`0.1` mole `HCl` is dissolved in distilled water of volume `V`.Then at `underset(Vrarroo)lim,(pH)_("solution")` is equal to......

underset(xrarr0)(lim)(sinnx)/x is equal to

If ammonia is dissolved in water, pH of the solution

40 mg of pure NaOH is dissolved in 10 litres of distilled water. The pH of the solution is

1 mole of glucose is dissolved in 4 moles of water to form a solution. Find mole-fraction of solute in solution (x_("solute")) ?

when 0.1 mole of ammonia is dissolved in sufficient water to make 1 litre of solution. The solution is found to have a hydroxide ion concentration of 1.34 xx 10^(-3) . The dissociation constant of ammonia is

When 0.1 mole of NH_(3) is dissolved in water to make 1.0 L of solution, the [OH^(-)] of solution is 1.30xx10^(-3)M. Calculate K_(b) for NH_(3).

When 0.1 mole of NH_(3) is dissolved in water to make 1.0 L of solution , the [OH^(-)] of solution is 1.34 xx 10^(-3) M. Calculate K_(b) for NH_(3) .

0.115 gm of sodium metal was dissolved in 500 ml of the solution in distilled water. Calculate the molarity of the solution ?

1 ml of 0.1 M HCl is added into 99 ml of water . Assume volumes are additive, what is pH of resulting solution .

0.05 mole of NaOH is added to 5 liters of water What will be the pH of the solution ?