Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.
The concept used in this problem is based on the solubility product.
Find the molar solubility of a given compound in the specific solution with the help of expression of solubility product.
Solubility product:
Solubility product basically defines the equilibrium between solids and its respective ions in the solution. The value of the solubility product represents the degree to which a chemical compound dissociates in water.
Example –
The dissociation reaction of ionic solid is given as shown below.
The expression corresponding to the solubility product is given as shown below.
The balanced chemical equation for the dissociation reaction of is as follows:
The expression corresponding to the solubility product is given as shown below.
…… (1)
The molar solubility of is calculated as shown below.
Consider the is the molar solubility of the given compound.
Substitute as the concentration of bromide ion and as the of in the equation .
Ans:The molar solubility of is .
Determine the molar solubility of AgBr in a solution containing 0.150 M NaBr. Ksp (AgBr) = 7.7 × 10-13.
Determine the molar solubility of AgBr in: Ksp (AgBr) = 7.7 x 10^ -13 a. a solution of pure water b. a solution containing 0.150 M NaBr c. A solution containing 0.25 M NaCL
Determine the molar solubility of AgBr in a solution containing 0.200 M NaBr. Ksp (AgBr) = 7.7 × 10-13. a. 3.8 × 10-12 M b. 5.8 × 10-5 M c. 0.200 M d. 8.8 × 10-7 M e.1.54 × 10-13 M
please solve and show work! Determine the molar solubility of AgBr in a solution containing 0.250 M MgBr2 (strong electrolyte). Ksp (AgBr) = 7.7 x 10-13 O A.8.8 x 107 M B.5.1 x 10-12 M c. 1.5 x 10-12 M O 0.5.8 x 10-5 M E.0.150 M
calculate the molar solubility of AgBr (Ksp = 7.7×10^-13) in a 5.0 x10^-6 M AgNO3 (aq) solution.
The Ksp of AgBr is 5.4x10^-13. What is the molar solubility of AgBr? The Ksp of AgBr is 5.4 x 10-13. What is the molar solubility of AgBr? 8.64 x 10-13 7.35 x 10-7 2.43 x 10-12 Not enough information 5.4x 10-13
1. what is the solubility of AgBr with a Ksp of 5.0x10-13 in 0.1M NaBr? Did you expect this to be higher or lower than the solubility of AgBr by itself? 2. Would you expect the solubility of AgBr to be significantly pH dependent? why or why not? 3. The Ksp of Mg(OH)2 is 1.8x10-11 at 25C. What is the pH of a saturated solution of Mg(OH)2 at 25C? 4. Would Mg(OH)2 be more soluble in water or a solution...
Determine the molar solubility of AgBr (Ksp = 5.40e-13) in 2.983 M NH3 if the complex ion [Ag(NH3)2]+ forms with a Kf = 1.70e7. 3.012e-3 0.01136 8.984e-3 7.104e-3
Determine the molar solubility of CuCl in a solution containing 0.030 M LiCl. Ksp (CuCl) = 1.7×10-7. Determine the molar solubility of CuCl in a solution containing 0.030 M LiCl. Ksp (CuCl) = 1.7×10-7. 4.1×10-4 M 2.9×10-14 M 5.7×10−6 M 5.1×10−9 M 4.7×10−5 M
) Determine the molar solubility of HgCO3 in a solution containing 0.080 M K2CO3. Ksp (HgCO3) = 9.0 x 10-15.
Bonus 1: (5 Pts Max; partial credit allowed.) What is the MOLAR solubility of AgBr in (a) pure water and (b) 0.005 M NaBr? Ksp for silver bromide is 7.7, x 10 , T