The mass of sulfuric acid is 490,395 grams.
The concentration of a solution is moles/volume. 2.943g of pure sulphuric acid H2S4 is approximately 15 moles, and 15/150 cm3 is 10.
I think you meant " How many moles of acetic acid in 25 grams of acetic acid? " We will use the chemist formula for acetic acid, 25 grams C2H4O2 (1 mole C2H4O2/60.052 grams) = 0.42 mole acetic acid =================
1 mole sulfuric acid for 1 mole calcium chloride
2 moles H2SO4 (98.086 grams/1 mole H2SO4)= 196.172 grams of sulfuric acid====================
Molarity = moles of solute/Liters of solution ( get moles of HNO3 and 300 ml = 0.300 Liters ) 0.31 grams Nitric acid (1 mole HNO3/63.018 grams) = 0.004919 moles HNO3 Molarity = 0.004919 moles HNO3/0.300 Liters = 0.0164 M HNO3
1. Add 80mls of distilled water in a beaker. 2. Now add 20mls of concentrated sulphuric acid in small quantities while stirring with a glass rod.
a ml of 36n or 18m sulphuric acid should weigh approx 1.84g. This is because conc sulphuric acid's density is 1.84g/ml
sulphuric acid is a diprotic acid so has two H+ and needs two moles of sulphuric acid to neutralise it
Cu + 2H2SO4 -> CuSO4 + 2H2O + SO2 Copper (Cu) on reacting with two moles of sulphuric acid (H2SO4) yields copper sulphate (CuSO4) and 2 moles of water (2H2O) and sulphur dioxide (SO2).
The molar mass of sulfuric acid is 98 grams per mole.
The concentration of a solution is moles/volume. 2.943g of pure sulphuric acid H2S4 is approximately 15 moles, and 15/150 cm3 is 10.
0.1538 grams
4 moles HNO3 (63.018 grams/1 mole HNO3) = 252 grams nitric acid ================
I think you meant " How many moles of acetic acid in 25 grams of acetic acid? " We will use the chemist formula for acetic acid, 25 grams C2H4O2 (1 mole C2H4O2/60.052 grams) = 0.42 mole acetic acid =================
3.33%
The mol mass of sulfuric acid is 98.078 g/mol, 98 g of sulfuric acid therefore contains 0.9992 moles. Using consistent significant figures and your calculations, 98 g sulfuric acid would be equal to 1.0 mol sulfuric acid.
The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 300 g of ammonia requires 300 g ÷ 34 g/mol ≈ 8.8 moles of sulphuric acid Therefore there will be 36.0 - 8.8 = 27.2 moles of sulphuric acid left.