0.1 mol of `NH_3` and 0.1 mol of `NH_4Cl` are dissolved in 1L of a buffer. What change in pH will be observed if-(a) 0.02 mol HCl gas, (b) 0.02 mol NaOH is dissolved in the solution?

What will be the pH if 0.01 mol of HCI is dissolved in the above buffer solution? Find the change in pH value.

Will the elevation in boiling point be same if 0.1 mol of Sodium chloride or 0.1 mol of sugar is dissolved in 1L of water ? Explain.

A buffer solution contains 0.02 moles of NH_4OH and 0.03 moles of NH_4CI dissolved in 1 litre of the solution. Calculate the pH of the solution. Dissociation constant of NH_4OH "is" 1.8 xx 10^-5

To 1.0L solution containing 0.1mol each of NH_(3) and NH_(4)C1,0.05mol NaOH is added. The change in pH will be (pK_(a) for CH_(3)COOH = 4.74)

To 1.0L solution containing 0.1mol each of NH_(3) and NH_(4)C1,0.05mol NaOH is added. The change in pH will be (pK_(a) for CH_(3)COOH = 4.74)

Calculate the Van't Hoff factor when 0.1 mol NH_(4)Cl is dissolved in 1 L of water. The degree of dissociation of NH_(4)Cl is 0.8 and its degree of hydrolysis is 0.1 .

Calculate the Van't Hoff factor when 0.1 mol NH_(4)Cl is dissolved in 1 L of water. The degree of dissociation of NH_(4)Cl is 0.8 and its degree of hydrolysis is 0.1 .

Calculate the Van't Hoff factor when 0.1 mol NH_(4)Cl is dissolved in 1 L of water. The degree of dissociation of NH_(4)Cl is 0.8 and its degree of hydrolysis is 0.1 .