There are 0.54 moles of hydrogen atoms in 0.09 moles of H2SO4. This is because each molecule of H2SO4 contains 2 hydrogen atoms. By multiplying the number of moles of H2SO4 by the number of hydrogen atoms per molecule, you can calculate the total moles of hydrogen atoms present.
A mole of sulfuric acid (H2SO4) contains one mole of sulfur (S), two moles of hydrogen (H), and four moles of oxygen (O).
When H2SO4 dissociates in water, it forms two steps of dissociation. First, it breaks into H+ and HSO4-. Then, HSO4- further dissociates into H+ and SO4^2-. This results in the formation of 2 moles of H+ ions and 1 mole of SO4^2- ion for every mole of H2SO4 dissociated.
The molar mass of H2SO4 is approximately 98.08 g/mol. Therefore, three moles of H2SO4 would have a mass of approximately 294.24 grams.
To calculate the mass of H2SO4 required, first calculate the number of moles needed using the formula: moles = molarity x volume (in liters). Then, multiply the moles by the molar mass of H2SO4 (98.08 g/mol) to find the mass. moles = 0.15 mol/L x 0.75 L = 0.1125 mol mass = 0.1125 mol x 98.08 g/mol ≈ 11.04 g of H2SO4.
There are 0.54 moles of hydrogen atoms in 0.09 moles of H2SO4. This is because each molecule of H2SO4 contains 2 hydrogen atoms. By multiplying the number of moles of H2SO4 by the number of hydrogen atoms per molecule, you can calculate the total moles of hydrogen atoms present.
A mole of sulfuric acid (H2SO4) contains one mole of sulfur (S), two moles of hydrogen (H), and four moles of oxygen (O).
When H2SO4 dissociates in water, it forms two steps of dissociation. First, it breaks into H+ and HSO4-. Then, HSO4- further dissociates into H+ and SO4^2-. This results in the formation of 2 moles of H+ ions and 1 mole of SO4^2- ion for every mole of H2SO4 dissociated.
The molar mass of H2SO4 is approximately 98.08 g/mol. Therefore, three moles of H2SO4 would have a mass of approximately 294.24 grams.
To calculate the mass of H2SO4 required, first calculate the number of moles needed using the formula: moles = molarity x volume (in liters). Then, multiply the moles by the molar mass of H2SO4 (98.08 g/mol) to find the mass. moles = 0.15 mol/L x 0.75 L = 0.1125 mol mass = 0.1125 mol x 98.08 g/mol ≈ 11.04 g of H2SO4.
The answer is 10 moles.
Since H2SO4 is a diprotic acid, it will require twice the amount of NaOH to neutralize it. Therefore, molarity of NaOH should also be 1 M. 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, to neutralize 1 mole of H2SO4, 2 moles of NaOH are required. To neutralize 1 mole of H2SO4 in 100 ml (0.1 L) of 1 M solution, you will need 0.1 moles of NaOH.
There are 6.3 moles of H atoms in 2.1 moles of H3PO4. This is because there are three moles of H atoms in one mole of H3PO4.
4.75 moles H2SO4 (2 mole H/1 mole H2SO4)(6.022 X 1023/1 mole H)(1 mole H atoms/6.022 X 1023) = 9.67 moles of hydrogen atoms ------------------------------------------ As you can see this set up is formal as the two last steps are superfluous when Avogadro's number actually apears over itself as a form of 1.
To completely neutralize 100ml of 1M H2SO4, you would need an equal number of moles of NaCl. H2SO4 is a diprotic acid, so it will require 2 moles of NaCl to neutralize 1 mole of H2SO4. Therefore, you would need 2 moles of NaCl for every mole of H2SO4. With a 1M solution of H2SO4 in 100ml, you have 0.1 moles of H2SO4. Therefore, you would need 0.2 moles of NaCl. The molar mass of NaCl is approximately 58.44g/mol, so you would need approximately 11.7 grams of NaCl to completely neutralize the 1M H2SO4 solution.
One gram-molecular weight of any substance contains Avogadro's number of molecules. For H2SO4, the gram-molecular weight is 98 g (2 for H, 32 for S, and 4 for O), so 1 gram of H2SO4 contains 1/98 moles of H2SO4 molecules, which is approximately 6.02 x 10^23 molecules.
The oxidation number of hydrogen (H) in H2SO4 is +1.