Consider the following chemical equation; properly balanced: 2NaOH + H 2 SO 4 è

Question

Consider the following chemical equation; properly balanced:

2NaOH + H2SO4 è Na2SO4 + 2H2O

If we were to use a solution of 1 M NaOH to run this reaction, what molar solution of H2SO4 would be needed to provide sufficient acid for the reaction to occur to completion?

12) For the same reaction, if we were to measure concentration using normality rather than molarity, for one liter of 1 N NaOH, what Normal concentration of H2SO4 would be required for the reaction to occur to completion?

13) A 1.0 N solution of H3PO4 is equivalent to what if measured in Molarity; ie., what M solution?

Explanation / Answer

12. Since 2 moles of NaOH react with 1 mole of H2SO4

So, required molar solution of H2SO4 = 1/2 = 0.5 M

13. Normality of H2SO4= molarity × 2 = 0.5 × 2 = 1 N

14. N/M = n

For H3PO4, n = 3 since, it is tribasic

M = 1/3

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