The ionic product of water is 10^(-14) . What is the hydrogen ion concentration of a 0.1 M NaOH solution?
At 25^(0) C, the hydroxyl ion concentration of a basic solution is 6.75 xx 10^(-3) M.Then the value of K_(w) is
The ionic product of water is 10^(-14) , The H^(+) ion concentration in 0.1 M NaOH soluiion is
The ionization constant of a weak acid is 1.6 xx 10^(-5) and the molar conductivity at infinite dilution is 380 xx 10^(-4) sm^(2) mol^(-1) . If the cell constant is 0.01m^(-1) , then conductance of 0.01M acid solution is
The ionization constant of phenol is 1.0xx10^(-10) . What is the concentration of phenolate ion in 0.05M solution of phenol? What will be its degree of ionization if the solution is also 0.01M in sodium phenolate ?
The first ionization constant of H_(2)S is 9.1xx10^(-8) . Calculate the concentration of HS^(-) ion in its 0.1M solution. How will this concentration be affected if the solution is 0.1M in HCl also ? If the second dissociation constant of H_(2)S is 1.2xx10^(-13) , calculate the concentration of S^(2-) under both conditions.
The H ion concentration of a solution is 4.75xx10^(-5) M. Then the OH ion concentration of the same solution is
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
