What is Ksp for calcium hydroxide if the concentration of OH in a saturated calcium hydroxide solution was found to be 0.0412 M? Select one: a. 3.78 x 10-5 M O b. 1.40 x 10-4 M O c. 2.80 x 104 M O d. 3.50 x 10-5 M O e. 5.5 x 10-6 M

A buffered solution containing dissolved aniline, C,H,NH,, and aniline hydrochloride, C,H;NH;CI, has a pH of 5.50. A. Determine the concentration of C,H,NH in the solution if the concentration of C,H,NH, is 0.305 M. The pKp of aniline is 9.13. [C,H;NH | 0.0715 M B. Calculate the change in pH of the solution, ApH, if 0.374 g NaOH is added to the buffer for a final volume of 1.05 L. Assume that any contribution of NaOH to the volume is negligible. 0.05 ApH = Incorrect

Barium sulphate is a relatively insoluble salt used for medical radiographs of the gastrointestinal tract: BaSO4 (s) Ba2+ (aq) + SO4²- (aq) The concentration of Ba2+ ions in a saturated aqueous solution is 1.05×105 M. Determine Ksp for barium sulphate dissolving in water. O 1.12 x 10-5 O 1.05 x 1025 O 2.12 x 10-5 1.10 x 10-25 O 1.10 x 10-10

19. A student prepared a 250.0 mL solution by dissolving 4.559 g of (NH4)2SO4 in enough water. The temperature is 298 K. The base dissociation constant for NH3 is 1.796x10-5. Please answer the following questions. A. B. What is the equilibrium concentration of H3O+ in the solution? Please provider your answer below. 00 + → What is the equilibrium concentration of OH in the solution? Please provider your answer below. OO → $ → $ C. What is the pH of the solution? pH = Please provider your answer below. S M M

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At what pH will an aqueous solution of 1.2 M Mg2+ begin to precipitate as Mg(OH)? The Ksp of Mg(OH)2 is 3.6 x 104. O a. 1.8 ОБ. 3.5 OC. 11.2 O d. 12.3 O e. 10.5

A 1.00 liter solution contains 0.54 M ammonia and 0.42 M ammonium chloride. If 0.21 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) vA. The number of moles of NH3 will increase. v B. The number of moles of NH.* will remain the same. v C. The equilibrium concentration of H3O* will increase. vD. The pH will decrease. E. The ratio of [NH3] / [NH4*] will decrease.

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