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[" (4) may increase or decrease the form...

[" (4) may increase or decrease the formate ion present in "0.100" M formic acid (HCOOH) solutional "],[" (Ke - "1.7times10^(-4))" ."],[[" (K) "4.7times10^(-4)" ."," (2) "3.1times10^(-3)M," (3) "2.1times10^(-3)M," (4) "5.1times10^(3)H]]

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Calculate the concentration of the formate ion present in 0.100 M formic acid (HCOOH) solution at equilibrium (K_(a) = 1.7xx10^(-4)) .

Calculate the concentration of the formate ion present in 0.100 M formic acid (HCOOH) solution at equilibrium (K_(a) = 1.7xx10^(-4)) .

Calculate the H^(+) ion concentration in 0.05M formic acid at 298K. (K_(a)=1.8xx10^(-4) for HCOOH).

What is the pH of a 0.15 M solution of formic acid, HCOOH ? {:("Formic Acid",K_a),(HCOOH,1.9xx10^(-4)):}

Calculate the degree of ionisation and concentration of H_(3)O^(+) ions in a solution of 0.01 M formic acid (K_(a)= 2.1 xx 10^(-4))

Calculate the degree of dissociation and concentration of H_3O^+ ion in 0.01 M solution of formic acid K_a = 2.1 xx 10^(-4) at 298K.

A mixture of weak acid is 0.1M in HCOOH (K_(a) = 1.8 xx 10^(-4)) and 0.1M in HOCN (K_(a) = 3.1 xx 10^(-4)) . Hence, [H_(3)O^(o+)] is

A mixture of weak acid is 0.1M in HCOOH (K_(a) = 1.8 xx 10^(-4)) and 0.1M in HOCN (K_(a) = 3.1 xx 10^(-4)) . Hence, [H_(3)O^(o+)] is

Calculate the degree of dissociation and concentration of H_(3)O^(+) ions in 0.01 M solution of formic acid (K_(c) =2.1 xx 10^(-4) " at " 298 K)