A nitric acid solution is composed of 63.75 g of HNO3 and 205.65 mL of pure...

A nitric acid solution is composed of 63.75 g of HNO3 and 205.65 mL of pure water. What is the percent by mass of the nitric acid solution? Use the density of water as 0.9984 g/mL.

Solutions

Expert Solution

water mass = volume x density

= 205.65 x 0.9984

= 205.32 g

% mass of HNO3 = (mass of HNO3 / total mass ) x 100

= (63.75 / 63.75 + 205.32) x 100

= 23.69 %

queen_honey_blossom answered 1 year ago

Next > < Previous

Related Solutions

20.0 mL of nitric acid (HNO3) solution is neutralized with 30.0 mL 0.10M of potassium hydroxide...

20.0 mL of nitric acid (HNO3) solution is neutralized with 30.0 mL 0.10M of potassium hydroxide (KOH) solution. what is the concentration of nitric acid solution? The answer is 0.67 M but how do you get that?

A solution is made by mixing 25.0 mL of 0.250 M nitric acid (HNO3) with 15.0...

A solution is made by mixing 25.0 mL of 0.250 M nitric acid (HNO3) with 15.0 mL of 0.500 M sodium hydroxide (NaOH). What is the resulting concentration of each ion in solution?

A concentrated nitric acid solution has a density of 1.41 g/mL at 25C and is 15.8...

A concentrated nitric acid solution has a density of 1.41 g/mL at 25C and is 15.8 M. What is the percent by mass of HNO3 in the solution? a. 70.6 % HNO3 by mass b. 1.12% c. .895 % d. 1.77 % e. 44.7% how do i identify which one is the solute and solvent of the two numbers given? and the correct answer is supposedly 70.6% from the solution :) thank you for you help!

It takes 25 ml of 0.40 M nitric acid solution to completely neutralize 50.0 ml of...

It takes 25 ml of 0.40 M nitric acid solution to completely neutralize 50.0 ml of 0.20 M NH3 solution (i.e. to reach the equivalence point). What is the pH of the equivalence point?(Kb NH3 = 1.8x10^-5)

A 7.81 g sample of an aqueous solution of nitric acid contains an unknown amount of...

A 7.81 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 23.2 mL of 1.68 M potassium hydroxide are required to neutralize the nitric acid, what is the percent by mass of nitric acid in the mixture?

Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and...

Nitric acid is usually purchased in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g/mL. How much concentrated solution would you take to prepare 1.00 L of 0.115 M HNO3 by mixing with water?

titration of 17.85 ml of nitric acid solution require 16ml of 0.16 M KOH solution. what...

titration of 17.85 ml of nitric acid solution require 16ml of 0.16 M KOH solution. what is the polarity of the acid?

Pure (100%) sulfuric acid has a density of 1.84 g/ml. How many mL of sulfuric acid...

Pure (100%) sulfuric acid has a density of 1.84 g/ml. How many mL of sulfuric acid need to be diluted with water to a total volume of 500 mL to prepare a solution with pH=0.500

A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M...

A 0.4000 M solution of nitric acid is used to titrate 50.00 mL of 0.237 M barium hydroxide. Using this information, complete the following: A.) Write a net ionic equation for the reaction that takes place during titration B.) What species are present at the equivalence point? C.) What volume is nitric acid is required to reach the equivalence point?

Consider the following series of balanced chemical reactions in the production of nitric acid, HNO3: 4...

Consider the following series of balanced chemical reactions in the production of nitric acid, HNO3: 4 NH3 + 5 O2 -----------> 4 NO + 6 H2O 2 NO + O2 -----------> 2 NO2 3 NO2 + H2O ------------> 2 HNO3 + NO If O2 and H2O are not limiting, how many grams of nitric acid, HNO3 (F.M. = 63.02), can be produced from the reaction of 120.0 g of ammonia, NH3 (F.M. = 17.04)? For your calculation, use the given...

Subjects