Home
Class 12
CHEMISTRY
What is the mass of precipitate formed w...

What is the mass of precipitate formed when 50 mL of `16.9%` solution of `AgNO_(3)` is mixed with 50 mL of `5.8%`NaCl solution?
(Ag=107.8,N=14,O=16,Na=23,Cl=35.5)

A

7g

B

14g

C

28g

D

3.5g

Text Solution

Verified by Experts

The correct Answer is:
A
Molarity (M) of `AgNO_(3)=(16.9xx10)/(169.3)=1.0M`
Molarity (M) of `NaCl=(5.8)/(58.5)xx10=0.9914M`
`AgNO_(3) +NaCl to AgCl darr+NaNO_(3)`
Moles `n={:((0.99Mxx50)/(1000),(0.99xx50)/(1000) ),(cong0.05,cong0.05):}`
`therefore` mols of AgCl formed=0.05
Mass of AgCl=0.05`xx142.5=7g`
Promotional Banner

Similar Questions

Explore conceptually related problems

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?

What will be present in th solution when 50 of ml 0.1 M HCl is mixed with 50 ml of 0.1 M NaOH soltion?

What mass of pb^(2+) ions is left in solution, when 50.0mL of 0.20M Pb(NO_(3))_(2) is added to 50.0mL of 1.5M NAC1 ?

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 ?

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

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) .

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

50mL of a solution containing 10^(-3) mole of Ag^(+) is mixed with 50 mL of a 0.1M HCl solution. How much Ag^(+) remains in solution ? (K_(sp) of AgCl=1.0xx10^(-10))

The amount of BaSO_(4) formed upon mixing 100mL of 20.8% BaCl_(2) solution with 50mL of 9.8% H_(2)SO_(4) solution will be : (Ba = 137, Cl = 35.5, S = 32, H = 1 and O =16)

When 100 ml of M/10 NaOH solution and 50 ml of M/5 HCI solution are mixed, the pH of resulting solution would be