In the reaction, $4N{H}_3+5O_2⟶4NO+6H_{2}O4NH\_3+\; 5O\_2\backslash longrightarrow4NO\; +\; 6H\_2O$, when one mole of ammonia and one mole of oxygen are made to react to completion, then

5 mL of 0.1M $Pb(N{O}_3{)}_{2}Pb(NO\_3)\_2$ is mixed with 10 mL of 0.02M KI. The amount of $Pb{l}_{2}Pbl\_2$ precipitated with be about

The mass of AgCl precipitated when 4.68g of NaCl is added to a solution containing 6.8 g of $AgN{O}_{3}AgNO\_3$ is

Twenty milliliter of a solution is 0.1 M in each of $N{a}_{2}C{O}_{3}Na\_2CO\_3$ and $NaHC{O}_{3}NaHCO\_3$. It is titrated against 0.1M HCI using phenolphthalein as the indicator. The volume of HCl used at the endpoint will be

An aqueous solution of 6.3g oxalic acid dihydrate is made up to 250 mL. The volume of 0.1N NaOH required to completely neutralize 10 mL of this solution is

In the standardization of $N{a}_2{S}_2{O}_{3}Na\_2S\_2O\_3$ using $K_{2}C{r}_2{O}_{7}K\_2Cr\_2O\_7$ by iodometry, the equivalent mass of $K_{2}C{r}_2{O}_{7}K\_2Cr\_2O\_7$ is

No. of oxalic acid molecules in 100 mL of 0.02N oxalic acid are :

30 mL of an acid is neutralized by 15 mL of 0.2N alkali. The strength of the acid is

To neutralize 100 mL 0.1M $H_{2}S{O}_{4}H\_2SO\_4$, the mass of NaOH required is :

0.16g of a dibasic acid required 25 mL of decinormal NaOH solution for complete neutralization. The molecular weight of the acid will be: