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A 3.0 L solution contains 73.5 g of H2SO4 Calculate the molar concentration of the solution?
Wiki User
∙ 15y ago
A)1. H2SO4 is the solute
2. Water is the solvent
3. Molarity = moles of solute / liter of solution = n / V
(Note the case of the letters is important in science. N stands for Normal in chemistry a type of concentration, n stands for number of moles)
Rearrange the formula to find n
n = M x V
Here are the known values,
M = 3.5M
n = x mol
V = 1.00L
Plug it in and solve for n (the number of moles of H2SO4 in the solution)
n = 3.5M x 1.00 L = 3.50 mol of H2SO4
Molecular mass of H2SO4 is 1g/mole H x 2 + 32.1g/mol S + 16g/mol O x 4 = 98.1g/mol H2SO4
mass = number of mole x relative molecular mass
mass = n x 98.1g/mol
mass = 98.1g/mol H2SO4 x 3.50mol H2SO4
= 343g H2SO4 <-answer
Wiki User
∙ 13y ago
Wiki User
∙ 15y ago0.25 M I had this question also, but I don't remember how I found the answer.
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What is the difference between 6 M H2SO4 and 0.1 M H2SO4?
The first solution is more concentrated because it contains 6 moles of H2SO4 per one liter of solution. The second solution is less concentrated because it contains 0.1 moles of H2SO4 in one liter. In equal amounts of each example, the first would have more H2SO4.
What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
Assuming pH on just simple concentration. - log(0.01 M H2SO4) = 2 pH =====
How do you make 80N H2SO4 solution from 98 percent acid?
You'll never reach that because 98% H2SO4 is of lower normality: max. 37 N Density 1840 g solution / L solution Molar mass 98 g/mol H2SO4 concentration 980 gH2SO4 / 1000g solution H2SO4 2 equivalent H+/mol H2SO4 All together making: [1840*(980/1000) / 98 ] * 2 = 36.8N H2SO4 Or the other way 'round: 80N = 40M = 40*98(g/mol) = 3920 gH2SO4/L = 3920/(98*100) = 4000 g (solution)/L , which is more than the most concentrated H2SO4 solution can weight
How will you make solution for ph4 of 0.005 normal h2so4?
how will make solution for 0.005 h2so4
Which is more acidic in HCl HNO3 H2SO4 and why?
H2SO4 is more acidic if you have equal molar quantities and the same volume for each (ie. Concentration) as it's diprotic . so for example a solution containing 1moldm-3 of H2SO4 has a [H+]of 2moldm-3 whereas HCL and HNO3 have will have a [H+] of 1moldm-3. [H+] is the concentration of hydrogen ions in a solution and [h+] is a measure of acidity as [H+]=10-ph or rearranged Ph=-log[H+]
What is the difference between 6 M H2SO4 and 0.1 M H2SO4?
The first solution is more concentrated because it contains 6 moles of H2SO4 per one liter of solution. The second solution is less concentrated because it contains 0.1 moles of H2SO4 in one liter. In equal amounts of each example, the first would have more H2SO4.
Which substance increase h ion concentration in a solution?
acids such as HCl, H2SO4 HNO3 etc
What is the pH obtained on dissolving 0.01M of H2SO4 in 2 liters of solution?
Assuming pH on just simple concentration. - log(0.01 M H2SO4) = 2 pH =====
How do you make 80N H2SO4 solution from 98 percent acid?
You'll never reach that because 98% H2SO4 is of lower normality: max. 37 N Density 1840 g solution / L solution Molar mass 98 g/mol H2SO4 concentration 980 gH2SO4 / 1000g solution H2SO4 2 equivalent H+/mol H2SO4 All together making: [1840*(980/1000) / 98 ] * 2 = 36.8N H2SO4 Or the other way 'round: 80N = 40M = 40*98(g/mol) = 3920 gH2SO4/L = 3920/(98*100) = 4000 g (solution)/L , which is more than the most concentrated H2SO4 solution can weight
How will you make solution for ph4 of 0.005 normal h2so4?
how will make solution for 0.005 h2so4
Which is more acidic in HCl HNO3 H2SO4 and why?
H2SO4 is more acidic if you have equal molar quantities and the same volume for each (ie. Concentration) as it's diprotic . so for example a solution containing 1moldm-3 of H2SO4 has a [H+]of 2moldm-3 whereas HCL and HNO3 have will have a [H+] of 1moldm-3. [H+] is the concentration of hydrogen ions in a solution and [h+] is a measure of acidity as [H+]=10-ph or rearranged Ph=-log[H+]
How much more acid is a solution of pH 2 than one of pH 5?
Only if it is the same acid. ie. You can have 1.0moldm^-3 H2SO4 (sulfuric acid, in car batteries) and 1.0moldm^-3 HCO3 (carbonic acid, in natural acid rain). Even though they are the same concentration, the sulfuric acid is much stronger.
What solutions has a concentration of one molar?
Molal is the number of mols of solute per kilo of solvent. Molar is the number of mols of solute per litre of solution. If you think those through, you should see that which is greater depends on the density of the solvent.
What is the molality of a solution that contains 60.0g H2SO4 in 7.00g of water?
7 g water doesn't contain 60 g sulfuric acid.
What does sulphuric acid contains?
sulphur and hydrogen the molecular formula is H2SO4
Which substances increase the H concentration in a solution?
H plus ion concentration can be decreased by adding base to the solution. The reduction can also be done by accepting hydrogen ions.
A 25.00ml sample of h2so4 requires 22.65 ml of the 0.550m naoh for its titration what was the concentration of sulfuric acid?
(25.00ml H2SO4)(H2SO4 M) = (22.65ml NaOH)(0.550M) = 0.4983M H2SO4
