Volume NaOH (added). pH of analyte 0.00 mL _1.00 10.00 mL 1.23 20.00 mL _1.54 30.00 mL _2.20 _33.33__ mL (at equivalence point) _5.22 35.00 mL _11.46 40.00 mL _12.04_ 9. Sketch your pH curve below. Place the pH on the y-axis and volume of NaOH added on the x-axis.
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- BONUS: During a titration, ammonia is added to the flask and titrated with HCI. Looking at the titration below and the indicator table, what would be a good indicator to use for this experiment? What color change would be observed? 12 10 20 40 60 80 100 120 140 mL d.1 M HCI TABLE 16.7 Common Acid-Base Indicators Approximate pH Range over which the Color Changes Color Change Gower to higher pH) Indicator Thymol blue Micdni otanpr 3234 Filyl d Mechyl purple Broeno purpkpH Measurement Experiment 1. Objectives: Explore different methods of measuring ph II. Materials: water window cleaner pH meter apple juice 0.1 M NaCl pH paper milk 0.1 M FeCl₂ litmus paper red/blue III. Results and Observations Red litmus paper water apple juice milk window cleaner 0.1 M NaCl 0.1 M FeCl3 IV. Conclusion Blue litmus paper Acidic/basic/neutral PHInterpret pH titration plots. Answer the following about the titration plot shown below, involving a monoprotic acid and base. 20 mL of 0.1M titrand titrated with 0.1M titrant. Data points at 1 mL increments. 14.0 12.0 10.0 5 8.0 6.0 4.0 2.0 0.0 seededood 0 0.0 10.0 مهمه 20.0 30.0 Volume of titrant (mL) (a) Is the species being titrated an acid or a base? (b) Is the species being titrated strong or weak? (c) What is the value of Ka (if a weak acid) or K, (if a weak base) for the species being titrated? If the species is strong (100% dissociated), enter 999. rààààààààà 40.0 50.0
- The pH of the standard solution were measured with a pH meter three times and the following data were obtained: 6.98, 7.20, and 7.22. If the pH of the standard solution is 7.00, this pH meter would provide the correct results at the 95% confidence level. Is this statement true or false? True FalseGiven the following titration curve answer questions 4-6. Make sure your mark on the graph the volume at the equivalence point, the pH at the equivalence point, the volume where the pH=pKa, and the value for the pKa. 15.00 14.00 13.00 12.00 11.00 10.00 9.00 8.00 pH 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 4 8 12 16 20 24 28 32 36 40 44 48 52 56 60 Volume of Titrant (mL) The above titration curve was obtained when a 10.00 mL sample of a 0.50 M base was titrated with an acid. 4. What is the approximate molarity of the acid (the titrant) used?In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?
- A 0.1-L unbuffered solution needs the pH adjusted from 6.8 to 2. How many microliters of a 6 molar HCI solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: • Assume the volume of HCI being added is negligible and the total volume of the solution does not change. • The volume of the solution is *not* 1 L like it was in the practice pools. • The question requests your answer be reported in uL (microliters)!Suppose a student wants to determine the color change interval of an unknown indicator. Her results are given in the table. Tube # pH Unknown indicator 4 6.39 red 7.11 red 6. 7.87 purple 7 8.81 purple 8. 9.07 blue 9 10.10 blue What is the interval of the unknown indicator? The color change interval is between pH 7.11 and pH 7.87. The color change interval is between pH 7.11 and pH 9.07. The color change interval is between pH 9.07 and pH 10.10. The color change interval is between pH 6.39 and pH 10.10. O OII. Titrating HCI Solution with NaOH Solution 1. Prepare a titration curve. Plot pH (on the y-axis) versus volume of NaOH solution added (on the x-axis). If your initial buret reading was not 0.00 mL, remember to subtract your actual initial reading from each of your subsequent buret readings before plotting the titration data.
- DATA Mass of NaCl needed for 50.0 mL of 0.200 M NaCl solution 0.5 (Show calculation below.) 50.OMLX1000 =0.05 0.01K354305844 Initial pH pH after addition of Change in pH from initial pH after addition of Change in pH from initial strong acid strong base 7.05/245 4.01181 173 7.09/2447-4102/11.89 4102/45(6 10.75(0.70 Water 0.200 M NaCl acetate FO.0104.10 008 -0.0011682/1 O.84 buffer phosphate bufferFact: The pH indicator Alizarin Yellow has a pH range of 10.0 (yellow) to 12.0 (red). Question: You added 8 drops of Alizarin Yellow indicator to 50 mL of distilled water and your solution appears yellow and transparent. What colour would your solution change to if you added 20 drops of 2.0 M NAOH? Think about what you did in the lab. Remember the results are reported on going from acid to base. O Your solution would turn red in colour and would be transparent (see through). O None of these answers are correct. Your solution would become colourless. OYour solution would remain yellow in colour and would be transparent (see through). Your solution would turn orange in colour and would be transparent (see through).Exactly 24.57 mL of 0.045 M strong acid is added to a 25.00 mL sample of a 0.044 M weak base solution. What is the pH at this point in the titration? Ky for the base is 4.62x10-4. REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS. Type your answer...