A 1 M solution of H 2SO 4 will contain one mole of H 2SO 4 in 1 liter of solution, but if the solution is titrated with a base, it will be shown to contain two moles of acid. Normality refers to compounds that have multiple chemical functionalities, such as sulfuric acid, H 2SO 4. Normality can only be calculated when we deal with reactions, because Normality is a function of equivalents. There is a relationship between normality and molarity. x 10 = 15.7 M How do I calculate the Normality of an acid or base from its Molarity? The above equation can then be used to calculate the Molarity of the 70 wt % Nitric Acid:
Where: % = Weight % d = Density (or specific gravity) MW = Molecular Weight (or Formula Weight). The following equation is used for calculating Molarity where the concentration is given in wt %: The Molarity Calculator Equation (Molarity Conversion) Dividing the grams of HNO 3 by the molecular weight of HNO 3 (63.01 g/mole) gives the number of moles of HNO 3 / L or Molarity, which is 15.7 M. Knowing that the solution is 70 wt % would then allow the number of grams of HNO 3 to be calculated: (0.700)(1413g) = 989.1 grams HNO 3 per liter. Knowing the density of the acid to be 1.413 g/mL, we can calculate the weight of 1 L of 70% HNO 3 to be 1413 grams. % Nitric Acid the number of moles of HNO 3 present in 1 liter of acid needs to be calculated. Some chemists and analysts prefer to work in acid concentration units of Molarity (moles/liter).
The concentration is expressed at 70% wt./wt. Using 70% concentrated Nitric Acid as an example: 70% Nitric Acid means that 100 grams of this acid contains 70 grams of HNO 3. How is the Molarity of a percentage solution calculated?
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