If 17.5 mL of 0.553 M KOH is needed to neutralize 25.0 mL of an HBr solution what is the molarity od HBr solution
moles KOH = .0175 * .553 = .00968
so, you need that many moles of HBr, making the molarity
M = .00968/.025 = 0.387
To find the molarity of the HBr solution, we need to use the concept of stoichiometry. In a neutralization reaction between KOH (potassium hydroxide) and HBr (hydrogen bromide), they react in a 1:1 ratio:
KOH + HBr → KBr + H2O
This means that one mole of KOH reacts with one mole of HBr.
First, let's calculate the number of moles of KOH used:
Moles of KOH = volume (in liters) × molarity
= 17.5 mL × 0.553 M
= 0.00968 moles
Since KOH and HBr react in a 1:1 ratio, the number of moles of HBr in the neutralized solution is also 0.00968 moles.
Now, let's find the molarity of HBr:
Molarity of HBr = moles of HBr / volume (in liters)
= 0.00968 moles / 0.0250 L
= 0.387 M
Therefore, the molarity of the HBr solution is 0.387 M.