Worksheet: Common Ion Effects

In this worksheet, we will practice using the solubility product to calculate the impact of a common ion on the dissolution or precipitation of a salt.

Q1:

In a solution of 0.025 MNaCl in contact with solid AgCl, what is [Ag]+ at equilibrium? The 𝐾sp of AgCl is 1.6×10.

  • A 7 . 9 × 1 0   M
  • B 5 . 1 × 1 0   M
  • C 1 . 6 × 1 0   M
  • D 4 . 0 × 1 0   M
  • E 6 . 4 × 1 0   M

Q2:

The solubility product of CaSO·2HO42 is 2.4×10. What mass of this salt will dissolve in 1.0 L of a solution with a SO42– concentration of 0.010 M?

Q3:

In a 0.00133 M solution of KF in contact with solid CaF2, what is [Ca]2+ at equilibrium? The 𝐾sp of CaF2 is 4.0×10 Give your answer to two significant figures.

  • A 1 . 2 × 1 0   M
  • B 1 . 3 × 1 0   M
  • C 4 . 4 × 1 0   M
  • D 2 . 3 × 1 0   M
  • E 5 . 1 × 1 0   M

Q4:

What is the concentration of sulfate ions when BaSO4 just begins to precipitate from a solution that is 0.0758 M in Ba2+? The 𝐾sp of BaSO4 is 2.3×10.

  • A 3 . 0 3 × 1 0   M
  • B 2 . 3 0 × 1 0   M
  • C 1 . 2 1 × 1 0   M
  • D0.0758 M
  • E 6 . 0 7 × 1 0   M

Q5:

What is the concentration of PO43– when AgPO34 starts to precipitate from a solution with an Ag+ concentration of 0.0125 M? The 𝐾sp of AgPO34 is 1.8×10 Give your answer to two significant figures.

  • A 1 . 4 × 1 0    M
  • B 3 . 0 × 1 0    M
  • C 1 . 2 × 1 0    M
  • D 2 . 3 × 1 0    M
  • E 9 . 2 × 1 0    M

Q6:

What is the concentration of Sr2+ when SrF2 starts to precipitate from a solution that is 0.0035 M in F–? The 𝐾sp of SrF2 is 4.3×10. Give your answer to two significant figures.

  • A 1 . 2 × 1 0   M
  • B 5 . 2 × 1 0   M
  • C 3 . 5 × 1 0   M
  • D 3 . 0 × 1 0   M
  • E 4 . 5 × 1 0   M

Q7:

For 0.500 L of a solution containing 19.50 g of KSO24 in contact with solid AgSO24, what is [Ag]+ at equilibrium to two significant figures? The 𝐾sp of AgSO24 is 1.2×10.

  • A 7 . 3 × 1 0   M
  • B 7 . 4 × 1 0   M
  • C 1 . 4 × 1 0   M
  • D 6 . 4 × 1 0   M
  • E 1 . 3 × 1 0   M

Q8:

A sample of CoCO3 (𝐾=1.0×10sp) is contaminated with 0.1 g of NiCO3 (𝐾=1.36×10sp). The sample is treated with the minimum amount of water required to completely dissolve the NiCO3. Noting that the two carbonate salts dissolve in the same volume of water, calculate the mass of CoCO3 that is also washed away.

  • A 4 × 1 0   g
  • B 5 × 1 0   g
  • C 7 × 1 0   g
  • D 6 × 1 0    g
  • E 1 × 1 0    g

Q9:

A solution contains 0.010 M of both Cu2+ and Cd2+. Sulfide ions are added to the solution until 99.9% of the Cu2+ ions have been precipitated as CuS. Calculate the percentage of Cd2+ ions remaining in the solution. The 𝐾sp value of CuS is 8.5×10 and that of CdS is 1.0×10.

Q10:

In a solution of 0.025 M TlNO3 in contact with solid TlCl, what is [Cl]– at equilibrium? The 𝐾sp of TlCl is 1.7×10 Give your answer to two significant figures..

  • A 5 . 6 × 1 0   M
  • B 4 . 3 × 1 0   M
  • C 6 . 8 × 1 0   M
  • D 6 . 0 × 1 0   M
  • E 4 . 8 × 1 0   M

Q11:

In 2.250 L of solution containing 8.156 g of Mg(NO)32 in contact with solid MgCO24, what is [CO]242– at equilibrium? The 𝐾sp of MgCO24 is 7.0×10 Give your answer to two significant figures.

  • A 2 . 9 × 1 0   M
  • B 7 . 2 × 1 0   M
  • C 6 . 4 × 1 0   M
  • D 3 . 1 × 1 0   M
  • E 8 . 0 × 1 0   M

Q12:

In a solution of 0.0313 MKF in contact with solid BaF2, what is [Ba]2+ at equilibrium? The 𝐾sp of BaF2 is 1.84×10. Give your answer to three significant figures.

  • A 2 . 0 1 × 1 0   M
  • B 1 . 7 3 × 1 0   M
  • C 1 . 8 8 × 1 0   M
  • D 6 . 5 0 × 1 0   M
  • E 1 . 5 9 × 1 0   M

Q13:

How many grams of Pb(OH)2 (𝐾=1.2×10)sp will dissolve in 500 mL of a 0.050 MPbCl2 solution?

  • A 9 . 3 × 1 0   g
  • B0.16 g
  • C 4 . 8 × 1 0   g
  • D 8 . 1 × 1 0   g
  • E 1 . 2 × 1 0    g

Q14:

A solution contains all of the following carbonates at the same concentration. If [CO]32– is gradually increased, which carbonate is first to precipitate?

  • A M n C O 3 ( 𝐾 = 5 . 1 × 1 0 ) s p  
  • B M g C O 3 ( 𝐾 = 3 . 5 × 1 0 ) s p  
  • C C a C O 3 ( 𝐾 = 4 . 2 × 1 0 ) s p  
  • D B a C O 3 ( 𝐾 = 4 . 4 × 1 0 ) s p  
  • E S r C O 3 ( 𝐾 = 3 . 9 × 1 0 ) s p  

Q15:

A solution contains all of the following carbonates at the same concentration. If [CO]32– is gradually increased, which carbonate is last to precipitate?

  • A M n C O 3 s p  𝐾 = 5 . 1 × 1 0   
  • B S r C O 3 s p  𝐾 = 3 . 9 × 1 0   
  • C B a C O 3 s p  𝐾 = 4 . 4 × 1 0   
  • D C a C O 3 s p  𝐾 = 4 . 2 × 1 0   
  • E M g C O 3 s p  𝐾 = 3 . 5 × 1 0   

Q16:

Which of the following, if added to a mixture of solid CaHPO4 and water at equilibrium, would decrease the solubility of CaHPO4?

  • A K C l O 4
  • B C a C l 2
  • C H C l
  • D N a B r
  • E C a H P O 4

Q17:

Which of the following, if added to a mixture of solid CaHPO4 and water at equilibrium, would increase the solubility of CaHPO4?

  • A C a C l 2
  • B C a H P O 4
  • C H C l
  • D N a B r
  • E K C l O 4

Q18:

A mixture of CaCO3, SrCO3, and BaCO3 contains 350 mg of each of the salts. What volume of 1.50 M aqueous CHCOH32 is required to dissolve this solid material?

Q19:

If solid Mg(OH)2 were dissolved in 0.01 M aqueous solutions of the following compounds, in which solution would the most solid dissolve per unit volume?

  • A M g ( O H ) 2
  • B H C l O 4
  • C N a C l
  • D N a N O 3
  • E M g C l 2

Q20:

H S 2 is added to a 0.125 M solution of Mn(NO)32 until the solubility limit of 0.100 M is reached. The solutes react to form MnS according to the following equations. MnS()Mn()+S()HS()+2HO()2HO()+S()saqaqaqlaqaq2+2–sp223+2–,𝐾=4.3×10,𝐾=1.0×10 Adding acid to the solution causes precipitation of the MnS product. To 2 decimal places, at what pH does MnS begin to precipitate?

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