A solution is made by adding 2.3 moles of Sr3(PO4)2 in 3.5L of water. Which of...
A solution is made by adding 2.3 moles of Sr3(PO4)2 in 3.5L of water. Which of the following statements are true?
- The solution is strongly basic
- The solution is strongly acidic
- The solution is weakly basic
- The solution is weakly acidic
- The solution is neutral
- The Ka and Kb of the species added must be known
Why would this not be weakly basic if the "roots" are Sr(OH)2, a strong base, and H3PO4, a weak acid? Do I have the roots wrong
Homework Answers
Your Reasoning is absolutely Correct. Aqueous Solution of Strontium Phosphate is Weakly Basic. But, The Correct Option will be :
- The Ka and Kb of the Species added must be known.
Because, Only from this information, you can know that Sr(OH)2 is a Strong Base and H3PO4 is a Weak Acid.
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A solution is made by adding 2.3 moles of
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Polyprotic acids have more than one proton to donate to water, therefore have more than one equilibrium constant for proton donation. For phosphoric acid, there is a three-step equilibrium: H, PO +H,0 5 H2PO4 + H30* H,PO," +H,0 5 HPO - +H30* HPO 2- +,0 5 PO.- +,0* Kai = 7.11 x 10-3 Ka2 = 6.32 x 10-8 Ka; = 4.5 x 10-13 For all conjugate acid base pairs: K, XKK where K is for the reaction...
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