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Write the total and net ionic equations for the reaction of BaSO4 dissociation, and calculate the trial Ksp for the product formed, when 40 mL of 0.1 M Ba(CH3COO)2 reacts with 60 mL 0.6 M MgSO4 and decide whether a ppt will form?

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Elin Hessel
Elin HesselLv2
28 Sep 2019

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Related questions

1. This experiment involves the reaction of Ba(OH)2 with H2SO4. Which of the following gives the balanced chemical reaction used in the experiment?

a. Ba(OH)2(aq) + H2SO4(aq) → H2Ba(s) + SO4(OH)2(l)
 
b. Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + H2O(l)
 
c. BaSO4(s) + 2H2O(l) → Ba(OH)2(aq) + H2SO4(aq)
 
d. Ba(OH)2(aq) + H2SO4(aq) → BaSO4(s) + 2H2O(l)
 
2) Which of the following gives the net ionic reaction for the reaction used in this experiment?
 
a. H+(aq) + OH-(aq) → H2O(l)
 
b. no net reaction
 
c. Ba2+(aq) + SO42-(aq) → BaSO4(s)
 

d. Ba2+(aq) + 2OH-(aq) + 2H+(aq) + SO42-(aq) → BaSO4(s) + 2H2O(l)

3) Ranjit titrates a sample 10.00 mL of Ba(OH)2 solution to the endpoint using 12.58 mL of 0.1023 M H2SO4.

Based on this data, calculate the concentration of the barium hydroxide solution.

[Ba(OH)2] = ___ M

4) Xianming runs a titration and collects, dries, and weighs the BaSO4(s) produced in the experiment. He reports a mass of 0.2989 g  Ba2SO4. Based on this, calculate the concentration of Ba(OH)2 solution.

[Ba(OH)2] = ___ M

 


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