Question

Questions 1. Why do you want to stop the titration of want to stop the titration of the solution at the lightest pink color you can detect? Because it's the equvilant point 2. How would this experiment change if the HCI was the standard solution and NaOH was the unknown? 3. What is the proper way to dilute acids with water? water then acid 4. In this experiment, you diluted the HCI given to you and then titrated the samples. What are the possible sources of error in the titration of the HCl samples? 5. Describe how to make 500 mL 0.464 M HNO, from a 6.00 M HNO, solution. 6. A titration of 50.00 mL of an unknown concentration of H,SO, required 29.26 mL of 0.1512 M NaOH standard. What is the molarity of the H, SO, solution?

Answer 1

Ans:

2. In the above titration reaction of HCl and NaOH, if HCl is the standard solution and NaOH is the unknown, then we need to use a different indicator to observe the change in colour at its equivalence point.
for example: methyl orange is used as an indicator to change colour in acidic range and phenolphthalein is used for the basic range. Phenolphthalein is pink in basic solutions and turns colourless in acidic solutions.

4. In the above experiment, if we dilute the standard solution of HCl then as per the equation,
M₁V₁ = M₂V₂

M_HCl and V_NaOH are constant, if we increase the V_HCl then M_NaOH will increase.

Thus it will show higher concenteration of NaOH.