What is the pH of a solution containing formic acid and potassium formate?

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The discussion revolves around calculating the pH of a solution containing 1.00 g of formic acid and 1.00 g of potassium formate dissolved in 100.0 ml of water. Participants express confusion about whether a reaction occurs between the two substances, clarifying that potassium formate is not an acid but a salt. The correct chemical formula for potassium formate is identified as KHCO2. The focus remains on understanding how to approach the pH calculation with the given components. The thread highlights the importance of distinguishing between acids and their corresponding salts in solution chemistry.
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1.00 g of formic acid and 1.00 g of potassium formate acid are dissolved in enough water to give 100.0 ml of solution. Calculate the pH of the solution.

>> I'm not really sure how to start this. These are two acids being mixed together... Would there be a reaction? I'm very confused on how to start this problem...
 
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Please any help would be greatly appreciated :(
 
Kawrae said:
1.00 g of formic acid and 1.00 g of potassium formate acid are dissolved in enough water to give 100.0 ml of solution. Calculate the pH of the solution.

>> I'm not really sure how to start this. These are two acids being mixed together... Would there be a reaction? I'm very confused on how to start this problem...

Check your question again. That should probably just be potassium formate. It's not an acid.
 
Oh yes you're right, I must have copied it wrong.

Okay, one more question: does anyone know the chemical formula for potassium formate?? I can't seem to find it anywhere in my book or online...
 
Potassium formate is KHCO2.
 
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