How Do You Calculate Molarity and Percent Mass in a Titration?

[leah0084]

Homework Statement

A student finds that it takes 32.17 mL of 0.1048 M NaOH to titrate 5.000 mL of sulfuric acid solution. Determine the molarity and percent mass of the sulfuric acid in the solution (you may assume that the density of the sulfuric acid solution is the same as pure water).
____M
____% sulfuric acid by mass.

Homework Equations

The Attempt at a Solution

our professor did not go through this part of the chapter yet but assigned the homework anyway. could anybody help me out please?

 

[anathema]

Hello student,

I am happy to help you with this problem. First, let's review the definition of molarity and percent mass. Molarity (M) is defined as the number of moles of solute per liter of solution. Percent mass is the mass of the solute divided by the total mass of the solution, multiplied by 100%.

To solve this problem, we need to use the equation M1V1 = M2V2, where M1 is the molarity of the sulfuric acid solution, V1 is the volume of the solution used in the titration (5.000 mL), M2 is the molarity of the NaOH solution, and V2 is the volume of NaOH used in the titration (32.17 mL).

From the problem, we know that the molarity of the NaOH solution is 0.1048 M. Plugging in all the values into the equation, we get:

M1(5.000 mL) = (0.1048 M)(32.17 mL)

M1 = (0.1048 M)(32.17 mL)/(5.000 mL)

M1 = 0.673 M

So, the molarity of the sulfuric acid solution is 0.673 M.

To find the percent mass of sulfuric acid, we need to know the mass of the solute (sulfuric acid) and the total mass of the solution. Since we are assuming that the density of the sulfuric acid solution is the same as pure water, we can use the density of water (1 g/mL) to find the mass of the solution. The total volume of the solution is 5.000 mL, so the total mass of the solution is 5.000 g.

To find the mass of sulfuric acid, we can use the molarity and volume of the solution. The molarity tells us the number of moles of sulfuric acid per liter of solution, so we can use the following equation to find the number of moles of sulfuric acid:

moles of sulfuric acid = molarity x volume (in liters)

= (0.673 mol/L)(0.00500 L)

= 0.003365 mol

Now, we can use the molar mass of sulfuric acid (98.08 g/mol) to find the mass of sulfuric acid:

mass of sulfuric acid = moles of sulfuric

 

[ogb p]

I understand the importance of carefully following instructions and completing assignments to the best of my ability. In this case, it seems that your professor has assigned a problem that may require knowledge beyond what has been covered in class so far. However, I can offer some guidance on how to approach this problem.

Firstly, it is important to understand the concept of titration and how it is used to determine the concentration of a solution. In this case, we are using a known concentration of NaOH to neutralize a known volume of sulfuric acid solution. The volume and concentration of NaOH used in the titration can be used to calculate the moles of NaOH used.

Next, we need to use the balanced chemical equation for the reaction between NaOH and sulfuric acid to determine the moles of sulfuric acid present in the 5.000 mL solution. From there, we can calculate the molarity of the sulfuric acid solution by dividing the moles of sulfuric acid by the volume of the solution (in liters).

To determine the percent mass of sulfuric acid in the solution, we need to use the molarity and the molar mass of sulfuric acid to calculate the moles of sulfuric acid present in the solution. Then, we can use the mass of the solution (which can be calculated from the density and volume) to calculate the percent mass of sulfuric acid.

Overall, it is important to carefully follow the steps and make sure all units are consistent in order to arrive at the correct solution. If you are still unsure, I would recommend reaching out to your professor for clarification or seeking additional resources such as a tutor or online tutorials. Good luck with your homework!

 

[m2003]

As a scientist, it is important to always follow the scientific method and approach problems with a systematic and logical approach. In this case, we are given information about a titration experiment and asked to determine the molarity and percent mass of sulfuric acid in a solution.

To begin, we can start by writing down the given information and identifying any relevant equations or concepts that may be useful in solving the problem. From the statement, we know that 32.17 mL of 0.1048 M NaOH was used to titrate 5.000 mL of sulfuric acid solution. This information can be represented as follows:

NaOH (aq) + H2SO4 (aq) → H2O (l) + Na2SO4 (aq)

From this balanced equation, we can see that there is a 1:1 mole ratio between NaOH and H2SO4. This means that the number of moles of NaOH used in the titration is equal to the number of moles of H2SO4 in the sulfuric acid solution.

Next, we can use the molarity formula, M = moles/volume (in liters), to solve for the molarity of the sulfuric acid solution. We know that the volume of NaOH used is 0.03217 L (converted from 32.17 mL) and the molarity of NaOH is 0.1048 M. Plugging these values into the formula, we get:

M = moles/0.03217 L
0.1048 M = moles/0.03217 L
moles = 0.003317

Since there is a 1:1 mole ratio between NaOH and H2SO4, we can conclude that there are also 0.003317 moles of H2SO4 in the sulfuric acid solution.

To find the molarity of the sulfuric acid solution, we can use the same formula, M = moles/volume. The volume in this case is 0.005000 L (converted from 5.000 mL). Plugging in the values, we get:

M = 0.003317 moles/0.005000 L
M = 0.6634 M

Finally, to find the percent mass of sulfuric acid in the solution, we can use the formula % mass = (mass of solute/mass of solution)