A standard nitric acid solution is prepared using 0.425 g of sodium carbonate, N

Question

A standard nitric acid solution is prepared using 0.425 g of sodium carbonate, Na_2CO_3. Find the molarity of the acid if 33.25 mL are required to reach a permanent endpoint. 2 HNO_3 (aq) + Na_2CO_3 (s) rightarrow 2NaNO_3(aq) + H_2O(1) + CO_2(g) A 10.0-mL sample of household ammonia solution required 27.50 mL of 0.241 M HNO_3 for neutralization. Calculate the molar concentration of the ammonia and the mass/mass percent concentration of ammonia (17.04 g/mol), given a solution density of 0.985 g/mL.

Explanation / Answer

1)Based on the chemical reaction

weight take/ molar mass= 0.425g/106g/mol= 0.004 moles of Na2CO3

Na2CO3 requires 2X0.004 mole of HNO3 = 0.008moles

Molarity= moles/litre= 0.008/0.03325= 0.241 M of HNO3

2) molarity of ammonia= (molarity of HNO3 X Vol. of HNO3)/Vol. of ammonia

   =27.50 x 0.241 / 10 = 0.663 M NH3

   molar mass x moles = 17 x 0.663 = 11.30 g of NH3

solution density =0.985g/mol = 985L

11.30/985 = 0.011= 1.14%

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