Molarity = mols/L and mols = g/molar mass so
mols = 4.9/98 = 0.05. You have 0.05 mols/L - 0.05 M.
N = 2 x M = 0.05 x 2 = ?
You have to prepare a pH 3.50 buffer, and you have the following 0.10M solutions available HCOOH, CH3COOH, H3PO4,CHOONa, CH3COONa, and NaH2PO4. a) What solutions would you use? b) How many milliliters of each solution would you use to make approximately 1
A solution of sodium bicarbonate is prepared by adding 45.00g of sodium bicarbonate to a 1.00-L volumetric flask and adding distilled water until it reaches the 1.00-L mark. Calculate the concentration of sodium in units of: a) milligrams per liter b)
What volume of 6.0m H2SO4 is needed to prepare 0.5L of a 0.3M H2SO4 solution?
Calculate the volume of concentrated reagent required to prepare the diluted solutions indicated: (a) 18 M H2SO4 to prepare 225 mL of 2.0 M H2SO4 (
h2so4 is labelled as 9.8 by weight. specific gravity of h2so4 is 1.8. the volume of acid to be taken to prepare 100 ml of 0.18M solution is?
A 10.0mL sample of H2SO4 was neutralized by 13.5mL of 1.0M KOH. What was its molarity of H2SO4? What is the normality?
a 20% solution of H2SO4 has a density of 1.14 g/mL. calculate the molarity, normality and molality of the solution.
How many milliliters of 5M H2SO4 are required to make a 1500ml of a .002M H2SO4 solution. I used the formula M*L=M * L so mL *5 = 1500 * .002 I got .6mL is this right?
prepare 1M 100 ml H2SO4. 98% H2SO4, density 1.84
a piece of Aluminium weighing 2.7g is titrated with 75 mL of H2SO4(specific gravity 1.18 and 24.7% H2SO4 by weight). after the metal is completely dissolved the solution is diluted to 400 mL . calculate the molarity of free H2SO4 in the solution.
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