The `P^(H)` of 0.01M solution of acetic acid is 5.0 What are the values of `[H^(+)]` and `Ka` respectively?

The p^(H) of 0.1 M NaCI solution is

pH of a 0.1M HCN solution is 5.2. What is the value of Ka for the acid?

The compound whose 0.1 M solution is acidic :

Calculate the pH at the equivalence point when a solution of 0.1 M acetic acid is titrated with a solution of 0.1 M NaOH. K_(a) for acid =1.9xx10^(-5) .

The addition of NH_(4)Cl to 0.1 M acetic acid will cause

Find the pH at equivalence points when a soluiton of 0.1M acetic acid is titrated with a solution of 0.3M NaOH K_(a) for acetic acid =7.5xx10^(-6)

When 0.2M solution of acetic acid is neutralised with 0.2M NaOH in 500 mL of water, the pH of the resulting solution will be: [pK_(a) of acetic acid = 4.74]

The P^(H) of a weak mono basic acid is 5. The degree of ionisation of acid in 0.1 M solution is

The dessociation cosntants of acetic acid and propionic acid are 1.0 xx 10^(-5) and 1.0 xx 10^(-6) respectively. The value of P^(K_(a)) (propionic acid) - P^(K_(a)) (Acetic acid) is

The hydrogen ion concentration of 0.1 M solution of acetic acid, which is 20% dissociated, is