An analytical chemist weighs out  0.149g  of an unknown diprotic acid into a  250mL  volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with  0.1400M   NaOH  solution. When the titration reaches the equivalence point, the chemist finds he has added  12.8mL  of  NaOH  solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.

An analytical chemist weighs out 0.406 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 34.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. C mol Explanation Recheck JAHE B! F2 # 3 80 F3 X $ 4 888 F4 S % LO 5 F5 MacBook Air A 2 F6 & 7 F7 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc * ∞ DII F8 9 FO A F10 4 F11

A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to HCl. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.20 ml of 0.100M NaOH? Select one:a. 9.80b. 10.26c. 9.90d. 11.08

An approximately 0.1 M NaOH solution is made by adding 4.0 g of solid NaOH to 1000 mL of water. The precise concentration of the solution is determined by titrating the NaOH against portions of a weak acid, potassium acid phthalate (KHP) obtained from the National Bureau of Standards and certified as being 99.99% pure. The KHP samples are weighed by difference on a balance. How would the calculated NaOH concentration be affected (in comparison with the true concentration), if: (does it become greater, smaller, or unchanged) 1. The KHP was not dried prior to weighing? 2. The balance always read high, but in proportion to the weight recorded?

please put the correct amount of sig figs

Calculate the molar mass of the unknown acid from the information below.

If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being titrated was 75 ml, then what is the unknown concentration of the oxalic acid in this titration. The volume of NaOH is 29ml.

An analytical chemist weighs out 0.026 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 3.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol

A 24.5 mL sample of vinegar is titrated with 0.451 M NaOH(aq). If the titration requires 33.0 mL of NaOH(aq) to reach the equivalence point, what is the concentration of acetic acid in the vinegar? Submit M Submit and Next Mark this question for later review.

An analytical chemist weighs out 0.318 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 82.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol x10 x 3