ—10βˆ’12) in different aqueous solutions. When this salt dissociates, it produces Pb2+ (aq) and the amphiprotic ion HPO42βˆ’ (aq).They prepare separate beakers with 100 mL of each of the following solutions to test:
  1. water
  2. 0.1 M Pb(NO3)2 (aq) (which fully dissociates in water)
  3. 1.0 M HCβ„“ (aq)
  4. 0.001 M NaOH (aq)
Unfortunately, the student forgot to label which beaker is which! They continue with their experiment and ranked each solution in terms of the molar solubility of PbHPO4 (s) in that solution. Use their data to complete the bottom row of the table below, and determine which solution is in which beaker.
More Solubility Rules and Precipitation Questions:
Practice: Ranking Solubilities
You have a series of beakers, each containing 100 mL of a different solution. If you added nickel (II) hydroxide (Ni(OH)2) to each of the beakers, rank them in order of the relative solubility of the Ni(OH)2 in each:
𝑁𝑖(𝑂𝐻)2(𝑠)β‡Œπ‘π‘–2+(π‘Žπ‘ž)+2π‘‚π»βˆ’(π‘Žπ‘ž)𝐾𝑠𝑝=6.0Γ—10βˆ’16𝑁𝑖(𝑂𝐻)_2 (𝑠) β‡Œπ‘π‘–^{2+} (π‘Žπ‘ž)+2𝑂𝐻^βˆ’ (π‘Žπ‘ž) \qquad \qquad 𝐾_{𝑠𝑝}=6.0Γ—10^{βˆ’16}
Additional Data:
A student adds some CuBr (s) (Ksp = 6.3x10βˆ’9) to each of the flasks shown here.
Assume that any salts in each flask were fully dissociated before CuBr(s) was added.
Additional data:
Solubility
Which of the following compounds is soluble in water at 25 Β°C?
Solubility: Dissociation of ions
What ions does Na2CO3 dissociate into in water?
Solubility
Which of the following compounds is soluble in water at 25 Β°C?
Solubility
Which of the following correctly describes what happens when aqueous solutions of ammonium carbonate, (NH4)2CO3, and potassium bromide, KBr, are mixed?
Does a precipitate form if Pb(NO3)2 is mixed with NaBr?
Solubility
Which of the following correctly describes what happens when aqueous solutions of ammonium carbonate, (NH4)2CO3, and potassium bromide, KBr, are mixed?
Solubility
If we mixed KCl(aq) and Pb(ClO3)2(aq) would a precipitate form? If yes, name the precipitate.
Enter the answer as either no or yes, chemical formula of precipitate
Solubility
If we mixed 2AgNO3(aq) and MgBr2 would a precipitate form? If yes, what would the precipitate be?
Enter answer as either no or yes, chemical formula of precipitate.
Does a precipitate form if Pb(NO3)2 is mixed with NaBr?
Enter no or yes, name of formula of precipitate
For PbCl2 (Ksp = 2.4 x 10–4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10-2 M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2 M NaCl?
If 4.5g of NaCl are added to a 2.0 L saturated solution of AgCl, what mass of AgCl(s) will precipitate? Ksp for AgCl is 1.7 x 10-17
Solubility: Rules and mechanisms
You have a series of beakers, each containing 100 mL of a different solution. If you added nickel (II) hydroxide (Ni(OH)2) to each of the beakers, rank them in order of the relative solubility of the Ni(OH)2 in each:
𝑁𝑖(𝑂𝐻)2(𝑠)β‡Œπ‘π‘–2+(π‘Žπ‘ž)+2π‘‚π»βˆ’(π‘Žπ‘ž)𝐾𝑠𝑝=6.0Γ—10βˆ’16𝑁𝑖(𝑂𝐻)_2 (𝑠) β‡Œπ‘π‘–^{2+} (π‘Žπ‘ž)+2𝑂𝐻^βˆ’ (π‘Žπ‘ž) \qquad \qquad 𝐾_{𝑠𝑝}=6.0Γ—10^{βˆ’16}
Additional Data:
Solubility: Will a Precipitate Form?
The Ksp for strontium fluoride SrF2 is 4.3x10βˆ’9. If 5.0 x10βˆ’6 mol of NaF (s) are added to 10.0 mL of 1.5x10βˆ’3 M Sr(NO3)2, will a precipitate form? Assume that any sodium salts or nitrate salts fully dissociate in water.
The Ksp for CuBr is 6.3x10βˆ’9. When 1.00 mL of 0.0010 M CuNO3 is mixed with 1.00 mL of 0.0010 M NaBr, will a precipitate form? Assume that any sodium salts or nitrate salts fully dissociate in water.
Which of the following would decrease the Ksp for PbI2?
For PbCl2 (Ksp = 2.4 x 10–4), will a precipitate of PbCl2 form when 0.10 L of 3.0 x 10-2 M Pb(NO3)2 is added to 400 mL of 9.0 x 10-2 M NaCl?
A student adds some CuBr (s) (Ksp = 6.3x10βˆ’9) to each of the flasks shown here.
Assume that any salts in each flask were fully dissociated before CuBr(s) was added.
Additional data:
Solubility: Practice
A student is preparing to test the molar solubility of PbHPO4 (s) (Ksp=3.5Γ—10βˆ’12) in different aqueous solutions. When this salt dissociates, it produces Pb2+ (aq) and the amphiprotic ion HPO42βˆ’ (aq). They prepare separate beakers with 100 mL of each of the following solutions to test:
water
0.1 M Pb(NO3)2 (aq) (which fully dissociates in water)
Molecular bonding: Physical Properties
Consider two liquids: pentane, C5H12, and a light mineral oil, C12H26.
a. In the table below identify which liquid is being described.
b. A student observed that a drop of water spreads on a glass surface while on a paraffin coated glass surface it beads. The student’s explanation for this is: β€œThe interaction between water and paraffin is strong because it forms a bead.” Is the student correct or incorrect? Explain
Solubility and Equilibrium
Does a precipitate of PbBr2 form if 50.0 mL of 0.0100 M Pb(NO3)2 is mixed with 50.0 mL of 0.100 M NaBr? (Ksp PbBr2 = 2.1 x 10-6)
More Solubility Product Constant, Ksp Questions:
For the following reaction, define Ksp.
SrCO3(s) <----> Sr2+(aq) + CO32-(aq)
Given the following values of Ksp for four slightly soluble sulphides at 25 Β°C.
SulphideKspCdS3.6Γ—10–29CuS8.7Γ—10–36PbS8.4Γ—10–28MnS5.1Γ—10–15\def\arraystretch{1.5} \begin{array}{c} \rm Sulphide &&K_{sp} \\ \hline CdS&& 3.6 \times10^{–29}\\ CuS && 8.7 \times10^{–36} \\ PbS&& 8.4 \times 10^{–28} \\ MnS&&5.1 \times10^{–15}\\ \end{array}
Which one of the following ions exists in the lowest concentration in a solution in which the sulphide ion concentration had been fixed at some (fairly large) constant value at 25Β°C?
Solubility Product: Ion Affects
You are trying to dissolve AgBr(s) in an aqueous solution. Which salt should you add to increase the solubility of silver bromide?
Does a precipitate of PbBr2 form if 50.0 mL of 0.0100 M Pb(NO3)2 is mixed with 50.0 mL of 0.100 M NaBr? (Ksp PbBr2 = 2.1 x 10-6)
A student is adding a saturated solution of lead (II) sulphate (Ksp = 1.3 x 10-8) to a reaction mixture but the label which used to have the concentration given is missing. Calculate the volume of solution the student needs to add in order to add 2.5 x 10-5 mol of Pb2+ ions.
The Ksp for CuBr is 6.3x10βˆ’9. When 1.00 mL of 0.0010 M CuNO3 is mixed with 1.00 mL of 0.0010 M NaBr, will a precipitate form? Assume that any sodium salts or nitrate salts fully dissociate in water.