Question

you mix excess AgNO3 with 25.0 ml of 0.302 M KCl is the maximun mass in...

you mix excess AgNO3 with 25.0 ml of 0.302 M KCl is the maximun mass in grams of AgCl that can be formed ?g ?

Homework Answers

Answer #2

thereaction is

AgNO3 + KCl --> AgCl + KNO3

Here AgNO3 is inexcess so limiting reagent is KCl

USE,

number of mole = molarity*volume of solution (in liter)

number of mole of KCl =(0.302*25)/1000

number of mole of KCl = 7.6*10-3

acording to above balanced equation 1 mole of KCl produces 1mole of AgCl

so,

7.6*10-3 mole of KCl produces 7.6*10-3mole of AgCl

mole of AgCl formed = 7.6*10-3

mass of AgCl formed/molar mass of AgCl= 7.6*10-3

molar massof AgCl= 143.3

mass of AgCl formed =  7.6*10-3*143.3 g

mass of AgCl formed = 1.09 g

answered by: anonymous
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
1- If 27.0 mL of AgNO3 is needed to precipitate all the Cl− ions in a...
1- If 27.0 mL of AgNO3 is needed to precipitate all the Cl− ions in a 0.795-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution? 2- If 45.7 mL of 0.110 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl,...
When 125 mL of 0.500 M AgNO3 is added to 100. mL of 0.300 M NH4Cl, how many extra mLs of excess reactant were used? AgNO3 (aq) + NH4Cl(aq) → AgCl(s) + NH4NO3 (aq)
Determine if AgCl precipitates out of solution when 200 mL of 1.0x10x-4 M AgNO3(aq) is mixed...
Determine if AgCl precipitates out of solution when 200 mL of 1.0x10x-4 M AgNO3(aq) is mixed with 900 mL of 1.0x10-6M KCl(aq). Ksp AgCl = 1.6x10-10
If 30.00 mL of 0.150 M CaCl2 is added to 20.5 mL of 0.100M AgNo3, what...
If 30.00 mL of 0.150 M CaCl2 is added to 20.5 mL of 0.100M AgNo3, what is the mass of the AgCl precipitate?
What mass of KCl is required to make 46 mL of a 0.10 M KCl solution?...
What mass of KCl is required to make 46 mL of a 0.10 M KCl solution? ____________ g KCl     How many moles of potassium ions are present in the solution? ____________ mol
How many grams of AgCl are produced from the reation of 135 mL of 0.567 M...
How many grams of AgCl are produced from the reation of 135 mL of 0.567 M AgNO3 with an excess of AlCl3
1. An experiment calls for you to use 100 mL of 0.25 M HNO3 solution. All...
1. An experiment calls for you to use 100 mL of 0.25 M HNO3 solution. All you have available is a bottle of 3.4 M HNO3. How many milliliters of the 3.4 M HNO3 solution do you need to prepare the desired solution? 2. How many milliliters of water do you need to prepare the desired solution? A. You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.160 M HCl(aq) solution is needed to...
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution...
You mix 5.00 mL of 1.0x10^-5 M AgNO3 with 10.00 mL of 2.00 M NH3 solution resulting in the formation of diamminesiler(I) complex ion, [Ag(NH3)2]. (Assume volumes are additive). a. Write the net-ionic equilibrium equation for the formation of this complex ion. b. Calculate the concentration of the complex ion in the reaction mixture, assuming the reaction goes to completion.
How many milliliters of 0.215 M FeCl3 solution are needed to react completely with 32.7 mL...
How many milliliters of 0.215 M FeCl3 solution are needed to react completely with 32.7 mL of 0.0509 M AgNO3 solution? The net ionic equation for the reaction is: Ag+(aq) + Cl-(aq) AgCl(s) mL of FeCl3: How many grams of AgCl will be formed?
First, he standardized the AgNO3 titrant with 0.1242 g dry NaCl dissolved in 25.0 ml DI...
First, he standardized the AgNO3 titrant with 0.1242 g dry NaCl dissolved in 25.0 ml DI water, and 26.25 ml of titrant was consumed. Then he used the standardized titrant to determine the concentration of chloride in the solution. 11.71 ml of AgNO3 solution was used to titrate 25.00 ml of solution a) Calculate the concentration (M) of AgNO3 titrant. b) Determine the content of chloride in the unknown solution (M).
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT