The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH.

Question

The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH.

What volume of NaOH is needed to reach the end point of the titration?

What was the initial concentration of HCl?

Answer 1

I posted a response earlier that you don't have enough information to answer this question. There are four items you need.

1. volume HCl
2. M HCl
3. volume NaOH
4. M NaOH.
You need any three of the four, then you can calculate the fourth..

Answer 2

To find the volume of NaOH needed to reach the end point of the titration, we need to determine the stoichiometry of the reaction between HCl and NaOH.

The balanced equation for the reaction is:

HCl + NaOH -> NaCl + H2O

From the equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH. In other words, the stoichiometric ratio between HCl and NaOH is 1:1.

To determine the volume of NaOH needed, we need to neutralize all the HCl present in the flask. The number of moles of HCl can be found by multiplying the initial concentration (in M) by the volume (in liters) of HCl solution used.

Given that the flask contains 10.0 mL of HCl, we can convert it to liters by dividing by 1000:

10.0 mL ÷ 1000 = 0.010 L

Next, we can calculate the number of moles of HCl using the formula:

moles of HCl = concentration × volume

Let's assume the initial concentration of HCl is "x" M. Therefore:

moles of HCl = x M × 0.010 L

Now, to determine the volume of NaOH needed to reach the end point, we can use the stoichiometry of the reaction. Since 1 mole of HCl reacts with 1 mole of NaOH, the number of moles of NaOH needed will also be equal to "x" moles.

To convert the number of moles of NaOH to volume (in liters), we can use the formula:

volume (in L) = moles ÷ concentration

Here, the concentration of NaOH is given as 0.270 M. Therefore:

volume of NaOH = x moles ÷ 0.270 M

To find the initial concentration of HCl, we need to know the volume of NaOH required to reach the end point of the titration. Unfortunately, the question does not provide that information. We can only calculate the initial concentration of HCl if we know the volume of NaOH required for neutralization.

Therefore, we cannot determine the initial concentration of HCl with the given information.

The flask shown here contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.270 M NaOH.

I posted a response earlier that you don't have enough information to answer this question. There are four items you need.

KHBKJBK

noob

To find the volume of NaOH needed to reach the end point of the titration, we need to determine the stoichiometry of the reaction between HCl and NaOH.