Precipitation of Silver Chloride

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Question 1

15 points

A 450.0 mL sample of a 0.292 M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the mass of the solid produced?

g solid produced

Hint 1

Always start by writing the equation for the reaction. Top of page

Hint 2

Balance the equation in standard form (using only whole numbers). 2 AgNO3(aq) + 1 CaCl2(aq) 2 AgCl(s) + 1 Ca(NO3)2(aq) Good effort! Top of page

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Hint 3

How many moles of Ag+ are present? * .1314 mol Ag+ Use this information to help you solve the problem! * Note : Significant figures are incorrect for answers marked with an asterisk. Top of page

More information on this hint

To find moles --Select--dividemultiply volume by the --Select--molar massdensitymolaritymass. First-rate thinking! Top of page

Hint 4

How many moles of CaCl2 are present? .0800 mol CaCl2 Excellent! Top of page

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Hint 5

Use the balanced equation to complete the mole ratio between AgNO3 and CaCl2. NOTE: Enter a ratio such as 1/2, 2/3, etc. = 2/1 Keep on truckin’! Top of page

Hint 6

The limiting reactant is --Select--calcium chloridesilver nitrate. Good to go from here! Top of page

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Hint 7

What number of moles of AgCl will be produced? .131 mol AgCl Good! Now you’re on your way to solving the problem! Top of page

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Hint 8

What mass of AgCl is produced? g AgCl Top of page

More information on this hint

To find mass of a compound we --Select--multiplydivide moles by --Select--massvolumemolaritymolar mass. Hope this helps! Top of page

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