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suppose of barium nitrate is dissolved in of a aqueous solution of sodium chromate. calculate the final molarity of nitrate anion in the solution. you can assume the volume of the solution doesn't change when the barium nitrate is dissolved in it. round your answer to significant digits.



Answer :

varshamittal029

The nitrate anion molarity in the solution is 0.173 M.

Molar concentration is a unit of measurement for the concentration of a chemical species, specifically a solute, in a solution, expressed as the amount of substance per unit volume of solution.

The balanced equation

Ba(NO3)2(aq) + Na2CrO4 (aq) → BaCrO4(s) + 2NaNO3(aq)

Mass of nitrate = 13.6 grams

Volume of 0.40M sodium chromate = 300 mL

Step 3: Calculate moles of Ba(NO3)2

Moles = mass / molar mass

Moles = 13.6 grams / 261.34 g/mol

Moles = 0.052 moles

Calculate moles of Na2CrO4

Moles = Molarity * Volume

Moles Na2CrO4 = 0.40 * 0.3L

Moles Na2CrO4 = 0.12 moles

Na2CrO4 is in excess so all of Ba(NO3)2 will be consumed and reacts to form BaCrO4(s) in the form no3

n(Ba2+)=n(BaCrO4) =n(Ba(NO3)2 = 0.0520 moles

C=n/v so C(Ba2+)=0.0520/0.300 = 0.173 M

The molarity of nitrate anion in the solution is 0.173 M

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