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Chapter 13: Problem 55

Commercial aqueous nitric acid has a density of 1.42 \(\mathrm{g} / \mathrm{mL}\) and is 16 \(\mathrm{M} .\) Calculate the percent \(\mathrm{HNO}_{3}\) by mass in the solution.

Short Answer

Expert verified
The percent HNO3 by mass in the commercial aqueous nitric acid solution is approximately 71%.

Step by step solution

01

Calculate the mass of the solution

We are given the density of the commercial aqueous nitric acid as 1.42 g/mL. To find the mass of 1 litre (1000 mL) of the solution, we can use the formula: Mass = Density × Volume Mass = 1.42 g/mL × 1000 mL Mass = 1420 g So, the mass of 1 litre of the commercial aqueous nitric acid solution is 1420 g.
02

Calculate the moles of HNO3 in 1 litre of the solution

We are given the molarity (M) of the solution as 16 M. By definition, molarity is the number of moles of solute per litre of solution. Thus, in 1 litre of the solution, we have: Moles of HNO3 = Molarity × Volume Moles of HNO3 = 16 mol/L × 1 L Moles of HNO3 = 16 mol So, there are 16 moles of HNO3 in 1 litre of the solution.
03

Convert the moles of HNO3 into mass of HNO3

Now we need to find the mass of HNO3, given the number of moles. We can use the molar mass of HNO3 to do this conversion. The molar mass of HNO3 is: HNO3: (1 × 1.01) + (1 × 14.01) + (3 × 16.00) = 1.01 + 14.01 + 48.00 = 63.02 g/mol Now, we can calculate the mass of HNO3 using the moles and molar mass: Mass of HNO3 = Moles × Molar mass Mass of HNO3 = 16 mol × 63.02 g/mol Mass of HNO3 = 1008.32 g So, the mass of HNO3 in 1 litre of the solution is 1008.32 g.
04

Calculate the percent HNO3 by mass in the solution

Finally, we can find the percent HNO3 by mass in the solution using the formula: Percent HNO3 = (Mass of HNO3 / Mass of the solution) × 100 Percent HNO3 = (1008.32 g / 1420 g) × 100 Percent HNO3 ≈ 71% Thus, the percent HNO3 by mass in the commercial aqueous nitric acid solution is approximately 71%.

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Most popular questions from this chapter

Indicate whether each statement is true or false: (a) If you compare the solubility of a gas in water at two different temperatures, you find the gas is more soluble at the lower temperature. (b) The solubility of most ionic solids in water decreases as the temperature of the solution increases. (c) The solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised. (d) Some ionic solids become less soluble in water as the temperature is raised.

An ionic compound has a very negative \(\Delta H_{\text { soln in water. }}\) (a) Would you expect it to be very soluble or nearly insoluble in water? (b) Which term would you expect to be the largest negative number: \(\Delta H_{\text { solvent }} \Delta H_{\text { solute }}\) or \(\Delta H_{\text { mix }}\) ?

Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 gof this enzyme in 210 \(\mathrm{mL}\) of solution has an osmotic pressure of 0.953 torr at \(25^{\circ} \mathrm{C}\) . What is the molar mass of lysozyme?

Arrange the following aqueous solutions, each 10\(\%\) by mass in solute, in order of increasing boiling point: glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right),\) sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right),\) sodium nitrate (\textrm{NaNO} _ { 3 } ) .

What is the osmotic pressure formed by dissolving 44.2 \(\mathrm{mg}\) of aspirin \(\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\right)\) in 0.358 \(\mathrm{L}\) of water at \(25^{\circ} \mathrm{C} ?\)
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