A goal of the acid-base titration in this scenario is to determine the concentration of sodium hydroxide solution. To do this, a 1.3000 g sample of potassium hydrogen phthalate (KHC8H4O4) is massed out. The KHP has one acid proton (H+). The solid is dissolved in a beaker and 2 drops of phenolphthalein indicator is used to note an endpoint. The difference between the initial and final buret readings shows that exactly 41.20 mL of the NaOH solution is required to react with KHP. Calculate the concentration of the NaOH solution.
If anybody can explain what this is saying and walk me through it I'd greatly appreciate it.
To determine the concentration of the sodium hydroxide (NaOH) solution in this scenario, an acid-base titration is performed using potassium hydrogen phthalate (KHP) as the primary standard.
First, a 1.3000 g sample of KHP is weighed out. KHP is a solid that contains one acid proton (H+). The solid is then dissolved in a beaker.
Next, two drops of phenolphthalein indicator are added to the solution. Phenolphthalein is commonly used in acid-base titrations to visualize the endpoint, which is the point at which the acid and base have completely reacted.
The titration is performed by adding the NaOH solution from a buret (a calibrated glass tube for precise liquid measurements) to the KHP solution in the beaker. The NaOH solution is gradually added until a color change is observed due to the presence of the phenolphthalein indicator. This color change indicates that the reaction between the acid (KHP) and the base (NaOH) is complete.
The volume of NaOH required to reach the endpoint is measured by noting the initial and final readings on the buret. In this case, the difference between the initial and final buret readings is precisely 41.20 mL, which represents the volume of NaOH solution required to react with the KHP.
To calculate the concentration of the NaOH solution, we can use a balanced chemical equation and the concept of stoichiometry.
The balanced equation for the reaction between KHP and NaOH is:
KHC8H4O4 + NaOH -> KC8H4O4Na + H2O
Based on the balanced equation, it can be determined that one mole of KHP reacts with one mole of NaOH.
To calculate the number of moles of NaOH used in the titration, we can use the formula:
moles of NaOH = volume (in liters) × molarity
Given that the volume of NaOH used is 41.20 mL (or 0.04120 L) and that the number of moles of KHP is determined by its mass (1.3000 g) divided by its molar mass, we can calculate the moles of NaOH used.
The molar mass of KHP (KC8H4O4) can be calculated by summing the atomic masses of its constituent elements: Potassium (K), Carbon (C), Hydrogen (H), and Oxygen (O).
Now, with the moles of NaOH used and the moles of KHP, we can determine the molarity (concentration) of the NaOH solution by dividing the moles of NaOH by the volume of NaOH used (in liters):
molarity of NaOH = moles of NaOH / volume (in liters)
By performing these calculations based on the given information, you can find the concentration of the NaOH solution.