what is the normality of a 3.5 M H2SO4 solution? Solution First, you have to kno

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First, you have to know how many equivalents there are in HNO3. Remember than an equivalent of acid tells you how much acid will give you 1 mole of H+ ions. If you separate HNO3 into its ions, you would get this equation: HNO3 --> H+ + NO3- This shows you that 1 mole of HNO3 can only give you 1 mole of H+ ions. Therefore, you only have 1 equiv HNO3. H2SO4, on the other hand, has two equivalents because 1 mol H2SO4 gives you 2 moles of H+ ions. To compute normality from molarity, we first have to multiply the molarity by the molar mass. 3.5 mol HNO3 / L * 63.01 g HNO3 * 1 mol HNO3 Remember too that the equivalent mass is the mass of one equivalent of acid/base. In this case, the mass of one equivalent of HNO3 is 63.01 g/equiv. We multiply by the equivalent mass to eventually get the normality. 3.5 mol HNO3 / L * 63.01 g HNO3 * 1 mol HNO3 * 1 equiv HNO3 / 63.01 g HNO3 = 3.5N Another way of expressing normality (N) is equiv/L.

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