A 0.860 −g sample of an unknown acid requires 33.0 mL of a 0.190 M barium hydroxide solution for neutralization. |
Part A Assuming the acid is diprotic, calculate the molar mass of the acid.
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A 0.860 −g sample of an unknown acid requires 33.0 mL of a 0.190 M barium...
A 0.864 −g sample of an unknown acid requires 32.7 mL of a 0.183 M barium hydroxide solution for neutralization. Assuming the acid is diprotic, calculate the molar mass of the acid.
2. A 0.2349 g sample of an unknown acid requires 33.66 mL of 0.1086 M NaOH for neutralization to a phenolphthalein end point. There are 0.42 mL of 0.1049 M HCI used for back-titration. a. How many moles of OH- are used? moles OH moles H b. How many moles of H+ from HCI? moles H c. How many moles of H+ are there ins solid acid? (Eq. 5) g/mol d. What is the molar mass of the unknown acid?...
A 0.767 g sample of a monoprotic acid is dissolved in water and titrated with 0.190 M KOH. What is the molar mass of the acid if 32.0 mL of the KOH solution is required to neutralize the sample? molar mass: g/mol
3. A 0.7026 g sample of an unknown acid requires 40.96 mL of 0.1158 M NaOH for neutralization to a phenolphthalein end point. There are 1.22 mL of 0.1036 M HCl used for back-titration. a. How many moles of OH are used? How many moles of Ht from HCI? moles OH moles H+ b. How many moles of Ht are there in the solid acid? (Use Eq. 5.) moles H+ in solid c. What is the molar mass of the...
(A) A 14.5 g sample of an aqueous solution of hydrobromic acid contains an unknown amount of the acid. If 26.8 mL of 0.557 M barium hydroxide are required to neutralize the hydrobromic acid, what is the percent by mass of hydrobromic acid in the mixture? (B) A 13.7 g sample of an aqueous solution of nitric acid contains an unknown amount of the acid. If 19.8 mL of 0.682 M potassium hydroxide are required to neutralize the nitric acid,...
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22. A 0.670 g sample of an unknown diprotic acid required 25.00 mL of 0.160 M NaOH to titrate it. What is the molar mass (g mol-') of unknown acid? A. 0.167 g mol-' B. 335 g mol-' C. 180. g mol-' D. 167.5 g mol' E. 0.335 g mol-'
A 0.4352-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized potassium hydroxide. The equivalence point in the titration is reached after the addition of 31.14 mL of 0.1833 M potassium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid. _____ g/mol
Given a .210 g sample of a diprotic acid of unknown molar mass: If the acid is dissolved in water and titrated with .241 M KOH it takes 10.5 mL of base to reach the equivalence point. What is the molar mass of the solution?
A 1.53 gram sample of an unknown monoprotic acid is dissolved in 25.0 mL of water and titrated with a a 0.234 M aqueous barium hydroxide solution. It is observed that after 16.3 milliliters of barium hydroxide have been added, the pH is 4.924 and that an additional 10.0 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol (2) What is the value of Ka for the...
A 1.48 gram sample of an unknown monoprotic acid is dissolved in 30.0 mL of water and titrated with a a 0.291 M aqueous barium hydroxide solution. It is observed that after 7.15 milliliters of barium hydroxide have been added, the pH is 9.104 and that an additional 13.2 mL of the barium hydroxide solution is required to reach the equivalence point. (1) What is the molecular weight of the acid? g/mol 2) What is the value of K_a for...