- Suppose your laboratory instructor inadvertently gave you a sample of KHP contaminated with NaCl to use in standardizing your NaOH. How would this affect the molarity you calculated for your NaOH solution? Justify your answer.
- A solution of malonic acid, H2C3H2O4, was standardized by titration with 0.1000 M NaOH solution. If 20.76
mL of the NaOH solution is required to neutralize completely 12.95 mL of the malonic acid solution, what is the molarity of the malonic acid solution? - A solution contains 6.30 × 10−2g of oxalic acid, H2C2O4 ∙ 2H2O, in 250 mL. What is the molarity of this solution?
- The titration of an impure sample of KHP found that 26.00 mL of 0.100 M NaOH was required to react completely with 0.700 g of sample. What is the percentage of KHP in the sample?
- Suppose that unknowingly to you, Ba(OH)2 was used instead of NaOH for the titration. How would this affect the percent of unknown acid?
- If unknown to the student, there was an error on the balance and the actual mass of KHP was 1.017g, how would this error affect the calculation of the Molarity of an unknown acid?
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