A `0.10` M solution of HF is `8.0%` dissocaited What is the `K_(a)`?

A 0.10 M solution of weak acid is 5.75% ionized. What is the K_a value for this acid ?

A 0.050 M solution of an unknown acid is 1.0 % ionized . What is the value of its K_b ?

The pH of 0.02M solution of HF is 2.62. Calculate K_4 of HF. What is the pH of 0.0002M HF solution ?

Calculate the pH of 0.10 M solution of NH_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8 X 10^(-5)

Calculate the pH of 0.10 M solution of Nh_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8xx10^(-5)

0.01 M monoprotonic acid is 10% ionised, what is K_(a) of the solution ?

0.01 M monoprotonic acid is 10% ionised, what is K_(a) of the solution ?

Depression in freezing point of 0.1 molal solution of HF is -0.201^(@)C . Calculate percentage degree of dissociation of HF. (K_(f)=1.86 K kg mol^(-1)) .