Write the balanced chemical equation for the reaction of KHP with NaOH. Suppose your laboratory instructor inadvertently gave you a sample of KHP contaminated with NaCl to standardize 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 0.100 M NaOH solution. If 21.82 mL of the NaOH solution were required to neutralize completely 12.12 mL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4 + 2NaOH rightarrow Na2C3H2O4 + 2H2O Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. In such a standardization it was found that a 0.432-g sample of sodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point for the reaction. Na2CO3(aq) + H2SO4(aq) rightarrow H2O(l) + CO2(g) + Na2SO4(aq) What is the molarity of the H2SO4? A solution contains 0.252 g of oxalic acid, H2C2O4. 2H2O, in 500 mL. What is the molarity of this solution?
