Is the solution produced by adding 1.0 mols K2CO3(s) to 1.0 L of 1.0 M (HO)3PO m

Question

Is the solution produced by adding 1.0 mols K2CO3(s) to 1.0 L of 1.0 M (HO)3PO mildly or strongly acidic or mildly or strongly basic? Discuss the chemistry which defends/explains your answer including equations for all pertinent B/L acid-base reactions involved. Also, calculate the pH for this solution. Include equations for all pertinent B/L acid-base reactions and indicate all necessary calculations but not actual arithmetic. Strong heating can change the pH of this solution significantly. Why? On strong heating could this change be prevented? Comment/explain. Please help!

Explanation / Answer

The balanced chemical equation between potassium carbonate and phosphoric acid is as follows:

3K2CO3 +2 H3PO4 ------> 3CO2 + 2K3PO4 + 3H2O

so when 1 mole of K2CO3 reacts with 1 moles of H3PO4..some amount of H3PO4 will left out..as 0.66 mole of H3PO4 is required to react with 1 moles of K2CO3.

and as H3PO4 is weak acid. solution will be mildly acidic.for calculating pH we will be needing the dissociation constant of H3PO4

H3PO4 <--> H2PO4- + H+

then we can find the concentration of H+

and therefor pH which is equal to -log[H+].

on heating dissociation constant and K of H3PO4 will change which will led to change in the concentration of [H+] and hence the pH

hopefully it help u..if u need to know anything else..i will be glad to help u.

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