Consider a saturated solution of barium iodate in 0.025 M BaCl,. For the salt: Ba(IO3)2(s)= Ba2+ + 2103 Ksp = 1.57 × 10-° at 25 deg CWhat is the concentration equilibrium constant, K'sp?O5.00x 10-98.00× 10-9O 1.57x 10-97.15×10-9

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Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) = Ba2+ + 2103 Ksp = 1.57 x 109 at 25 deg C What is the concentration equilibrium constant, K'sp? O 5.00x 10-9 O 8.00x 10-9 O 1.57x 10-9 7.15×10-9

Consider a saturated solution of barium iodate in 0.025 M BaCl2. For the salt: Ba(IO3)2(s) = Ba2+ + 2103 Ksp = 1.57 x 109 at 25 deg C What is the concentration equilibrium constant, K'sp? O 5.00x 10-9 O 8.00x 10-9 O 1.57x 10-9 7.15×10-9

Chemistry: Principles and Reactions

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Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 62QAP: Consider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this...

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A 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Kc1,1, or 1 for a titration reaction?
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
A solution is prepared by mixing 13.00 mL of 0.0021 M aqueous Hg2(NO3)2 with 25.0 mL of 0.015 M HCl. Assume that volumes are additive. (a) Will precipitation occur? (b) Calculate [Hg22+], [Cl-], and after equilibrium is established.
Consider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this solution, 4.8 g of CaCl2 are added. (a) What is [OH-] before CaCl2 is added? (b) Will a precipitate form? (c) What is [Ca2+] after equilibrium is established?
Consider a saturated solution of BaCO3 at 7.5C. Answer the following questions using LT (for is less than), GT (for is greater than), EQ (for is equal to), or write MI if more information is required. (a) At equilibrium [Ba2+] [CO32-]. (b) The temperature is increased to 2000C. The Ksp at 75C Ksp at 2000C. (c) A solution of NaNO3 is added. [Ba2+] before NaNO3 is added [Ba2+] after NaNO3 is added. (d) Solid Na2CO3 is added. After equilibrium is reestablished, [Ba2+] [CO32-].
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
A solution is prepared by mixing 45.00 mL of 0.022 M AgNO3 with 13.00 mL of 0.0014 M Na2CO3. Assume that volumes are additive. (a) Will precipitation occur? (b) Calculate [Ag+], [CO32-], [Na+], and [NO3-] after equilibrium is established.
A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?
. Under what circumstances can we compare the solubilities of two salts by directly comparing the values of their solubility products?
If 13.0 mL of 0.19 M MgCl2 are mixed with 21.9 mL of 0.54 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 ✕ 10-11 for Mg(OH)2. (in M)

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