Questions 1. Calculate the molarity of a sodium hydroxide (NaOH) solution that is titrated with 0.6887 g of oxalic acid (Equation 2). The titration requires 15.80 mL of the NaOH solution to reach the end point. 2. Calculate the molarity of a sulfuric acid (H2SO4) solution if 30.10 mL of 0.6210 M NaOH is required to reach the end point when titrated against 10.00 mL of the unknown acid solution. The balanced chemical equation for the reaction is given below. (Refer to Example 2 for help with calculations). H2SO4(aq) + 2 NaOH(aq) ? Na2SO4(aq) + 2 H2O(l)
Added by Virginia V.
Close
Step 1
The molar mass of oxalic acid is: Molar mass of H2C2O4 = 2(1.01) + 2(12.01) + 4(16.00) = 90.04 g/mol Now, we can find the moles of oxalic acid: Moles of H2C2O4 = (0.6887 g) / (90.04 g/mol) = 0.00765 mol The balanced chemical equation for the reaction between Show more…
Show all steps
Your feedback will help us improve your experience
Oluwapelumi Kolawole and 84 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Sodium Hydroxide reacts with sulfuric acid. 2 NaOH(aq) + H2SO4(aq) ----> Na2SO4(aq) + 2 H2O A flask contains 25.00 mL of H2SO4(aq) of unknown concentration. Titration of the sample requires 25.20 mL of 0.1000 M NaOH(aq) for neutralization. What is the molarity of the sulfuric acid solution? Sodium hydroxide reacts with hydrochloric acid. NaOH(aq) + HCl(aq) ----> NaCl(aq) + H2O A flask contains 20.00 mL of 0.1030 M HCl. What volume of 0.2010 M NaOH must be added to just neutralize the acid? Hint: MaVa = MbVb
Suman K.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD