the solubility of Ba(IO3)2 in a solution prepared by mixing 300 mL of 0.010 M Ba(NO3)2 with 200 mL of 0.10 M NaIO3 .(K.S.P=1.57X 10-9) is

a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3g/molb)  Solubility product, Kspc) Vapor pressure of the solution in kPa

When 200.0 mL of 5.15 x 10-4 M Ba(NO3)2 is added to 150.0 mL of 8.25 x 10-4 M Na2SO4. Ksp(BaSO4) = 1.08 x 10-10. A precipitate choose your answer.... Ksp because Qsp choose your answer... choose your answer... SIGMA = form

Calculate the molar solubility of Fe(OH); (K, = 2.79 x 10-39) in a sp solution that is buffered at pH = 2.91.

Calculate the concentration of IO3 in a 8.18 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 x 10-13. Assume that Pb(IO3)2 is a negligible source of Pb²+ compared to Pb(NO3)2. [103] = M A different solution contains dissolved NaIO₂. What is the concentration of NaIO, if adding excess Pb(IO3)₂(s) produces a Pb²+ concentration of 6.90 x 10-6 M? concentration: M

a) The concentra=on of Mg2+ in seawater is 0.052 M. If the Ksp for Mg(OH)2 is 8.9 × 10–12, at what pH will >99.9% of the Mg2+ be precipitated from seawater as its hydroxide salt? b) The solubility of the ionic compound M2X3, having a molecular mass of 288 g/mol, is 3.60 × 10–7g/L. Calculate the Ksp of the compound.

Calcium hydroxide has a solubility product of Ksp = 5.02 x 10-6. What mass of calcium hydroxide can be dissolved in 1.00 L of 0.254M potassium hydroxide

The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?

Hw.128.

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