what is the molarity of a h2so4 solution if 18.5ml of naoh are needed to neutralize 25.0 mL of the sample?
Don't get too lazy in chemistry that you can't punch the caps key. Co, CO, and co are three distinct things.
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
You didn't provide enough information to answer the question.
To determine the molarity of the H2SO4 solution, we first need to know the balanced equation for the neutralization reaction between H2SO4 and NaOH. The balanced equation is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH.
Next, we need to calculate the number of moles of NaOH that reacted. To do this, we will use the following formula:
moles = volume (in liters) × molarity
Given that 18.5 mL of NaOH solution was needed to neutralize the H2SO4 solution, we need to convert this volume to liters. Since there are 1000 mL in 1 L, we can calculate:
volume (in liters) = 18.5 mL / 1000 = 0.0185 L
Now we need to find the molarity of NaOH. However, this information is not provided in the question. So, without this information, we cannot determine the molarity of the H2SO4 solution using this data alone.
To calculate the molarity of the H2SO4 solution, we need additional information. Specifically, we need the molarity of the NaOH solution used for neutralization. With that information, we can use the balanced equation and the stoichiometry of the reaction to determine the molarity of the H2SO4 solution.