200mL of 0.2M HCl is mixed with 300 m L of 0.1M NaOH. The molar heat of neutralization of this reaction is `-57.1kJ`. The increase in temperature in `.^(@)C` of the system on mixing is `x xx 10^(-2)`. The value of x is __________. (Nearest integer)
[Given : Specific heat of water `=4.18Jg^(-1)K^(-1)` Density of water `=1.00gcm^(-3)`]
(Assume no volume change on mixing)

400 ml of 0.2 M-HCl is mixed with 600 ml of 0.1 M-NaOH solution. The maximum mass of NaCl fromed is :

60ml of 0.1M HCl is mixed with 40ml of 0.05M H_(2)SO_(4) .The "pH" value of the resulting solution is

20mL of 0.5 M HCl and 35 mL of 0.1 N NaOH are mixed. The resulting solution will

50 mL of 0.1 M HCl and 50 mL of 2.0 M NaOH are mixed. The pH of the resulting solution is

The pH of a solution obtained by mixing 50 mL of 1 M HCl and 30 mL of 1M NaOH is x xx 10^(-4) . The value of x is ________. (Nearest inetger) [log 2.5 = 0.3979]

75 mL of 0.2 M HCl is mixed with 25 mL of 1 M HCl . To this solution 300 mL of distilled water is added. What is the pH of the resultant solution ?

When 400 mL of 0.2 M H _(2) SO _(4) soltution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is _______ xx 10 ^(-2) K. (Round off to the nearest integer). [Use : H ^(+) (aq) + OH ^(-) (aq) to mol ^(-1) ] Delta H =- 57.1 kJ mol ^(-1)] Specific heat of H _(2) O = 4. 18 J K ^(-1) g ^(-1) density of H _(2) O = 1. 0 g cm ^(-3) Assume no change in volume of solutio on mixing.