Question
Can someone please explain this problem to me step by step pleaseeeeeee?
In the following acid—base neutralization reaction
HNO3 (aq)+ KOH (aq)---KNO3(aq) + H2O(I)
What is the molarity (M) of an HNO3 solution if 50.0ml is needed to react with 25.0ml of 0.150M KOH solution?
In the following acid—base neutralization reaction
HNO3 (aq)+ KOH (aq)---KNO3(aq) + H2O(I)
What is the molarity (M) of an HNO3 solution if 50.0ml is needed to react with 25.0ml of 0.150M KOH solution?
Answers
How many mols KOH do you have? That's mols KOH = M x L = ?
How many mols HNO3 will that neutralize. The same number since the equation is 1 mol HNO3 to 1 mol KOH.
M HNO3 = mols HNO3/L HNO3.
How many mols HNO3 will that neutralize. The same number since the equation is 1 mol HNO3 to 1 mol KOH.
M HNO3 = mols HNO3/L HNO3.