Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO₃ by mass in the solution.

Video transcript

Hello everyone today, we are being given the following question and asked to solve for it, It says the density of a commercial sulfuric acid solution is 1.84 g per minute leader as a concentration of 18 Moeller. Were then asked to calculate the mass percent of the solution. So in situations like such, we have to assume that we're working with one liter of solution and so we have to calculate the mass of that one liter solution. So we take our one leader and we convert that to middle leaders. So we'll say that one millimeter is equal to 10 to the negative third leaders. And then we're gonna go ahead and we're going to multiply by our density. So that's going to be 1.84 g per one mil liter. And once our units cancel out, we're left with 1840 g of our solution. Next we have to calculate the mass of our sulfuric acid, which is H. Two S. 04. And so first we can say that the molar mass Of this H two s. 04 is going to be equal to 98.09 g per mole. And so starting out with our mill arat E of our H two S. 04, we have 18 moles of H two S. 0. 4/1 leader or solution. We're going to multiply that by our molar mass and we're gonna say that one mole of this H two S. 04 is going to be equal to its molar mass of 98.9 g to give us 1756. g of H two S. 04 or for sulfuric acid. Lastly, we must calculate our mass percent. So we're gonna say our mass percent is going to be equal to our 65 or the mass of the sulfuric acid. We're gonna say H two S. 04 here, we're gonna place that over our 18 40 g of our solution And we're gonna multiply that by 100% to give us 95.96%. I hope this helped. And until next time.