Solution Stoichem Questions

label Chemistry
account_circle Unassigned
schedule 1 Day
account_balance_wallet $5

(a) A sample of solid Ca(OH)2 is stirred in water at 30°C until the solution contains as much dissolved Ca(OH)2 as it can hold. A 100.-mL sample of this solution is withdrawn and titrated with 5.00 ✕ 10−2 M HBr. It requires 48.8 mL of the acid solution for neutralization. What is the molarity of the Ca(OH)2 solution?

(b) What is the solubility of Ca(OH)2 in water, at 30°C, in grams of Ca(OH)2 per 100 mL of solution?

Oct 3rd, 2015

Thank you for the opportunity to help you with your question! I will do my best!


Ca(OH)2 + 2HBr → CaBr2 + 2H2O 
1mol Ca(OH)2 reacts with 2mol HBr 

Ma * Va = 2* Mb*Vb 
Ma * 100 = 2*0.05* 48.8 
Ma = 2*0.05*48.8/100 
Ma = 0.0488 mol Ca(OH)2 per litre 
Molarity of Ca(OH)2 solution = 0.0488M First answer 

Molar mass Ca(OH)2 = 74.093 g/mol 
0.0488M = 74.093*0.0488 = 3.616g/litre 


Solubility = 0.3616 g per 100 mL solution.

Please let me know if you need any clarification. I'm always happy to answer your questions. Thank you very much!
Sep 19th, 2015

Did you know? You can earn $20 for every friend you invite to Studypool!
Click here to
Refer a Friend
Oct 3rd, 2015
Oct 3rd, 2015
Jun 28th, 2017
Mark as Final Answer
Unmark as Final Answer
Final Answer

Secure Information

Content will be erased after question is completed.

Final Answer