In a different titration experiment, it took 23.95 mL of a 0.175 M solution of NaOH to titrate 20.00 mL of an unknown HCI solution. Calculate the molarity of the HCI solution. HCl(aq) + NaOH(aq) →→→ NaCl (aq) + H₂O (1)
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- ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELLA 25.00 mL sample of vinegar (acetic acid) was titrated with the same 0.300 M NaOH from the previous question. 41.68 mL of the 0.300 M NaOH solution was required to reach the endpoint of the titration. The balanced equation below can help you answer these questions. HC2H3O2(aq) + NaOH(aq) --> NaC2H3O2(aq) + H2O(l) Part A: How many Liters of NaOH were dispensed from the buret?In a different titration experiment, it took 23.96 mL of a 0.105 M solution of NaOH to titrate 20.00 mL of an unknown HCl solution. Calculate the molarity of the HCl solution. HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l)
- An analytical chemist weighs out 0.045 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 0.1800 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 4.2 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 molConsider a buffer solution that consists of two separate components: the weak acid, CH3COOH(aq), and its conjugate base, CH3COO¯ (aq) (added as NaCH3COO). Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution. Which component will react with OH-(aq) from a strong base? Write the net ionic equation for the reaction that occurs when OH-(aq) is added to the buffered solution.1.15 g of an unknown triprotic acid (H3A) is titrated with 2.50 M KOH. It takes 35.5 mL of KOH to reach the equivalence point of the titration. Calculate the molar mass of the unknown acid. H3A (aq) + 3 KOH (aq) → 3 H2O (l) + K3A (aq)
- A chemistry graduate student is given 125. mL of a 0.80M ammonia (NH3) solution. Ammonia is a weak base with K₂ = 1.8 × 10. What mass of NHÂBr should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.55? 4 You may assume that the volume of the solution doesn't change when the NH Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 0 x10 × SAn analytical chemist weighs out 0.275 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0500M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 73.3 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol x10 X SAn analytical chemist weighs out 0.099 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 0.1400 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 12.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. 1 g mol Explanation Check 3 80 Xx 4 888 S 5 F MacBook Air 6 Fa 33 5 ?圖□ 圆图 ( oll Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessil Ar
- The NaOH solution was standardized using the following system. The balanced neutralization reaction is 2 NaOH(aq) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) Three flasks containing 25.00 mL H2SO4 each was titrated with NaOH. The standard sulfuric acid concentration is 0.150M. The data is below: Titration 1 Titration 2 Titration 3 Starting volume buret 1.10 mL 24.56 mL 1.76 mL Buret volume at end 24.34 mL 47.52 mL 24.86 mL a. Calculate the volume of NaOH that was added in each titration. b. Determine the average volume of NaOH added among the three trials. c. What was the concentration of NaOH?This is another titration question. When 35.00 ml of phosphoric acid of unknown concentration is titrated with 1.025 M NaOH, and 18.75 ml of NaOH is required to reach the endpoint, what is the molarity of the phosphoric acid? The reaction is: H3PO4 (aq) + 3 NaOH (aq) → Na3PO4 (aq) + 3 H2O (l)A student is conducting a titration between a weak, monoprotic acid and sodium hydroxide, NaOH. The student titrates 20.0 mL of the weak acid with 0.300 M sodium hydroxide, NaOH(aq). When 5.00 mL of NaOH(aq) has been delivered the pH of the weak acid is 5.328. Determine the Ka of the weak acid.