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What is the volume of 80 percent H2SO4?

Density of 80\% sulphuric acid would be 1.8 g/ml not 1.8g/mol. First you have to calculate the molarity of 80\% acid solution which will act as stock solution. In next step you require 0.2 M acid solution from 14.68M stock solution. 13.62 ml of 80 \% sulphuric acid is required.

What is the molarity of solutions of H2SO4 which has a density of 1.84 g ml at 25oc and contains 98\% by weight?

What is the molarity of H2SO4 solution that has a density of 1.84g/cc at 350C and contains 98\% by weight? A . 4.18M.

What is the molar mass of h2so4?

98.079 g/mol
Sulfuric acid/Molar mass

What is molarity of pure water if its density is 1000 kg m3?

Thus, the molarity of the water is 55.56 M.

What is the volume of 95 h2so4?

Hence, the volume of 95\% sulphuric acid and mass of water needed to prepare 15\% sulphuric acid solution is $9.4\,c{{m}^{3}}$ and 93.5 g respectively. Note: From the volume of 95\% sulphuric acid that is $9.4\,c{{m}^{3}}$ we can get volume of water as 100 – 9.4 = $90.6\,c{{m}^{3}}$.

How do you make 98 sulfuric acid?

If 49.0g of 100\%pure acid is present in 1.0 L,it is 1N.So, 0.1N, means 4.90g acid per L. Usually acid availability is 98\% , density 1.84g/ML.So , volume of acid sample needed will be: 1.0L solution weighs =1840g which contains 1840×98/100g acid.

How do you find the molarity of 98 H2SO4?

Molarity = No. of moles of solute/Volume of the solutions in liter. = 17.98 M. Hence, the molarity of the solution is 17.98 M.

How do you find the density of H2SO4?

1.83 g/cm³
Sulfuric acid/Density

What is the molarity of 1800g of pure H2SO4 in 1L of solvent?

Therefore, you obtain 1800 g of pure H2SO4 in 1 litre of solvent. But our actual solution is 80\% (w/w) H2SO4. Hence, we need to take 80\% of the 1800 g for our further calculations. And since we have assumed volume of solvent to be 1L, so molarity would just be equal to number of moles. 8 clever moves when you have $1,000 in the bank.

What is the density of a solution of H2SO4?

1answer Conc. H2SO4 has a density 1.9g/ml and is .99\% H2SO4 by weight. Find molarity of solution. askedMay 26, 2019in Chemistryby Bhawna(68.5kpoints)

What is the density of 80\% sulphuric acid in grams?

There is a little correction in the question. Density of 80\% sulphuric acid would be 1.8 g/ml not 1.8g/mol. First you have to calculate the molarity of 80\% acid solution which will act as stock solution. Now you have molarity of your stock solution 14.68M

How much 80\% sulphuric acid is required to make stock solution?

First you have to calculate the molarity of 80\% acid solution which will act as stock solution. In next step you require 0.2 M acid solution from 14.68M stock solution. 13.62 ml of 80 \% sulphuric acid is required. I would just clarify upon the already existing correct answer by Chaitnaya Kumar so as to make it more clear to wider audience.