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What is the endpoint of a titration of NaOH?

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What is the endpoint of a titration of NaOH?

The point at which exactly enough titrant (NaOH) has been added to react with all of the analyte (HCl) is called the equivalence point. As such, it should change from colorless to purple around the equivalence point of this titration. Our approximation of where the equivalence point occurs is called the endpoint.

How do you find the volume of NaOH for a titration?

Calculating a volume

  1. 25.00 cm 3 of 0.300 mol/dm 3 sodium hydroxide solution is exactly neutralised by 0.100 mol/dm 3 sulfuric acid.
  2. Volume of sodium hydroxide solution = 25.0 ÷ 1000 = 0.0250 dm 3
  3. Amount of sodium hydroxide = concentration × volume.
  4. Amount of sodium hydroxide = 0.300 mol/dm 3 × 0.0250 dm 3
  5. = 0.00750 mol.
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What volume of 0.200 M NaOH is required to react completely with 25 mL of 0.020 M HCL?

Also, recall that moles = molarity × volume. ANSWER: The volume of NaOH required is 25.2 mL.

How do you titrate H2SO4 with NaOH?

These have 2 equivalent points – one when the first H+ is lost, and another when the second H+ is lost. If you are to told to titrate H2SO4 with NaOH, you can’t do it until you are told which equivalence point you are after. Then you choose a suitable indicator – one whose end point is the same as the equivalence point.

What is the pH at the equivalence of NaOH?

In the example above, the pH at the equivalence (the amount of NaOH added that completely reacts with all the NaOH) point is 7. So, you need an indicator that changes color at pH 7.

What is the theoretical value of NaOH to be poured?

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The theoretical value of NaOH to be poured was 9.50 cm 3, and more or less than 0.1 cm 3 of that value. However, the amount I added on an average was 10.4 cm 3, which suggests why the solution became unusually dark pink as supposed to light pink.

Is NaOH a good base to titrate acetic acid?

NaOH isn’t a particularly strong base. It’s not particularly dangerous either. Especially not if you use it at 0.1 M – 1M concentrations which is what undergrads use to titrate acetic acid. And no, I don’t think there is. If you use a carbonate base, you have a problem because you can’t really standardize it.