Question

In: Chemistry

A 10.0% by mass H2SO4 (aq) solution has a density of 1.07 g/mL. How many milliliters...

A 10.0% by mass H2SO4 (aq) solution has a density of 1.07 g/mL. How many milliliters of solution contain 8.37 g of H2SO4? What is the molality of H2SO4 in solution? What mass (in grams) of H2SO4 is in 250 mL of solution?

Solutions

Expert Solution

10% H2So4 means 10g of H2SO4 present in 100g of solution

volume of solution = mass/density

                               = 100/1.07

                               = 93.46ml

10g of H2SO4 present in 93.46ml of solution

8.37g of H2So4 present in = 93.46*8.37/10    = 78.23ml of solution

mass of solvent = mass of solution - mass of solute

                            = 100-10 = 90g

molality      =   W*1000/G.M.Wt*weight of solvent in g

                   = 10*1000/98*90

                   = 1.134m >>>>>>>>answer

93.46ml of solution contains 10g of H2SO4

250ml of solution contains = 10*250/93.46    = 26.75g of H2So4


Related Solutions

How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL)...
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 1.80?
How many milliliters of a solution that is 10.25% HNO3 (w/w) with a density of 1.2792g/mL...
How many milliliters of a solution that is 10.25% HNO3 (w/w) with a density of 1.2792g/mL should be diluted in order to make 5.00L of a .250M HNO3 solution?
13. A 15.0 mL NaOH solution is required to neutralize 10.0 mL of 0.100 M H2SO4(aq)...
13. A 15.0 mL NaOH solution is required to neutralize 10.0 mL of 0.100 M H2SO4(aq) solution.         What is the concentration of NaOH solution used?   2NaOH (aq) + H2SO4(aq) → Na2SO4(aq) + 2H2O(l)
How many moles of CoCl3​ are in 172.6 ml of a 19.6 mass % solution of CoCl3​ which has a density of 1.206 g/ mL?
How many moles of CoCl3​ are in 172.6 ml of a 19.6 mass % solution of CoCl3​ which has a density of 1.206 g/ mL? __________
A 0.573 M Pb(NO3)2(aq) solution has a density of 1.17 g/mL. Calculate the % mass of...
A 0.573 M Pb(NO3)2(aq) solution has a density of 1.17 g/mL. Calculate the % mass of this solution to three significant figures. The molar mass of lead(II) nitrate is 331.2 g/mole.
The density of the plasma membrane of a cell was found to be 1.07 g/mL. If...
The density of the plasma membrane of a cell was found to be 1.07 g/mL. If the density of the lipid component is 0.91 g/mL and the density of the protein component is 1.36 g/mL, what is the percent composition (to the nearest ones) of the lipid component of the membrane, assuming the plasma membrane consists only of the lipid and protein components?
The density of the plasma membrane of a cell was found to be 1.07 g/mL. If...
The density of the plasma membrane of a cell was found to be 1.07 g/mL. If the density of the lipid component is 0.91 g/mL and the density of the protein component is 1.36 g/mL, what is the percent composition (to the nearest ones) of the lipid component of the membrane, assuming the plasma membrane consists only of the lipid and protein components?
1. how many milliliters of C3H20O4 does 3.0 moles occupy? Density is 1.2 g/mL 2. How...
1. how many milliliters of C3H20O4 does 3.0 moles occupy? Density is 1.2 g/mL 2. How many grams is 4.3 moles of C3H8O2
An aqueous solution containing 50% K2CO3 has a density of 1.5404 g/mL. a) how many grams...
An aqueous solution containing 50% K2CO3 has a density of 1.5404 g/mL. a) how many grams of K2CO3 are contained in 1 L of solution. b) Calculate the molarity (mol/L) of the K2CO3 solution c) Calculate the molarity (mol/kg) of the K2CO3 solution.
A 12.0 mass % solution of H3PO4 in water has a density of 1.104 g/mL. Calculate...
A 12.0 mass % solution of H3PO4 in water has a density of 1.104 g/mL. Calculate the pH in the solution. Ka1= 7.1 × 10−3 Ka2 = 6.3 × 10−8 Ka2 = 4.2 × 10−13
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT