Rugort Sbeet Titration of Acids and Base Average percent of KHP Calculations of
ID: 542133 • Letter: R
Question
Rugort Sbeet Titration of Acids and Base Average percent of KHP Calculations of percent KHP and standard deviation (show using equations with units): Standard deviation QUESTIONS rite the balanced chemical equation for the reaction of KHP with NaOH 2. Suppose your laboratory instructor inadvertently gave you a sample of KHP contaminated with NaCI to use in standardizing your NaOH. How would this affect the molarity you calculated for your NaOH solu- tion? Justify your answer 3. How many grams of NaOH are needed to prepare 500 mL of 0.125 MNaOH? 4. A solution of malonic acid, H,C,H204, was standardized by titration with 0.1000 M NaOH solution. I 20.76 mL of the NaOH solution is required to neutralize completely 13.15 mL of the malonic acid solu- tion, what is the molarity of the malonic acid solution? y you used KHP in this experiment. In such a standardizatiou, it was found that a 0.512 g sample of sodium carbonate quíred 25.3 mL of a sulfuric acid solution to reach the end point for the reaction. 5. Sodium carbonate is a reagent that may be used to standardize acids in the same wa NaCO, (ag)+H,SO (og)H,0+00(8)+Na,SO,(ag)Explanation / Answer
The reaction between an acid and base produces a salt and water, in this reaction the acid is potassium hydrogen phthalate (KHP), and the base is sodium hydroxide (NaOH).
Balanced equation is as below
NaOH(aq) + KHC8H4O4(aq) = KNaC8H4O4(aq) + H2O(l)
Here salt formed is potassium sodium phthalate.
2)
NaCl in KHP doesn't effect above reaction. But it alter the molarity of standard KHP.
The prepared standard has less molarity than calculated.So more volume is required to neutralize NaOH.So molarity of NaOH will be higher than actual value.
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