A 0.298 g sample of an unknown monoprotic acid is titrated with 0.300 M KOH to the equivalence point. It requires 15.8 mL of KOH to reach this point. Elemental analysis is also performed, showing that the acid contains 1.6% H, 22.2% N, and 76.2% O. Use this information to determine the molecular formula and the molar mass of the unknown acid. molecular formula of unknown acid: HNO molar mass of unknown acid: Draw the Lewis structure of the unknown acid in which the H atom(s) are bonded to O atom(s). g/mol

A solution of a weak acid is titrated with a standard solution of a strong base. The progress of the titration is followed with a pH meter. Which of the following observations best describes what would occur? Initially the pH of the solution increases slowly, and then it increases much more rapidly, before increasing slowly again At the equivalence point, the pH is 7 The pH of the solution gradually decreases throughout the experiment After the equivalence point, the pH becomes constant because this is the buffer

Please only answer the question below. The questions shown are already solved, you don’t need to add anything, they are there for context. 3) Calculate the [Ba2+] left in solution when Ca2+ starts to precipitate. Then calculate the % of the original Ba2+ left in solution when Ca2+ starts to precipitate. A) 1.1 • 10^-2 % B) 2.8 • 10^-7 % C) 9.3 • 10^-3 % D) 6.7 • 10^-3 % E) 5.6 • 10^-3 %

theoretically, the equivalence point and end point of a titration should be the same. Describe four factors that could be responsible for the difference between these two in an actual titration

Question 6 (1 point) 14 12 10 8 PH 00 6 4 2 0 0 20 40 60 volume added (mL) Consider the graph. What type of titration does it represent? A strong base titrated with a strong acid. A weak acid titrated with a strong base. A weak base titrated with a strong acid. A strong acid titrated with a strong base.

(Answer highlighted questions please) A 50.050.0 mL solution of 0.1390.139 M KOHKOH is titrated with 0.2780.278 M HClHCl. Calculate the pH of the solution after the addition of each of the given amounts of HClHCl. 20.0 mLpH=20.0 mLpH=     24.0 mLpH=24.0 mLpH=     25.0 mLpH=25.0 mLpH=

Select ALL of the following that can be determined from the titration of a strong, monoprotic acid with a standardized solution of sodium hydroxide? moles of acid in the titration moles of hydroxide ions used in the titration mass of acid titrated | volume of sodium hydroxide used in the titration Select ALL of the following quantities that must be used in a titration calculation to find the identity of an unknown strong acid: concentration of the standardized base solution stoichiometric ratio of acid to base volume of the acid solution used in the titration volume of the base used in the titration at the equivalence point Need Help?

A 0.338-g sample of an unknown triprotic acid is titrated to the third equivalence point using 33.4 mL of 0.163M NaOH. Calculate the molar mass of the acid.     Question 1 options:   A)  5.44 g/mol   B)  1.86× 102 g/mol   C)  20.7 g/mol   D)  69.3 g/mol   E)  62.1 g/mol

3. A 0.3535 g sample of KHP requires 19.27 mL of NaOH to reach the end point. What is the concentration of NaOH? 4. What properties should the indicator have for titration of KHP with NaOH?

Regarding titrations, which of the following is TRUE? A plot of pH vs. the [base]/[acid] ratio is known as a titration curve. The equivalence point is when the moles of base equals the moles of acid during any acid–base titration. Indicators do not respond to changes in pH. The pH is always 7 once the equivalence volume has been delivered. None of the answers are true.