Saturday, March 8, 2014

What volume of 0.250 M potassium hydroxide solution is needed to react completely with a solution containing 1.00 g of phosphoric acid?

This is an acid-base neutralization reaction, represented by the following equation:


`3 KOH + H_3PO_4 -gt K_3PO_4 + 3 H_2O`


From the balanced equation, we can see that 3 moles of KOH react for every one mole of phosphoric acid. Here are the steps to solving the problem:


1. Find molar mass of phosphoric acid:


3(1.01) + 30.97 + 4(16.00) = 98.0 grams/mole


2. Find moles of phosphoric acid:


1.00 g H3PO4 x (1 mole/98.0g)...

This is an acid-base neutralization reaction, represented by the following equation:


`3 KOH + H_3PO_4 -gt K_3PO_4 + 3 H_2O`


From the balanced equation, we can see that 3 moles of KOH react for every one mole of phosphoric acid. Here are the steps to solving the problem:


1. Find molar mass of phosphoric acid:


3(1.01) + 30.97 + 4(16.00) = 98.0 grams/mole


2. Find moles of phosphoric acid:


1.00 g H3PO4 x (1 mole/98.0g) =0.0102 moles


3. Find moles of KOH neutralized by 0.0102 moles H3PO4:


(0.0102 moles H3PO4) x (3 moles KOH/1 mole H3PO4) = 0.0306 moles KOH


4. Find volume of 0.250M KOH that contains 0.0306 moles KOH:


(M = molarity = moles of solute /1 liter of solution)


(0.0306 moles) x (1 liter/0.250 moles) = 0.122 liters  = 122 milliliters 

No comments:

Post a Comment

What is the Exposition, Rising Action, Climax, and Falling Action of "One Thousand Dollars"?

Exposition A "decidedly amused" Bobby Gillian leaves the offices of Tolman & Sharp where he is given an envelope containing $1...