If 20 mL of 0.1 M NaOH is added to 30 mL of 0.2 M CH_(3)COOH (pK_(a)=4.74), the pH of the resulting solution is :
Calculate pH of a buffer solution that contains 0.1M NH_(4)OH(K_(b)=10^(-5)) and 0.1 M NH_(4)Cl.
What is the pH of 0.1M NaOH solution?
one litre of an aqueous solution contains 0.15 mole of CH_(3)COOH(pK_(a) =4.8)) and 0.15 mole of CH_(3) COONa. After the addition of 0.05 mole of solid NaOH to this solution, the pH will be :
What is the pH of 0.0001 M HCl solution?
What is [NH_(4)^(+)] in a solution that contain 0.02 M NH_(3)(K_(b)=1.8xx10^(-5)) and 0.01 M KOH?
At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :
10mL of 0.1 M HCl solution reacts completely with 10 mL of 0.1 M NaOH solution. What will be the pH of the resulting solution?
The compound whose 0.1 M solution is acidic :
We have three aqueous solutions of NaCl labelled as 'A', 'B' and 'C' with concentrations 0.1M, 0.01 and 0.001M, respectively. The Value of Van't Hoff factor for these solutions will be in the oder
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
