Question 10, HW Week 10
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Question 10, HW Week 10
The question asks you to arrange solutions from highest to lowest pH. I knew that HNO3 is a strong acid, so it has the lowest pH. HBrO is a weak acid, so it's the next highest on the list. NH3 is a weak base, so it goes after HBrO. However, RbOH and Sr(OH)2 are both strong bases. How do I determine which has the higher pH?
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Re: Question 10, HW Week 10
Hi! To answer this question, you need to see how strong the two bases are relative to each other. In regards to this question, Sr(OH)2 produces two OH− ions per formula unit, it will give a more basic solution than RbOH, which produces only one OH− ion per formula unit. Thus, Sr(OH)2 is more basic since it releases more hydroxide ions into a solution than RbOH would. Hope this helps!
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Re: Question 10, HW Week 10
In order to figure out whether RbOH or Sr(OH)2 is stronger, it is good to know that the more OH- ions it produces, the stronger it will be. Therefore, Sr(OH)2 is a stronger base than RbOH.
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Re: Question 10, HW Week 10
Hi,
You would be able to determine which is the stronger base based on how many OH- ions in the formula. Since Sr(OH)2 produces 2 and RbOH only produces one, we can conclude that Sr(OH)2 is a stronger base, thus making it have a higher ph.
You would be able to determine which is the stronger base based on how many OH- ions in the formula. Since Sr(OH)2 produces 2 and RbOH only produces one, we can conclude that Sr(OH)2 is a stronger base, thus making it have a higher ph.
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Re: Question 10, HW Week 10
between RbOH and Sr(OH)2, Sr(OH)2 is the stronger base since it has 2 "OH"'s.
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Re: Question 10, HW Week 10
The more H+ there are, the stronger the acid is. The more OH- there are, the more basic the solution. You can check on how many OH- there are in each compound, and the one with the higher number of OH reigns as the more basic compound
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