500 ml of `0.1 M AlCl_(3)` is mixed with 500 ml of `0.1 M MgCl_(2)` solution. Then calculation the molarity of `Cl^(-)` in final solution.

500 ml of 2M NaCl solution was mixed with 200 ml of 2 M NaCl solution. Calculate the molarity of NaCl in final solution

A solution containing 200 ml 0.5 M KCl is mixed with 50 ml 19% w/v MgCl_(2) and resulting solution is dilute 8 times. Molarity of chloride ion is final solution is :

If 500 mL of 0.4 M AgNO_(3) is mixed with 500 mL of 2 M NH_(3) solution then what is the concentration of Ag(NH_(3))^(+) in solution? Given : K_(f1)[Ag(NH_(3))]^(+)=10^(3),K_(f2)[Ag(NH_(3))_(2)^(+)]=10^(4)

100 ml of 0.1 M solutio of AB (d = 1.5 gm/m) is mixed with 100ml of 0.2 M solution of CB_(2) (d = 2.5 gm/m). Calculate the molarity of B^(-) in final solution if the density of final solution is 4gm/m. Assuming AB and CB_(2) are non reacting & dissociates completely into A^(+), B^(-), C^(2+)

500 ml of 2 M CH_(3)COOH solution is mixid with 600 ml 12 % w//v CH_(3)COOH solution then calculate the final molarity of solution.

If 200ml of 0.2 M BaCl_(2) solution is mixed with 500ml of 0.1M Na_(2)SO_(4) solution. Calculate osmotic pressure of resulting solutions , if temperature is 300 K ?

What volume (in ml) of 0.8M AlCl_(3) solution should be mixed with 50 ml of 0.2 M CaCl_(2) solution to get solution of chloride ion concentration equal to 0.6 M ?

40 ml of 0.1 M CaCl_2 solution is mixed with 50 ml of 0.2 M AgNO_3 solution. Mole of AgCl formed in the reaction is

20 mL of 0.5 M HCl is mixed with 30 mL of 0.3 M HCl, the molarity of the resulting solution is :

200 ml of water is added of 500 ml of 0.2 M solution. What is the molarity of this diluted solution?