The Ksp of BaF2 is 2.45 x 10-5. Given that value, calculate the molar concentration of Ba2+ ion in a saturated solution. (a) 3.2 x 10-4 (b) 8.00 x 10-7 (c) 1.04 x 10-5 (d) 1.83 x 10-2
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The Ksp of BaF2 is 2.45 x 10-5. Given that value, calculate the molar concentration of Ba2+ ion in a saturated solution. (a) 3.2 x 10-4 (b) 8.00 x 10-7 (c) 1.04 x 10-5 (d) 1.83 x 10-2
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- of the five salts listed below, which has the highest concentration of its cation in water? assume that all salt solutions are saturated and that the ions do not undergo any additional reactions in water. (a) lead(ii) chromate, ksp = 2.8 × 10–13 (b) cobalt(ii) hydroxide, ksp = 1.3 × 10–15 (c) cobalt(ii) sulfide, ksp = 5 × 10–22 (d) chromium(iii) hydroxide, ksp = 1.6 × 10–30 (e) silver sulfide, ksp = 6 × 10–51The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?