Home
Class 12
CHEMISTRY
What weight of AgCl will be precipitated...

What weight of `AgCl` will be precipitated when a solution containing `4.77 g NaCl` is added to a solution of `5.77 g` of `AgNO_(3)`.

Text Solution

Verified by Experts

The correct Answer is:
4.879 gm
`L.R`
`darr`
`AgNO_(3)+NaCl to NaNO_(3)+AgNO_(3)`
`5.77 gm " " 4.77 gm `
` 0.034 "mole" " " 0.082 "mole"`
wt. of `AgCl=0.034xx143.5=4.879 gm`
Promotional Banner

Topper's Solved these Questions

  • MOLE CONCEPT

    ALLEN|Exercise Basic Exercise|29 Videos

  • MOLE CONCEPT

    ALLEN|Exercise S-I (Problems Related with Different Types of Atomic Masses & Basic Concept of Mole)|52 Videos

  • MOLE CONCEPT

    ALLEN|Exercise J-ADVANCE|2 Videos

  • METALLURGY

    ALLEN|Exercise EXERCISE-05 [B]|26 Videos

  • p-Block Element

    ALLEN|Exercise All Questions|20 Videos

Similar Questions

Explore conceptually related problems

The weight of AgCl precipitated when a solution containing 5.85 g of NaCl is added to a solution containing 3.4g of AgNO_3 is

When NaCl is added to aqueous solution of glucose

How many moles of AgCl will be precipitated when an excess of AgNO_3 is added to a molar solution of [CrCl(H_2O)_5]Cl_2 ?

Calculate the molarity of a solution containing 5 g of NaOH in 450 mL solution.

Ethyne gives a white precipitate with ammoniacal solution of ___. (AgNO_3//NaCl)

What happens when C Cl_(4) is treated with AgNO_(3) solution ?

Which of the following will not produce a precipitate with AgNO_3 solution?

What will be the molarity of a solution, which contains 5.85g of NaCl(s) per 500mL?

What will be the molarity of a solution, which contains 5.85g of NaCl(s) per 500mL?

What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO_(3) is mixed with 50 mL of 5.8% NaCl solution?