Data Table for Unknown # 8 1 Mass of unknown ammonium salt 2 Molarity of NaOH(aq), M2 3 Molarity of HCl(aq), M1 4 Volume of NaOH(aq) measured For back-titration 5 Initial Volume of HCl(aq) used Final Volume of HCl(aq) used 6 7 Volume of HCl(aq) used, V1 End Point (Color Change) 8 Trial 1 0.400g 0.1938 M 0.1942 M 50.00mL OmL Trial 2 0.415g 0.1938 M 0.1942 M 50.00mL 23.00mL 42.80mL 50.00ml 23.00mL 50.00mL blue green → Yellow Trial 3 0.403g 0.1938 M 0.1942 M 50.00mL OmL 20.80mL 50.00mL

Use the References to access important values if needed for this question. An aqueous solution contains 0.367 M hypochlorous acid. How many mL of 0.224 M potassium hydroxide would have to be added to 125 mL of this solution in order to prepare a buffer with a pH of 7.300? Submit Answer Retry Entire Group mL 8 more group attempts remaining Pravious Email Instructor Next> Save and Exit

The experimental procedure above was used to generate the data in the tables below. Data Collection Table Titration    Mass of Sample       Initial Buret Reading (mL)        Final Buret Reading (mL) 1                1.234                               1.05                                       19.95 2                1.213                                4.00                                      23.50 3                 1.273                               0.30                                    20.05 4                 1.292                             5.95                                       25.65 - For each titration, calculate: - The number of moles of potassium permanganate used in the titration (H x L of KMnO4) - The number of moles of iron present in the sample (stoichiometry in balanced equation) - The percentage by mass of iron in the solid sample (Equation 1) - The average mass % of iron in your unknown - The standard deviation in your % Fe results:

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help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

9.4 mL of 2.4 M HCI is used to titrate 12.6 mL of NH3 its endpoint. What is the initial molar concentration of the NH3? answer to two significant figures.

Please correct answer and don't use hend raiting

Describe the information necessary (and why) to choose a good indicator for a weak acid/strong base titration. Answer:

[Review Topics] [References] Use the References to access important values if needed for this question. An aqueous solution contains 0.370 M acetic acid. How many mL of 0.361 M sodium hydroxide would have to be added to 150 mL of this solution in order to prepare a buffer with a pH of 4.400? Submit Answer Retry Entire Group mL 7 more group attempts remaining Previous Email Instructor Naxt Save and Exit

Solve correctly please. (Gpt/Ai wrong answer not allowed)