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Home  >>  JEEMAIN and AIPMT  >>  Chemistry  >>  Solutions
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What is the normality of 0.20M $H_3PO_4$ (a tribasic acid)in the following reaction?$H_3PO_4+2OH^-\rightarrow HPO_4^{2-}+2H_2O$

$\begin{array}{1 1}(a)\;0.30N\\(b)\;0.40N\\(c)\;0.90N\\(d)\;0.15N\end{array}$

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Answer: 0.4 N
Normality = Basicity $\times$ Molarity
Normality is given as 0.2M and Basicity can be inferred to be 2, hence the Normality $= 2 \times 0.2 = 0.4\;N$
answered Feb 13, 2014 by sreemathi.v
edited Jul 17, 2014 by balaji.thirumalai
 

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