A solution containing 5.00g of solid Al2(CO3)3 dissolved in water to a total volume of 200. mL is combined with 140. mL of 1.0 M HBr.
Write the total of ionic equation for the reaction described below and find the molar concentration of all ions remaining in a solution that is prepared by mixing the compounds listed below. Assume all equeous products are saluble.
chemistry - DrBob222, Monday, April 16, 2012 at 9:35pm
I should point out that Al2(CO3)3 is not soluble in water.
Convert 5.00 g Al2(CO3)2 to mols. mol = grams/molar mass.
Convert HBr to mols mols = M x L = ?
Use the equation below to determine the limiting reagent and use that information to determine how much of each reagent remains. Then you can write the ionic equation.
Al2(CO3)3 + 6HBr ==> 2AlBr3 + 3H2O + 3CO2