Home
Class 12
CHEMISTRY
500 ml of a 0.1 N solution of AgNO(3) ad...

500 ml of a 0.1 N solution of `AgNO_(3)` added to 500 mlof 0.1 N solution of KCI. The concentration of nitrate ion in the resulting mixture is

A

0.05 N

B

0.1 N

C

0.2 N

D

reduced to zero

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Similar Questions

Explore conceptually related problems

250 ml of 0.10 M K_2 SO_4 solution is mixed with 250 ml of 0.20 M KCI solution. The concentration of K^(+) ions in the resulting solution will be:

If 250 ml of 0.25 M NaCl solution is diluted with water to a volume of 500 ml, the new concentration of 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)

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.

Silver is removed electrolytically from 200mL of a 0.1N solution of AgNO_(3) by a current of 0.1A . How long will it take to remove half of the silver from the solution ?

On addition of 100mL 0.01 M of NaOH solultion to 100mL 0.01M triethyl amine solution .The concentration of Triethyl ammonium ion [C_(6)NH_(16)]^(+) in resulting solution will be :

6.025 xx 10^(20) molecules of acetic acid are present in 500 ml of its solution. The concentration of solution is

1 mL of 0.1 N HCl is added to 999 mL solution of NaCl. The pH of the resulting solution will be :

Equal volumes of 0.1M AgNO 3 ​ and 0.2M NaCl are mixed. The concentration of NO 3 − ​ ions in the mixture will be:

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