1 mol of `C_(6)H_(6)` , 0.1 mol of `HNO_(3)` and `0.05` mol of `H_(2)SO_(4)` are mixed and water is added to the mixture . pH of the solution , if the final volume is 1 L , is

5 mL of N-HCl , 20 mL of N//2 H_(2)SO_(4) and 30 mL of N//3 HNO_(3) are mixed together and the volume is made to 1 L . The normality of the resulting solution is

An equilibrium mixture CO(g)+H_(2)O(g) hArr CO_(2)(g)+H_(2)(g) present in a vessel of one litre capacity at 815^(@)C was found by analysis to contain 0.4 mol of CO, 0.3 mol of H_(2)O, 0.2 mol of CO_(2) and 0.6 mol of H_(2) . a. Calculate K_(c) b. If it is derived to increase the concentration of CO to 0.6 mol by adding CO_(2) to the vessel, how many moles must be addes into equilibrium mixture at constant temperature in order to get this change?

0.1M HCl and 0.1 MH_(2)SO_(4) , each of volume 2 ml are mixed and the volume is made up to 6 ml by adding 2 ml of 0.01 N NaCl solution. The pH of the resulting mixture is

100 mL of 0.1 M HCl + 100 mL of 0.2 M H_(2)SO_(4) + 100 mL of 0.1 M HNO_(3) are mixed togther. a. What is the final conecntration of the solution. b. What would be the final concentration of the solution. If the solution is made to 1 L by adding H_(2) O ? c. What would be the final concentration of the solution if 700 mL of H_(2)O is added to the solution?

A mixture of 0.1 mol of Na_(2)O and 0.1 mol of BaO is dissolved in 1000 g of H_(2)O . Calculate the vapour pressure of solution at 373 K .

1 mol of N_(2) and 2 mol of H_(2) are allowed to react in a 1 dm^(3) vessel. At equilibrium, 0.8 mol of NH_(3) is formed. The concentration of H_(2) in the vessel is

The reaction, CO(g)+3H_(2)(g) hArr CH_(4)(g)+H_(2)O(g) is at equilibrium at 1300 K in a 1 L flask. It also contains 0.30 mol of CO, 0.10 mol of H_(2) and 0.02 mol of H_(2)O and an unknown amount of CH_(4) in the flask. Determine the concentration of CH_(4) in the mixture. The equilibrium constant K_(c ) for the reaction at the given temperature us 3.90 .

0.1mol of RNH_(2)(K_(b) = 5 xx 10^(-4)) is mixed with 0.08mol of HC1 and diluted to 1L . Calculate the [H^(o+)] in the solution.

45 g of ethylene glycol (C_(2) H_(6)O_(2)) is mixed with 600 g of water. The freezing point of the solution is (K_(f) for water is 1.86 K kg mol^(-1) )

At 700 K, CO_(2) and H_(2) react to form CO and H_(2)O . For this purpose, K_(c ) is 0.11 . If a mixture of 0.45 mol of CO_(2) and 0.45 mol of H_(2) is heated to 700 K . (a) Find out amount of each gas at equilibrium. (b) When equilibrium has been reached, another 0.34 mol of CO_(2) and 0.34 mol of H_(2) are added to the reaction mixture. Find the composition of of mixture at new equilibrium.