Consider the neutralization reaction 2 HNO_3 (aq)+Ba(OH)_2 (aq) + 2H_2O(1)+Ba(NO),(aq) A 0.105 L sample of an unknown HNO_3 solution required 37.1 mL of 0.150 M Ba(OH)_2 for complete neutralization. What is the concentration of the HNO_3 solution? concentration:

To find the concentration of HNO3 in the given reaction, we used stoichiometry and molarity calculations. The final calculated concentration of HNO3 is 0.106 M.

Explanation:

In the given chemical reaction, we know that 2 moles of HNO3 react with one mole of Ba(OH)2. Because of this stoichiometry, we can say 37.1 mL of 0.150 M Ba(OH)2 solution contains 0.150 M * 37.1/1000 L = 0.005565 moles of Ba(OH)2. Since it requires 2 moles of HNO3 to react with one mole of Ba(OH)2, there are double the amount of moles of HNO3 in the solution, which is 0.005565 moles * 2 = 0.01113 moles.

So, the molarity (concentration in moles per liter) of HNO3 in the solution is the number of moles divided by the volume of the solution in liters. Therefore, the concentration of HNO3 is 0.01113 moles/0.105 L = 0.106 M.

The concentration of the HNO3 solution is 0.106 M.

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