III. Questions. 1. During the preparation of the KHP solution, some KHP is spilled on the counter. How will this affect the calculated concentration of NaOH (too high, too low, or unchanged?) Explain clearly. 2. During the titration several milliliters of deionized water are added to the Erlenmeyer flask containing the KHP solution. How will this affect the calculated concentration of NaOH (too high, too low, or unchanged?) Explain clearly. 3. A 25.00 mL volumetric pipet is rinsed with deionized water. Several drops of water remain in the pipet. It is then used to deliver a 25.00 mL aliquot of the KHP solution into the Erlenmeyer flask in which the sample will be titrated. How will this affect the calculated concentration of NaOH (too high, too low, or unchanged?) Explain clearly. 4. A buret is cleaned and rinsed with deionized water. Some water remains in the buret. It is then filled with the NaOH solution which is being standardized. How will this affect the calculated concentration of NaOH (too high, too low or unchanged?) Explain clearly.
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If some KHP is spilled on the counter during the preparation of the KHP solution, the actual amount of KHP in the solution will be less than what was intended. This will result in a lower concentration of KHP in the solution. During the titration, less NaOH will Show more…
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1. Speculate on the shape of the curve that would be generated had the unknown acid been diprotic. How would this have changed your calculations? 2. Why doesn't it matter how much water you dissolve the KHP sample in at the beginning of the titration? 3. Why does it matter that you take care to dry the burette and rinse it with the standard NaOH solution before using it to titrate your unknown? 4. The concentration of your standard NaOH solution was determined by titrating it with a standard HCl solution. (a) Write a balanced equation for this reaction (b) If it took 23.60 mL of NaOH to neutralize 25.00 mL of 0.1110 M HCl, what is the molarity of the NaOH solution? 5. How many grams of NaOH are needed to prepare 1.00 liter of 0.100 M NaOH solution?
Shaiju T.
(b) A 25.00 mL aliquot of KHP prepared in (a) required 23.85 mL of NaOH solution to reach the end point during titration (i) Write a balanced equation of the reaction [2] (ii) What is the exact concentration in moles/Litre of your NaOH solution? [1] (iii) Which one between KHP and NaOH is the primary standard and why? [2] (iv) Which indicator is suitable for a weak-acid strong-base titration and why? [2] (c) Suppose we titrate 20mL of 0.100M HCHO2 with 0.100M NaOH. Calculate the pH: (i) Before any base is added. [3] (ii) When half of the HCHO2 has been neutralized. [3] (iii) After a total of 15.0mL of base has been added. [3] Hint: Read Brown and Lemay (Topic: acid and base equilibrium) The dissociation constant for formic acid is, Ka = 1.8 x 10-4
Sri K.
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