What are the molar concentrations of the ions in 0.16 M aluminum sulfate?
What are the molar concentrations of the ions in 0.16 M aluminum sulfate?
What is the molar concentration of sulfate ions in a 0.500 M CS2SO4 solution? O 0.500 M 1.50 M 1.00 M 0.250 M
The following table lists molar concentrations of seven major ions in seawater. Using a density of 1.022 g/mL for seawater, convert the concentrations for the following two ions into molality. The sodium ion: The sulfate ion:
Calculate the number of sulfate ions in 7.254 x 10-4 kg of aluminum sulfate.
b. What is the molar mass of aluminum ammonium sulfate dodecahydrate? Use the periodic table in the back of the lab manual to answer this question. Formula: Molar mass of one mole of atoms x # of each species = total molar mass per element N: H: Al: S: O: Molar mass of NHAI(SO4)2·12H2O =
Calculate the molar mass of alum, KAI(SO4)2·12H20 (potassium aluminum sulfate dodecahydrate). Type the molar mass without units, to the nearest whole number.
The molar solubility of barium sulfate in a 0.216 M potassium sulfate solution is M. That is all it asks, no Ksp given.
Calculate the ratio of the molar concentrations of HPO42- and H2PO4- ions required to obtain a buffer solution at pH = 7.0. For phosphoric acid, Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13
Calculating Ksp If X = [Cs2SO4], which equation can you use to get the molar concentrations of the cesium and sulfate ions? [Cs2SO4] = [X]2 × [X] [Cs2SO4] = [2X]2 × [X] [Cs2SO4] = [2X]2 × 4[X]
What are the concentrations of H3O+ and OH- ions (in M) in an aqueous solution with a pOH of 10.17? Is this solution acidic or basic? Explain your answer.
What is the molar solubility of 7 x 10^-5 M barium sulfate?