2.) A n experiment similar to the one performed was done in order to determine t

Question

2.) A n experiment similar to the one performed was done in order to determine the Ksp of Ba(OH)2. In this instance, a strong acid, HCl is placed in the buret and a titration performed. Using the data provided, complete the remaining entries in the table. a. Write the solubility equation of Ba(OH)2(s) in water. b. Write the Ksp expression for this equilibrium. c. Write the reaction that occurs when HCl is added. d. If phenolphthalein is used as an indicator, describe the appearance of the solution prior to and at the endpoint.

Explanation / Answer

Ba(OH)2 +2HCl-----------> BaCl2 +2H2O

before and after addition pink to clear

Average titration volume= (39.71+39.86+39.75)/3= 39.77 ml =0.03977 L

Molarity of HCl = 0.05020M, moles of HCl =0.03977*0.05020=.001966 moles= 1.996 milli moles

2 moles of HCl correspond to 1 mole of Ba(OH)2

1.996 millimoes correspond to 1.996/2= 0.998milli moles of Ba(OH)2

Ba(OH)2-------> Ba+2 +2OH-

1 milli mole of Ba(OH)2 gives 2 moles of OH-

0.998 mill moles of Ba(OH)2 correspond to 0.998*2= 1.996 mill moles of OH-

Concentrations

Ba+2= 0.998*10(-3)*1000/25=0.03992 mole/L

OH- = 1.996*10-3*1000/25= 0.07984 moles/L

Solubility of Ba(OH)2= 0.03992*171.35 g/L =6.84 g/L

Ksp =[Ba+2] [OH-]2 = 0.03992*(*0.07984)2 =0.000254

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