How many mL of 0.58 M sodium hydroxide solution should be required to neutralize 2.5 L of a hydrobromic acid solution that has a concentration of 4.22 mM?

Answer 1

first step is to write the balanced chemical equation:

NaOH + HBr --> NaBr + H2O

now you can use the molarity and volume of HBr to find the moles of HBr, convert moles of HBr to moles of NaOH, and finally convert moles of NaOH to volume using the molarity

(4.22E-3 mol/L HBr) X (2.5L HBr) X (1 mol NaOH/1 mol/L HBr) X (1 L NaOH/0.58 mol NaOH) X (1000ml/L)= 18.19 mL