What is the pH of a mixture that contains 0.60 M # HCl# and 0.30 M #HNO_2#?

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Answer 1 · 2017-02-22T17:59:31

pH of 0.6M HCl = -2.94
pH of 0.3M HNO2(very weak acid) = 1.96019

The #"Ka"# of HCl is #1.3 xx 10^6#

#sqrt(Ka xx"moles") = p#

      #"pH" = -logp#

#"pH of HCl"#

#= sqrt( 1.3 xx 10^6 xx 0.6)#

# sqrt780000#

= #883.176086633#

#"pH of HCl" = -log883.176086633#

#"pH of HCl" = -2.94604730135#

Which means its very acidic

The #"Ka"# of #HNO_2# is #0.00040#

#= sqrt( 0.00040 xx 0.3)#

= 0.01096

#"pH of" ##HNO_2 = -log0.01096#

#"pH of" ##HNO_2 = 1.96019#