In: Chemistry
K2SO4(aq) + AgNO3(aq) → Ag2SO4(s) + KNO3 (aq)
a Balance the reaction.
b. Given that you have a 1.75 L solution of 0.170 M K2SO4 and a 2.00 L solution of 0.110 M AgNO3, calculate the amount in grams of precipitate formed. Show work
c.Calculate the concentration of SO2− ions left after the reaction has been completed
precipitate formed. show work
(a) Balancing the equation
K2SO4(aq) + AgNO3(aq) → Ag2SO4(s) + KNO3 (aq)
You can see that the starting material has 2 K atoms so the product needs to have 2 K so 1 KNO3 become 2 KNO3 now since NO3 is 2 equivalent we make AgNO3 in the starting as 2 AgNO3. So now there are 2 Ag to start with but in the product also we have 2 Ag as Ag2SO4 so the equation is completelt balanced
Balanced equation
K2SO4(aq) + 2AgNO3(aq) → Ag2SO4(s) + 2KNO3 (aq)
(b) 1.75 L solution of 0.170 M K2SO4 and a 2.00 L solution of 0.110 M AgNO3
1.75 L solution of 0.170 M K2SO4
means 1.75 x 0.170 M = 0.2975 moles of K2SO4
2.00 L solution of 0.110 M AgNO3
means 2.0 x 0.110 M = 0.22 moles of AgNO3
As per the balance equation
K2SO4(aq) + 2AgNO3(aq) → Ag2SO4(s) + 2KNO3 (aq)
2 moles of AgNO3 gives 1 mole of Ag2SO4(s) which is the precipitate
since we have 0.22 moles of AgNO3 we will have 0.11 mole of Ag2SO4(s) precipitate
MW of Ag2SO4 is 311.79 g·mol−1
so 0.11 mole of Ag2SO4 will be 0.11 moles x 311.79 g·mol−1 = 34.29 g
so 34.29 g of precipitate is formed
(c) Calculate the concentration of SO2− ions left after the reaction has been completed
0.11 mole of Ag2SO4(s) precipitate
1 mole of Ag2SO4 has 1 mole of SO4 (sulphate)
We started the reaction with 0.2975 moles of K2SO4 this has 0.2975 moles of SO4
since 0.11 moles of SO4 precipitate as Ag2SO4
0.2975 - 0.11 moles of SO4 remain in solution
0.1875 moles of SO4 remain in solution
In the reaction total volume is 1.75 L K2SO4 solution and a 2.00 L AgNO3 solution
That is 3.75 L total solution
Concentration of SO4 will be moles/L or 0.1875 moles in 3.75 L
That is 0.05 moles/litre or 0.05 M is the concentration of sulphate