# Concentrated Nitric Acid Used In Laboratory Work Is 68% Nitric Acid By Mass In Aqueous Solution. What Should Be The Molarity Of Such A Sample Of The Acid If The Density Of The Solution Is 1.504 G Ml–1? (2023)

## 1. QUESTION 2.4 Concentrated nitric acid used in laboratory work is 68 ...

• Concentrated nitric acid used in laboratory work is 68%68\%68% nitric acid by aqueous solution. What should be the molarity of such a sample of the acid if the ...

• QUESTION 2.4 Concentrated nitric acid used in laboratory work is 68 % nitric acid by aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL 1 ?

## 2. Concentrated nitric acid used in laboratory work is 68 ... - Doubtnut

• Duration: 5:15Posted: Jul 21, 2023

• 68% by mass that 68g of HNO(3) is present in 100g of solution. Volume of solution =(Mass of solution )/(Density of solution ) =(100g)/(1.50gmL^(-1))=66.5cm^(3)=0.65L Molar mass, Mw(B) of HNO(3)=1+14+48=63 Molarity=(W(A))/(Mw(B)xxV) =(68g)/(63g mol^(-1)xx0.0665)=16.23M

## 3. [Gujrati] Concentrated nitric acid used in laboratory work is 68% nitr

• Duration: 5:15Posted: Feb 15, 2023

• Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in an aqueous solution. This means that 68 g of nitric acid is dissolved in 100 g of the solution. Molar mass of nitric acid (HNO(3)) = 1xx1+1xx14+3xx16 = 63 g mol^(-1) Then, number of moles HNO(3)=(68)/(63)mol = 1.079 mol Given, Density of solution = 1.504 g mL^(-1) Therefore, Volume of 100 g solution = (100)/(1.504)mL = 66.49 mL = 66.49xx10^(-3)L Molarity of solution = (1.079 mol)/(66.49xx10^(-3)L)-16.23 M

## 4. Concentrated nitric acid used in the laboratory work is 68% nitric ... - Zigya

• Answer: 68% by mass implies that 68 g of HNO3 are present in 100 g of solution. ... = 100 g 1 . 504 g mL - 1 = 66 . 5 cm 3 = 0 . 665 L . Molar mass, M B of NHO 3 ...

• Answer: 68% by mass implies that 68 g of HNO3 are present in 100 g of solution.Volume of solution = Mass of solutionDensity of solution                             = 100g1.504 g mL-1= 66.5 cm3 = 0.665 L.Molar mass,        MB of NHO3 = 1+14+48 = 63.           Molarity = ωAMB×V               = 68 g63 g mol-1 × 0.0665               = 16.23 M.

## 5. Concentrated nitric acid used in laboratory work is ... - Shaalaa.com

• Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in an aqueous solution. This means that 68 g of nitric acid is dissolved in 100 g of ...

• Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution

## 6. Concentrated nitric acid used in the laboratory work is 68 ... - Vedantu

• Complete step by step answer: The percentage of nitric acid used for laboratory purposes is 68%. Hence, in 100 g of dilute nitric acid, 68 g is nitric acid and ...

• Concentrated nitric acid used in the laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is\$1.504\\text{g m}{{\\text{L}}^{-1}}\$?. Ans: Hint:This q...

## 7. Concentrated nitric acid used in laboratory work is 68 ... - Careers360

• 68\% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504\; g\; mL^{-1}\; ?

• 2.4    Concentrated nitric acid used in laboratory work is nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is

## 8. Concentrated nitric acid used in laboratory work is 68% nitric acid by ...

• Feb 29, 2020 · 68% of nitric acid by mass means that Mass of nitric acid = 68g · Mass of solution = 100g · Molar mass of HNO3 = 63g mol-1? · ∴ 68 g HNO3 = mole = ...

• Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be ... of the solution is 1.504 g mL-1?

## FAQs

### Is concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution? ›

Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in an aqueous solution. This means that 68 g of nitric acid is dissolved in 100 g of the solution.

What is the molarity of concentrated nitric acid which is 68% by mass in aqueous solution? ›

Therefore molarity of nitric acid = (1.08/66.49) x 1000 = 16.24 M.

What mass of a concentrated solution of nitric acid 68.0% HNO3 by mass is needed to prepare 400.0 g of a 10.0% solution of HNO3 by mass? ›

Answer: The required amount of concentrated nitric acid solution is 58.82 g.

What is the molar mass of 68% nitric acid? ›

The molar mass of nitric acid is 63 g/mol. It is given that the nitric acid used in the laboratory is 68% by mass in aqueous solution. 100 g of solution contains 68 g of nitric acid or 6368=1.079 moles of nitric acid. Density of solution is 1.504 g/mL.

Top Articles
Latest Posts
Article information

Author: Fr. Dewey Fisher

Last Updated: 19/06/2023

Views: 5654

Rating: 4.1 / 5 (62 voted)

Author information

Name: Fr. Dewey Fisher

Birthday: 1993-03-26

Address: 917 Hyun Views, Rogahnmouth, KY 91013-8827

Phone: +5938540192553