`2.5mL` of `(2)/(5)` weak monoacidic base (`K_(b)= 1xx10^(-12)` at `25^(@)C`) is tittrated with `(2)/(15)MHCI` in water at `25^(@)C`. The concentration of `H^(+)` at equivalence point is: `(K_(w)= 1xx10^(-14)at 25^(@)C)`

When 2.5 mL of 2//5M weak monoacidic base (K_(b) = 1 xx 10^(-12) at 25^(@)C) is titrated with 2//15 M HCI in water at 25^(@)C the concentration of H^(o+) at equivalence point is (K_(w) = 1 xx 10^(-14) at 25^(@)C)

2.5mL of 2//5M weak mono-acidic base (K_(b) = 1 xx 10^(-12) at 25^(@)C) is titrated with 2//15M HCI in water at 25^(@)C . Find the concentration of H^(o+) ions at equivalence point. (K_(w) = 1 xx 10^(-14)at 25^(@)C) a. 3.7 xx 10^(-13)M b. 3.2 xx 10^(-7)M c. 3.2 xx 10^(-2)M d. 2.7 xx 10^(-2)M

2.5 mL of (2)/(5)M weak monoacidic base (K_(b)=1xx10^(-12) at 25^(@)C) is titrated with (2)/(15) M HCl in water at 25^(@)C . Calculate the concentration of H^(+) at equilibrium point. (k_(w)=1xx10^(-14))

2.5 ml 0.4 (M) weak monoacidic base ( k_b=1 xx 10^(-12) at 25^@ C ) is titrated with 2/15(M) HCl in water at 25^@C . The concentration of H^+ at equivalence point is ( K_w=1xx10^(-14) , at 25^@C )